Chemistry Questions and Answers August 02, 2020

Determine the number of valence electrons for each of thefollowing four elements. Part A Ga _______ Express your answer as an integer. Part B Pb ________ Express your answer as an integer. Part C Cl ___________ Express your answer as an integer. Part D N _____________ Express your answer as an integer. Part E Which elements do you expect to lose

Calculate the root mean square velocity of F2,Cl2, and Br2 at294 K . Calculate the kinetic energy of F2,Cl2, and Br2 at 294 KRank the three halogens with respect to their rate of effusion.Rank the three halogens with respect to their rate of effusion.Cl2>F2>Br2 F2>Cl2>Br2 Br2>Cl2>F2F2>Br2>Cl2

a) The dipole moment of HBr is 0.80D. Whatis the dipole moment of HBr in C?m? (answer= 2.67 x10^-30 c x m) b) The distance between the atomsof H?Br is 1.41. What is the distance inmeters? c) What is the charge associated with each side ofthe HBr molecule? d) What is the percent ionic character ofthe H?Br bond?

In this experiment iodination of salicylamide was performed inwhich 0.250g of salicylamide was used and 0.3g of sodium Iodide(NaI) and 9.2mL of sodium Hypochlorite was used. How do I calculatethe percent yield? Salicylamide Molarmass = 137.138 g/mol Sodium Iodide Molar Mass = 149.89 g/mol and Density = 3.67g/cm3

Draw the structure of the compound that is consistent with the H NMR data below. (Assume that longrange coupling is not observed.) Suggestion Find end groups (like methyls) and work as far as possible towards the middle When neighboring hydrogens are unequal, the splitting gets quite complex and multiplets result. This is especially true if a

The density of a 0.438 M solution of potassium chromate (K2CrO4) at 298 K is 1.063 g/mL. Calculate the vapor pressure of water above the solution. The vapor pressure of pure water at this temperature is 0.0313 atm. Assume complete dissociation. Pvap = ________atm

Draw the structure of the starting material in the ozonolysis reaction below. Hint: The starting material and product have the same number of carbons (i.e., 1 mol reactant : 1 mol product.

1.) 03, CH2C12 2.) (CH3)2S H

Which changes are evidence of a chemical reaction? Drag each item to the appropriate bin. Help Reset A beaker of water becomes cool to the touch upon adding a saltto it. A cloudy solution becomes clear upon adding another solution toit. Bubble formation on chalk added to acid Water condensing Bubbles forming in a shaken water bottle Evidence Not

Determine the average rate of change of B from t = 0 to t =222. A -------> 2B Time (s) Concentration of A [M] 0 0.660 111 0.420 222 0.180 PLEASE SHOW WORK

Determine whether each of these processes is reversible orirreversible. Drag the appropriate items to their respective bins. Bins: Reversible and Irreversible 1) solid melting infinitesimally slowly at its melting point 2) a single swing of a real pendulum 3) gas condensing infinitesimally slowly at its condensationpoint 4) solid melting

The data below were collected for the following reaction at 500?C: CH3CN(g)?CH3NC(g) Time (h) [CH3CN] (M) 0.0 1.000 5.0 0.794 10.0 0.631 15.0 0.501 20.0 0.398 25.0 0.316 Determine the order of the reaction at this temperature. What isthe half-life for this reaction (at the initial concentration)? Howlong will it take for 80% of the CH3CN to

Which equation is an expression of the second law ofthermodynamics for a spontaneous process? 1) ?H univ = ?H sys + ?H surr < 0 2) ?S univ = ?S sys + ?S surr < 0 3) ?S univ = ?S sys + ?S surr = 0 4) ?S univ = ?S sys + ?S surr > 0

Determine theelectron geometry (eg) and molecular geometry (mg) ofNCl 3 . Is it: A,B,C,D, or E below? A) eg = tetrahedral,mg = trigonal pyramidal B) eg = linear, mg =trigonal planar C) eg = trigonalplanar, mg = bent D) eg = linear, mg =linear E) eg = tetrahedral,mg = tetrahedral

Draw a condensed structure forCH 3 C(CH 3 ) 2 CH 2 CH 2 CH(CH 3 )CH 3 . Draw a condensed structure forCH 3 CH(CH 3 )CH(CH 2 CH 3 )CH(CH 2 CH 3 )CH 2 CH 2 CH 3 .

Part A Which of the following best describes the side chain of argin in eat a pH of 11? non-polar uncharged but polar charged and polar aprotic hydrophobic Charged and polar is incorrect. My textbook says the pKa of the side chain is 12.48. Can you please explain what the correct answer is?

Consider the following unbalanced redox reaction. Cr2027(aq) Cu(s)Cr3(aq)Cu2 (aq) Part A Balance the equation aCr2027(aq)BH(aq)yCu(s)5Cr3(aq)cH2O(kCu2 (aq) Give your answer as an ordered set of numbers a, , y, ... Use the least possible integers for the coefficients. a, , V, 5, E, K 1,14,3,2,7,3 ANSWER

Determine the OH- of a solution that is 0.180M in F-. What is the pH? I keep getting the wrong answer! Do I need the Ka of HF?

Draw the organic product of the following reaction between (1S,3S)-1-chloro-3-methylcyclopentane and methanethiol in the presence of sodium hydroxide. Show any H's on chirality centers, if applicable, and use wedge-and-dash bonds.

H will anall S, S R, R R, S Chiral Racemic Achiral Cl SH NaOH Also, Select all that apply The product of the reaction is characterized as being

Consider the following set of reactions: N2 + 2O2?N2O4 ,? H =?8 kJ/mol N2 + O2?2NO ,? H =180 kJ/mol The equations given in the problem introduction can be addedtogether to give the following reaction: overall: N2O4?2NO + O2 However, one of them must be reversed, reaction1: N2 + 2O2?N2O4 What is the enthalpy for reaction 1 reversed? reaction 1

Determine which of the following pairs of reactants will result in a spontaneous reaction at 25C. Fe3+(aq) +Al(s) Pb2+(aq) + Au(s) Na+(aq) + Cr(s) Ag+(aq) + Br(aq) None of the above pairs will react.

Calculate the standard cell potential for each of the following electrochemical cells. You may want to reference (Pages 854861) Section 19.4 while completing this problem. Part A Ni (aq) Mg(s)Ni(s) Mg(aq) Express your answer in volts using two decimal places. Excell Submit Part B Incorrect Try Again 14 attempts remaining Ecell Submit 17 Ni (s)

A chemist designs a galvanic cell that uses these two halfreactions halfreaction N(9)4HO(1)4e Answer the following questions about this cell. Write a balanced equation for the halfreaction that 0 happens at the cathode. Write a balanced equation for the halfreaction that happens at the anode. Write a balanced equation for the overall reaction that

select the reaction which Kp=Kc

P4 (s) 10Cl (g) 4PCl, (g) S(s) 3F (g) SF6 (g) CaCO3(s) Ca0(s) CO(g) 2SO(g) O(g) 2S03(g) Fe3O4(s) 4H(g) 3Fe(s) 4HO(g) 2HS(g) 2H(g) S(g) N(g) 3H(g) 2NH3(g) Fe0(s) CO(g) Fe(s) CO(g) N04 (9) 2NO(g) 2KCIO3(s) 2KCI(s) 30(g) 2CO(g) O(g) 2C0(g) 2BrCl(g) Br(g) Cl(g)

Now consider the following set of reactions: N2 + 2O2->N2O4 ,delta H =-8 kJ/mol N2 + O2->2NO , delta H =180 kJ/mol What is the enthalpy for the following reaction? overall:N2O4->2NO + O2 Express your answer numerically in kilojoules permole.

Show that there is an existance of

1) The existance of HISTIDINE at pH 4 is NH3 A) HC NH HN C) 00C N NH3 NH B) OOC HN D) OOC NH3 NH NH NH

Now consider the following set of reactions: 2NO2?2NO + O2 ,? H =109 kJ/mol N2O4?2NO + O2 ,? H =172 kJ/mol Part A The equations given in the problem introduction can be addedtogether to give the following reaction: overall: N2O4?2NO2 However, one of them must be reversed. Which one? reaction 1: 2NO2?2NO + O2 reaction 2: N2O4?2NO + O2 Part B What

Consider the following reaction occurring at 298 K:N2O(g)+NO2(g)?3NO(g) Part A Show that the reaction is not spontaneous under standard conditions by calculating ? Part B If a reaction mixture contains only N2O and NO2 at partial pressures of 1.0 atm each, the reaction will be spontaneous until some NO forms in the mixture. What maximum partial

How does a buffer resist change in pH upon addition of a strong acid The strong acid reacts with the weak base in the buffer to form a weak acid, which produces few H ions in solution and therefore only a little change in pH. The strong acid reacts with the weak acid in the buffer to form a weak base, which produces few H ions in solution and

Determine the average rate of change of B from t=0 s to t=202s. A --> 2B Time (s) Concentration of A(M) 0 0.640 101 0.380 202 0.120 Answer in M/s. Show work and explain

For the equilibrium Br2( g )+Cl2( g )?2BrCl( g ) at 400 K, K c = 7.0. Part A If 0.25 mol of Br2 and0.55 mol of Cl2 are introduced into a3.0-L container at 400 K, what will be the equilibriumconcentration of Br2? Express your answer to two significant figures and include theappropriate units. Part B If 0.25 mol of Br2 and0.55 mol of Cl2 are

Consider these two entries from a fictional table of standardreduction potentials. X2+ + 2e- => X(s) E=1.85 V Y2+ + 2e- => Y(s) E=0.39 V Which pair of species would react under standard conditions? _X and Y2+ _X2+ and Y _X2+ and Y2+ _X and Y

classify the species given below by the intermolecular forcespresent in a pure sample of each: Ar H2 HCN HF BrCl5 NH3 CH3OH H2S PF5 CH2Cl2 are they dispersion, dipole-dipole, or h bond?

Consider teh following structure H2C=O. What is the hybridization of the carbon atom? What is the H-C-O bond angle? What is the functional group? What orbitals overlap in the C-H bonds?

Here is the chemical reaction that represents solid leadchloride dissolving in water: PbCl2(s) ?Pb2+(aq)+2Cl?(aq) Ksp =1.210?5 Part A Which of the following actions would shift this reaction towardsolid lead chloride? Add more lead chloride. Add more chloride ions. Remove chloride ions. Remove lead ions.

calculate the equilibrium constant (kc) for the reaction at this temperature. co(g)+2h2(g)->ch3oh(g). a reaction mixture in a 5.16L flask at a certain temperature initially contains 27.3g co and 2.33g h2. at equilibrium the flask contains 8.64g ch3oh

Calculate E ?cell for each of the followingbalanced redox reactions. PartA: O2(g)+2H2O(l)+4Ag(s) ? 4OH?(aq)+4Ag+(aq) PartB: Br2(l) + 2I?(aq) ? 2Br?(aq) + I2(s) Part C: PbO2(s)+4H+(aq)+Sn(s)?Pb2+(aq)+2H2O(l)+Sn2+(aq) Part D: Which of thereactions are spontaneous as written. Check all that apply PbO2(s)+4H+(aq)+Sn(s)?Pb2+(aq)+H2O(l)+Sn2+(aq)

Classify the following complex ions as high spin or low spin: 1) [ Fe (CN)6 ] 4- no unpaired e- 2) [ Fe (CN)6 ] 4- one unpaired e- 3) [ Co (NH3) 6 ] 2+ three unpaired e-'s 4) [ Co F6 ] 3- four unpaired e-'s 5) [ Mn (H2O) 6 ] 2+ five unpaired e-'s

Choose the thermochemical equation that illustrates H 0 f forLi 2 SO 4 . H 2 S ( g) + 3O 2 (g) <=> 3H 2 O(g) + SO 2 (g) 8 Li 2 SO 4 (s) ----- > 16 Li(s) + S 8 (s,rhombic) + 16 O 2 Li 2 SO 4 (aq) ----- > 2Li + (aq) + SO 4 2- (aq) 2Li (s) + 1/8 S 8 (s,rhombic + 2 O 2 ------ >Li 2 SO 4 (s) 2 Li + (aq) + SO 4 2- (aq) -----> Li 2 SO 4

Choose the situation below that would result in an endothermic?H solution . When < When > When is close to When >> There isn't enough information to determine. Choose the situation below that would result in an exothermic?H solution . When < When >> When > When is close to There isn't enough information to determine. A

The equilibrium reaction CaCO3(s) ? CaO(s) + CO2(g) reaches ?G= 0 at 835C. At this temperature: the pressure of CO2 is 1 atm thepercent yield of CaO reaches 100% ?H = ?S the decomposition ofCaCO3 begins the reaction becomes exothermic

What is the charge of the common ion formed by each of theseatoms? Either -2,-1,+1, or +2. S, Br, I, Li, Sr, Mg, Na, Cs, Ba, F, and O How are these changes found?

An electrochemical cell has a positive standard cell potentialbut a negative cell potential. what must be true of Q and Kfor the cell? (choose one and please explain why you chose thatletter.) a.) K>1; Q>K b.) K<1; Q>K c.) K>1; Q d.) K<1; Q

Enter a balanced equation for the dissolution of CaCO3. Expressyour answer as a chemical equation. Identify all of the phases inyour answer. I tried to put CaCO3(s)?Ca+2(aq)+CO3?2 (but it doesnt work) Enter a balanced equation for the dissolution of AgI. Expressyour answer as a chemical equation. Identify all of the phases inyour answer. Enter a

Balance each of the following redox reactions occurring inacidic aqueous solution. art A K( s )+Cr3+( a q )?Cr( s )+K+( a q ) Express your answer as a chemical equation. Identify all of thephases in your answer. Submit My Answers Give Up Part B Cd( s )+Cu+( a q )?Cd2+( a q )+Cu( s ) Express your answer as a chemical equation. Identify all of

Which choice is a pair of isomers? 1. H_2NCH_2CH_3 and CH_3CH_2NH_2 2. CH_3CH_2CH_2OH and CH_3CH_2OCH_2CH_3 3. ethanol and propene 4. 1-butene and 2-methylpropane 5. CH_3CH_2CH_2CH_2CH_3 and CH_3CH_2CH(CH_3)_2 **THE DASHES ARE JUST TO INDICATE THAT THE NUMBER IS A SUBSCRIPT (BELOW THE

Draw the structure of NO 3 - . Include all lone pairs of electronsand formal charges. Draw the structure of CO 3 2 - . Include all lone pairs ofelectrons and formal charges. Write Lewis structure that obeys the octet rulefor OCS and assign formal charges to each atom.

For an electron in a given atom, the larger n, the A) larger the average distance from the nucleus and the higher the orbital energy. B) smaller the average distance from the nucleus and the higher the orbital energy. C) smaller the average distance from the nucleus and the lower the orbital energy. D) larger the average distance from the

Balance each of the following chemical equations. Give youranswer as coefficients separated by commas. MnI2( a q )+AgNO3( a q )?AgI( s )+Mn(NO3)2( a q ) Express your answers as integers separated by commas.

Describe and explain the possible effect on your results of the following experimental errors or variations. In each case specify the component(s) whose percentage(s) would be too high or too low. (a) After adding the dichloromethane to Panecetin, you didn't stir the mixture long enough. (b) During the NaOH extraction, you failed to mix the

Draw the unique stereoisomers for 2-chloro-2,3-dimethylpentane.Show stereochemistry clearly. To ensure proper grading, explicitlydraw all four groups, including wedge/dash bonds, around achirality center. Indicate whether the compounds could exist in anoptically active form.

Draw the unique stereoisomers for 2chloro2,3dimethylpentane. Show stereochemistry clearly. To ensure proper grading, explicitly draw all four groups, including wedgedash bonds, around a chirality center. Indicate whether the compounds could exist in an optically active form. could exist in optically active form cannot exist in optically active

Draw the ester that is formed from the reaction of benzoic acid and ethanol. Draw the alcohol needed to form isobutyl benzoate (2-methylpropyl benzoate). Draw heptanoic acid, which is the carboxylic acid needed to form the ester that smells like grape Draw ethanol, which is the alcohol needed to form the ester that smells like grape.

What is the rate constant (k)? (MTS 2/17/2018) Expt initial rate (M/s) initial [A] (M) initial [B] (M) initial [C] (M) 1 6.0x10-6 0.024 0.085 0.032 2 9.6x10-5 0.096 0.085 0.032 3 1.5x10-5 0.024 0.034 0.080 4 1.5x10-6 0.012 0.170 0.032

Consider the following general reaction and data 2A 2BCD3E

Compare and contrast the IR spectrum of your benzilproduct to that of pure benzoin in the lab manual. (Benzoin spectrais the top graph, while Benzil is the graph below it.)

100 Transmittance 06 Transmittance 4000 55 50 45 40 35 30 25 20 4000 oHo 3500 3000 3000 2500 2000 m Wavenumbers Benzil IR 2000 R 1500 m 2000 7500 Wavenumber (Cm) 1000 1000 500

Calculate the standard enthalpy change for the following reaction at 25 o C. Standard enthalpy of formation values can be found in this table. Link to table here: https://sites.google.com/site/chempendix/thermo

Calculate the standard enthalpy change for the following reaction at 25 C. Standard enthalpy of formation values can be found in this table. CH(g) 50(g) 3CO(g) 4HO(g) rxn Number kJ

Classify the definitions as that of an Arrhenius acid, an Arrhenius base, or that of a different type of acid or base. Arrhenius acid definition Arrhenius base definition Answer Bank A substance that produces an excess of hydrogen ions (H) in aqueous solution. A substance that produces an excess of hydroxide ions (OH) in aqueous solution. A

D Question 10 This question is worth 0.5 points. When carbon bonds in organic compounds, which of the following are true All of these are true Carbon forms covalent bonds. None of these are true. Carbon makes 4 bonds. Carbon can form single, double or triple bonds. Carbon atoms can form branched chains. 0.5 pts

This is cis norbornene 5,6-endo dicarboxylic anhydride Please explain why these peaks are assigned like picture(orders1234) and why 1, 2 H nmr show triplet , monolet.

8.4 H 8.0 7.6 CDC13 NO 7.2 ESSEL 6.8 SEZER 63197 6.3160 D 3 6.4 t 6.0 5.6 5.2 4.8 4.0 b 3.6 E 3.2 2.8 2.4 BRET 2.0 1.7815 ZRAEK BLAC 1.6 1.2 1,5700 0.8

please solve all questions! Thanks

A) 0.274 M B) 2.74 M C) 3.04 M D) 4.19 M E) 17.5 M 5. Calculate the molarity of a 17.5 (by mass) aqueous solution of nitric acid (63.01 gmol) whose density is 1.51 gmL. d M 17.59 salute A) 0.45 C B) 0.45 C C) 0.23 C D) 0.23 C E) 1.23 C 7. One of the following is NOT true nsdute n 17.S A) 2.216 B) 125.5 C) 225.9 D) 115.8 E) 86.5 100 g 1518027

Based on your answer above, how is the unit cell of TlCl(s)likely to be structured?

even that the density of TICI(s) is 7.00 gcm and that the length of an edge of a unit cell is 385 pm, determine how many formula units of TII there are in a unit cell. Number 1 formula units Based on your answer above, how is the unit cell of TICI(s) likely to be structured same as CsCl(s) same as NaCl(s) neither CsCl(s) NaCl(s)

Item 4 An aqueous KNO3 solution is made using 74.1 g of KNO3 diluted to a total solution volume of 2.06 L. Part A Calculate the molarity of the solution. (Assume a density of 1.05 gmL for the solution.) M Submit m IVE Submit My Answers Give Up Part B Calculate the molality of the solution. (Assume a density of 1.05 gmL for the solution.) VE My

1) Choose the pair of substances that are most likely to form a homogeneous solution. A) C6H14 and C10H20 B) LiBr and C5H12 C) N2O4 and NH4Cl D) C6H14 and H20 E) None of the pairs above will form a homogeneous solution. Answer A 2) Place the following substances in order of increasing vapor pressure at a given temperature NF3 NH3 BC13 A) NH3 NF3

Classify each statement about effective nuclear charge, Zeff, as true or false. True Effective nuclear charge does not depend on the number of electrons present in an atom. Electrons in an s orbital are more effective than those in other orbitals at shielding other electrons from the nuclear charge. A 1s electron in a Be atom has a smaller Zeff

20. Choose the bond below that is most polar. A) HI B) HBr HF D) HCI E) CH 21. Choose the best Lewis structure for CH2C12. A) H888H B D) E) H Co H HH D) 2 E) 3 H CICIE H 22. Identify the compound with the smallest percent ionic character. A) HF B) IBr C) HCI LiF H ccct H 23. Draw the best Lewis structure for BrO4 and determine the formal charge on

C) D) III IV 11. Which is the anticipated product in the following reaction A) B) C) D) I A) B) C) D) II III IV 12. Which of the following is NOT an activated dienophile A) I B) II C) III D) IV III 13. Which is the favored product in the reaction shown I II III Both II III in equal amounts OF OL 8. TV ( 1 H,CO,C. hay Hy C0.CHy CHO COyCly 11 W

What are the expected bond angles inICl 4 + ? Select all that apply. 90 degrees, 109.5 degrees, 180 degrees, 120 degrees

Which element has thefollowing configuration: [ X e ] 6 s 2 4 f 7 5 d 1 ? i know its Ce , but i need theelectrons number too

Consider the following reaction: 3CH4(g)?C3H8(g)+2H2(g) You may want to reference (Pages 832 - 835) Section19.7 and (Pages 1088 - 1091) Appendix C while completingthis problem. Part A: Using data from Appendix C in the textbook,calculate ?G? at 298 K. Express the Gibbs free energy in kilojoules to one decimalplace. ?G?= ____ kJ Part B. Calculate

The equilibrium constant for the equation HNO2(aq)H2O(l)H3O(aq)NO2(aq) is Ka5.6x104 M at 25.0 C. Calculate the value of AGorxn at 25.0 C for nitrous acid when NO2H3OHNO21.00 M AGorxn kJmol Will the acid spontaneously dissociate under these conditions yes no Calculate the value of AGrxn for nitrous acid when NO2H3O3.18x105 M and HNO21.457 M. AGrxn

What are the electron andmolecular geometries, respectively, for the carbonate ion,CO3 2? ? -Electronic geometry is trigonal planar. Molecular geometry is trigonal planar. -Electronic geometry is tetrahedral. Molecular geometry is trigonal planar. -Electronic geometry is tetrahedral. Molecular geometry is tetrahedral. -Electronic geometry is

Which of the following describes a physical propertyof copper metal? At high temperatures, copper forms a black copper oxide. Copper slowly oxidizes to form a green patina, like that on theStatue of Liberty. Copper metal is ductile. It can be ulled into thin wires. Copper does not react with water.

Distilled water (1.072 mL) is added to a cuvette for calibrationof the SpectroVis. 3 aliquots, each 182.36 L in volume, of 0.40 MCuSO4 are then added sequentially to the water in the cuvette. Whatis [CuSO4] after the third aliquot is added?

Consider the following hypothetical aqueousreaction: A(aq)B(aq). A flask is charged with0.065 mol of A in a total volume of100.0 mL. The following data are collected: Time (min) 0 10 20 30 40 Moles of A 0.065 0.051 0.042 0.036 0.031 Calculate the average rate of disappearanceof A between t= 0 min and t= 10 min,in units of M/s. Calculate the

Draw the Fischer projection for the D2ketotetrose. Switch between an aldose and a ketose by clicking on switch carbonyl group. Add or delete carbon atoms using the add () or delete (x) buttons. Clicking on a blue box once adds a hydrogen atom (H). Clicking on a blue box again toggles between H and OH. switch carbonyl group CHOH

Draw a Lewis structurefor SiF 5 - andanswer the following questions based on your drawing. 1. For thecentral silicon atom: ... The number of lonepairs = The numberof single bonds = The numberof double bonds = 2. Thecentral silicon atom ____ ... A. Obeys the octet rule B. Has an incomplete octet. C. Has an expanded octet.

Consider this system at equilibrium. A(aq)<--->B(aq)deltaH=-750 kJ/mol What can be said about Q and K immediately afteran increase in temperature? A) Q > K because Q increased B) Q> K because K decreased C) Q < K because Q decreased D) Q< K because K increased E) Q = K because neither charged How will the system respond to a

Consider this initial-rate data at a certain temperature for the reaction described by SO2 Cl2(g) SO2(g) + Cl2(g) Determine the value and units of the rate constant. [SO2Cl2]0 (M) Initial rate (M/s) 0.1 1.60 x 10^-6 0.2 3.20 x 10^-6 0.3 4.80 x 10^-6

12.2 a) Calculate the lattice energyof RbBr (s) using the following thermodynamicdata (all data is in kJ/mol). Note that the data given has beenperturbed, so looking up the answer is probably not a goodidea. Rb (s) H sublimation = 61 kJ/mol Rb (g) Ionization energy = 383 kJ/mol Br - Br (g) Bond energy = 173 kJ/mol Br (g) Electron affinity = -345

A) Calculate the total mass ofthe protons and electrons in 19 9F. Use 1.007825 amu as the mass of 11H (mass of a proton andan electron). Express your answer in atomic mass units to 6 significantfigures. B) Calculate the total mass ofthe neutrons in 19 9F. Use 1.008665 amu as the mass of 10n (mass of aneutron). Express your answer in atomic mass

Determine the kinds of intermolecular forces that are present ineach element or compound. Part A Ar dispersion forces dipole-dipole forces dispersion forces and dipole-dipole forces dispersion forces, dipole-dipole forces, and hydrogenbonding SubmitRequest Answer Part B NO dispersion forces dipole-dipole forces dispersion forces and dipole-dipole

Consider this initial-rate data at a certain temperature for thereaction described by C2H5CL5(g) -> C2H4 (g) + HCl (g) [C2H5Cl]0 (M) Initial rate (M/s) 0.100 0.770*10^-30 0.200 1.54*10^-30 0.300 2.31*10^-30 Determine the value and units of the rate constant k =

Determine which of the following statements about the pentosephosphate pathway are true. 1. Glucose-6-phosphate is reduced to ribulose-5-phosphate inthis series of reactions. 2. The pentose phosphate pathway contributes to nucleotidesynthesis. 3. Glucose is a precursor of the pentose phosphate pathway. 4. Products of the pentose phosphate pathway

Ethyl chloride vapor decomposes by the first-orderreaction C2H5Cl?C2H4+HCl The activation energy is 249 kJ/mol and thefrequency factor is 1.61014s?1 Part A Find the value of the specific rate constant at730 K . Express your answer using two significant figures. Part B Find the fraction of the ethyl chloride that decomposes in 20minutes at this

The enthalpy changes, ?H, for three reactions are given. H2(g)+1/2O2(g)?H2O(l) ?H=?286 kJ/mol Ca(s)+2H+(aq)?Ca2+(aq)+H2(g) ?H=?544 kJ/mol CaO(s)+2H+(aq)?Ca2+(aq)+H2O(l) ?H=?193 kJ/mol Using Hess's law, calculate the heat of formationfor CaO(s) using the reaction shown. Ca(s)+1/2O2(g)?CaO(s) ?H=?kJ/mol

Alkene Nomenclature Draw the structure of (2E,4E)1chloro3methyl2,4hexadie Draw the structural formula of (2E,4E)1chloro3methyl2,4hexadiene. Draw the molecule on the canvas by choosing buttons from the Tools (for bonds), Atoms, and A by default. I 2 2 H 120 Marvin JS ChemAxon 004 HCNOSTE CI Br I P F

Classify each of the given electronic transitions for a hydrogen atom.

Classify each of the given electronic transitions for a hydrogen atom. n4 n3 n4 n2 n3 n4 n6 n1 n6n2 n2 n5 n1 n5 n6 n3 n3n5 n3 n1 n1 n2 n2 n3 Ultraviolet Ultraviolet Absorption Visible Emission Visible Infrared Infrared

Classify these substances. More than one answer may apply in each case. N NO compound homogeneous mixture element pure substance heterogeneous mixture solution A pure substance solution element compound homogeneous mixture about us careers privacy policy 0 0 0 compound element terms of use homogeneous mixture pure substance heterogeneous mixture

H H H H T I HIGI H H H H H H H III H I H H H H H H H ,Choose the Lewis structure for the compound below (CH3CH)2CHCHCHOH I H H H H H I H L H H H H 5 H H H OI H H H H H H 30

Calcium ions contribute to the hardness of water. a) Based on the Ksp experiment, describe a way to soften water by removing calcium ions. 2. b) What would be the advantages and disadvantages of your method

Answer the questions for the following addition reaction. x HBr What would be the Major Organic Product WITHOUT considering Carbocation Rearrangement What is the Major Organic 1. 2. Br Br

Classify each of the following as a redox reaction or anon-redox reaction.

Classify each of the following as a redox reaction or a nonredox reaction. Redox Nonredox 2C00, ) 2C0, Zn CuCl, ZnCl, Cu SO3 HO HSO4 HCI NaOH HO NaCl

Classify bond as ionic or covalent from formula. (Pool 1 of 2) Determine whether bonds in the following species are ionic or covalent Cl CO CaF2 CrO2 HF Reset References Classification CaO P4 KCI SiCl4 CUS Covalent bonding lonic bonding,Classify bond as ionic or covalent from formula. (Pool 2 of 2) Determine whether bonds in the following species

What is the approximate pka for the weak acid. pH 14 12 10 8 6 4 2 0 0 Answer 2 (c) Equivalence point (b) Buffer region (a) Weak acid (d) Excess hydroxide ion 4 6 8 10 Volume of NaOH (mL) 12 14 Titration curve for the titration of a weak acid with a strong base. X 16

11. Which of the following compounds have the same empirical formulas a. CaH and CH4 b. HO and HO c. NOs and N4010 d. CHs and C4H10 e. More than one answer is correct 12. Putrescine, a compound produced by decaying animals, has the empirical formula CHeN an molecular mass of approximately 90 amu. Its molecular formula is a. CHN b. C4H6N2 c.

Calculate the standard potential, E, for this reaction from its equilibrium constant at 298 K. X(s) Y(aq) X4 (aq) Y(s) K 8.77 10 E V

Calculate the boiling point of a 12.75 m aqueous solution of propanol. Boiling point constants can be found in the list of colligative constants. Tb about us careers privacy policy C terms of use contact us help

Calculate the frequency of the n 2 line in the Lyman series of hydrogen. V 121 In what region of the electromagnetic spectrum is this line observed gamma radio infrared ultraviolet Xray microwave visible 1

complete the lewis structures of the atoms and ions by addingelectrons, as needed. a) Li B) Na C) Na+ D) F-

Complete these structures by adding bonds and lone pairs asnecessary. Then, determine the nitrogen-to-oxygen bond order ineach ion.

Complete these structures by adding bonds and lone pairs as necessary. Then, determine the nitrogentooxygen bond order in each ion. NO, NO NO, N N N bond order 1 1.33 1.5 1.67 2 bond order 1 1.33 1.5 1.67 bond order 1 1.33 1.5 1.67 2

Draw the structure for: a). 1,5-dichloro-3-hexyne.

Which electrons in this diagram contribute to the stability of the ion? a. One electron in the sigma 1s MO and another one in the sigma* 1s MO. b. The two electrons in the sigma 1s MO. c. All electrons. d. The electron in the sigma* 1s MO. Energy-level diagram for theHe2+ ion: