Chemistry Questions and Answers July 31, 2020

36) For the equation 2 CH2Cl2 (g) CH4 (g) CCl4 (g), you start,with 0.25 M of CH2Cl2 and it has a Kc value of 0.84. What are the equilibrium concentrations of all species

37) For the reaction at 2000 K CO (g) H (g) CO2(g) HO(g) For an experiment, the equilibrium values of each substance are as follows H 0.20 M CO 0.30 M H0 CO 0.55 M a. What is the mole fraction of CO in the equilibrium mixture b. Calculate the value of Kc, the equilibrium constant for the reaction above. c. Determine Kp in terms of Kc for

38) For the reaction PCIs (g) PCl3 (g) Cl2 (g) It is observed that greater amounts of PCI3 and Cl2 are produced as the temperature is increased. a) What is the sign of AS for the reaction Explain. b) What change, if any, will occur in A G for the reaction as the temperature is increased Explain. c) If He gas is added to the original mixture at

CO(g) 2H2S(g) HO(g) CS2(g) H(g),39) Consider the following reactions at 1200 K. CO(g) 3H2(g) CH4(g) HO(g) K1 3.92 CH4(g) 2H2S(g) CS2(g) 4H2(g) K2 3.3x10 Use the above reactions to determine the equilibrium constant for the following reaction at 1200 K.

(a) 4NO(g) N2(g) 2NO2(g) (b) 4NO2(g) 2N2(g) 402(g) (c) 2NO(g) 2NO(g) 302(g) 2N(g),41) Given the following data (1) N2(g) O2(g) 2NO(g) Kc1 4.3 x 1025 (2) 2NO(g) O2(g) 2NO2(g) Kc2 6.4 x 10 Determine the values of the equilibrium constants for the Following reactions

42) Methanol is manufactured according to the reaction CO(g) 2H2(g) CH3OH(g) The equilibrium constant (Kc) for the reaction is 10.5 at 220 C. What is the value of Kp at this temperature

43) At 1280 C the equilibrium constant (Kc) for the reaction Br2 (g) 2 Br (g) is 1.1 x 10. If the initial concentrations are Br 0.2 M and Br OM, calculate the concentrations of these species at equilibrium

44) The equilibrium constant Kp for the decomposition of phosphorus pentachloride (PCIs) to phosphorus trichloride (PCI3) and chlorine (Cl) PCI5 (g) PCl3 (g) Cl2 (g) is found to be 1.05 at 250 C. The equilibrium partial pressures of PCIs and PCl3 are 0.875 atm and 0.463 atm, respectively. What is the equilibrium partial pressure of Cl2 at 250 C.

Blood is buffered by carbonic acid and the bicarbonate ion.Normal blood plasma is 0.024 M in HCO 3 - and0.0012 M H 2 CO 3 (pk a forH 2 CO 3 at body temperature is 6.1). a) What is the pH of blood plasma? b) If the volume of blood in a normal adult is 5.0L, what massof HCl could be neutralized by the buffering system in blood beforethe pH falls

Calculate the number of moles of Cl atoms in1.2010 24 formula units of magnesium chloride,MgCl 2 . Express your answer numerically in moles Cl.

10) What is the frequency (s -1 ) of electromagneticradiation that has a wavelength of 2.3 m? a. 1.6 10 8 s -1 b. 1.3 10 33 s -1 c. 1.3 10 8 s -1 d. 1.8 10 -9 s -1 e. 1.3 10 -33 s -1 11) The energy of a photon that has a wavelength of 8.33 10-6m is ____ J. a. 2.39 ' 10-20 b. 4.5 10-25 c. 3.60 1013 d. 2.7 109 e. 2.20 10-26 14) What is the

Calculating the pH When a Common Ion Is Involved For the generic equilibriumHA(aq) ? H+(aq) + A?(aq) , which of thesestatements is true? For the generic equilibrium rm HA (aq) ~ rightleftharpoons~rmH^+ (aq)~+~A^-(aq), which of these statements is true? 1 If you add the soluble salt KA to a solution of HA that is atequilibrium, the pH would

Calculate the enthalpy of solution in kilojoules per mole of solute Separation of solute: 13.5 kj/mol Separation of solvent: 19.8 kj/mol Formation of solute-solvent interactions: -88.8 kj/mol solute (-88.8) - (13.5 + 19.8) (-88.8) - (33.3) = - 122 kJ/mol

Calculate the pH of the resulting solution if 21.0 mL of 0.210 MHCl(aq) is added to 1. 31.0 mL of 0.210 M NaOH(aq). pH = ? 2. 11.0 ml of 0.310 M NaOH(aq). pH =

Calculate the pH for each of the followingcases in the titration of 50.0 mL of 0.250 M HClO(aq) with 0.250 MKOH(aq). The ionization constant for HClO can be foundhere. (a) before addition of any KOH (b) after addition of 25.0 mL of KOH (c) after addition of 30.0 mL ofKOH (d) after addition of 50.0 mL ofKOH (e) after addition of 60.0 mL ofKOH

Calculate the pH of the resulting solution if 30.0 mL of 0.300 MHCl(aq) is added to (a) 40.0 mL of 0.300 M NaOH(aq). PH= (b) 20.0 mL of 0.400 M NaOH(aq). PH=

In a chemical reaction, exactly 2 mol of substance A react to produce exactly 3 mol of substance B. How many molecules of substance B are produced when 29.5 g of substance A reacts? The molar mass of substance A is 15.7 g/mol. Convert the mass of A to moles Convert the number of moles of A to the number of moles of B Convert the number of moles of

Calculate the heat capacity of a calorimeter if the combustion of 5.000 g of benzoic acid led to a temperature increase of 24.153 degrees Celsius. The heat of combustion of benzoic acid is 26.38 kJ/g.

Calculate the mass (in g) of 2.0 10^24 atoms of Hg. Calculate the mass (in g) of 2.0 10^24 atoms of Hg. a) 6.5 10^2 g b) 3.2 10^2 g c) 2.4 10^2 g d) 1.5 10^2 g e) 3.9 10^2 g

A) Calculate the mass defect of the oxygennucleus 16 8O. The mass ofneutral 16 8O is equal to 15.994914 atomicmass units. Answer in amu. B) Calculate the binding energy E of theoxygen nucleus 16 8O (1eV=1.60210?19J).Answer in MeV C) Calculate the binding energy pernucleon of the oxygen nucleus 16 8O.Answer in MeV / nucleon

A certain weak acid, HA, with a K a valueof 5.61?10?6, is titrated with NaOH. Part A A solution is made by titrating9.00mmol (millimoles) of HA and 3.00mmol of thestrong base. What is the resulting pH? Express the pH numerically to two decimal places. Part B More strong base is added until the equivalence point isreached. What is the pH of this

Which of the binary compounds formed by the following pairs ofelements contain covalent bonds? C and Fe Na and O Al and Cl N and O Which of the binary compounds formed by the following pairs ofelements are considered ionic compounds? C and Fe Na and O Al and Cl N and O

Calculate the molar solubility of barium fluoride in each of the following Part A pure water. S = Part B 0.10 M Ba(NO3)2 S= Part C 0.15 MNaF Express all answers using three significant figures.

Calculate the pH of the resulting solution if 23.0 mL of 0.230 M HCl(aq) is added to (a) 33.0 mL of 0.230 M NaOH(aq). pH= (b) 13.0 mL of 0.330 M NaOH(aq). pH=

Calculate the [H3O+] of the following polyprotic acid solution:0.135M H2CO3. Express two significant figures. [H3O+] =2.4?10 ?4 M Calculate the p H of this solution. Express two significant figures Calculate the [H3O+] of the following polyprotic acid solution:0.125M H3C6H5O7. Express as two significant figures Calculate the p H of this solution

Calculate the equilibrium constant for each of the reactions at25 ?C. Standard Electrode Potentials at 25 ?C Reduction Half-Reaction E ?(V) Pb2+( a q )+2 e ? ?Pb( s ) -0.13 Mg2+( a q )+2 e ? ?Mg( s ) -2.37 Br2( l )+2 e ? ?2Br?( a q ) 1.09 Cl2( g )+2 e ? ?2Cl?( a q ) 1.36 MnO2( s )+4H+( a q )+2 e ? ?Mn2+( a q )+2H2O( l ) 1.21 Cu2+( a q )+2 e ? ?Cu(

Which is the best way to prepare 3-methoxypentane via the Williamson method? ( please explain why) A). CH3OH + CH3CH2CHOHCH2CH3 + H2SO4, 140'C B). CH3OH + (CH3)2 CHCH2CH2OH+ H2SO4, 140' C C). CH3ONa + (CH3CH2)2CHBr D). CH3 I + (CH3CH2)2CHONa

Butane (C4H10) has a heat of vaporization of 22.44 kJ/mol and a normal bioling point of -0.4 celsius. A 250 Ml sealed flask contains 0.55 grams of butane at -22.0 celsius. How much butane is present as a liquid? If the butane is warmed to 25 celsius, how much is present as a liquid?

Calculate the standard entropy change for the reaction using the data from the following table AS HA Value Substance AH (kJmol) AG (kJmol) So J(K mol) H(g) 130.6 205.0 69.90 02 (8) HO (1) Express your answer to four significant figures and include the appropriate units. View Available Hint(s) 2H2(g) O2(g) 2HO(1) Submit Previous Answers J K 0.00

6) Which molecule below has hydrogen bonding A) HO B) CH3OH C) HF D) NH3 E) all of the above 7) Which intermolecular forces are found in CC4 A) Xforces (B) dispersion forces C) dipoledipole forces D) hydrogen bonding E) none of the above 8) Which intermolecular force is common to all polar molecules but NOT nonpolar molecules A) hydrogen bonding

After 55 years, what mass (in g) remains of a 200.0 g sample of a radioactive isotope with a halflife of 10.0 years O 170 g 4.4 g O 0.22 g 51 g

3. (6 pts) Use the answer bank and label the molecular shape around each of the central atoms in the amino acid glycine. H . 3b 0 30 3a 4. (8 pts) Draw the Lewis structure of the following molecules. 1 4a) CHCCHOH 4b) CHCCHCHO 5. Below are the structures of 5 different alcohols. Ethanol, CHCHOH 1Propanol, CH3CHCHOH 1Butanol, CHCHCHCHOH H 5a. (2

553 For each of the following pairs of drawings, determine the relationship between the two drawings Me a. b. C. d. e. f. H HO H HO H H HO H Me CI CH3 H Me OH H CH 3 Et OH OH H OH Me H H Me CI HO CH3 HO H H HO HO I H HO OH H CH3 Et Me H OH H

choose the best Lewis structure for seO4

49 50) Give the Lewis structure, bond angle, bonding pairs, lone pairs, electron geometry, molecular geometry for SeO42 and PF5 Se 1086 0 Se0

45. A) 62.1 g B) 48.6 g C) 21.5 g D) 27.5 g E) 0.016 g 46. A) 28.1 g B) 14.04 g C) 4.96 g D) 7.02 g E) 400.0 g 47. How many grams are present in 0.885 moles of manganese What mass, in grams, of sodium carbonate is required for complete reaction with 8.35g of nitric acid to produce sodium nitrate, carbon dioxide, and water Sulfur dioxide reacts

19) You need to prepare 2.00 L of 0.100 M Na2CO3 solution. The best procedure is to weigh out A) 10.6 g Na2CO3 and add 2.00 L of water to it. B) 21.2 g Na2CO3 and add 2.00 L of water to it. C) 10.6 g Na2CO3 and add water until the final solution has a volume of 2.00 L. (D)21.2 g Na2CO3 and add water until the final solution has a volume of 2.00 L.

What is the net cell reaction for the cobalt-silver voltaic cell? Express your answer as a chemical equation. Please include if it is (aq), (l), (s), or (g).Thanks! Co(s) -> Co^3+(aq) + 3e^- ( Anode ) Ag^+(aq) + e^- --> Ag(s) ( Cathode)

Composition of Inorganic Conjugate AcidBase Pairs in Blood The following table gives the aciddissociation constant values, Ka, for carbonic acid, H2CO3, and phosphoric acid, H3PO4. Acid Ka1 Ka2 Ka3 H2CO3 4.3x107 5.6x1011 not applicable H3PO4 7.2x103 6.2x108 4.2x1013 pH of blood The two most important inorganic blood buffers (acidbase conjugate

Classify each of the following as a Lewis acid or a Lewis base.Drag the appropriate items to their respective bins. 1.OH- 2.(CH3)2NH 3.SiCl4 4.I- 5.Ag+ 6.NO2 7.CH3OH Lewis acids Lewis bases Part C In the following pair, which species would you expect tobe the stronger Lewis acid? Hints In the following pair, whichspecies would you expect to be the

What will be the cell potential for a Cu?Zn galvanic cell with[Zn2+]=0.1 M and the [Cu2+]=0.01 M? What will be the cell potential for a galvanic cellwith and the ? A) 1.10 V b) 1.13 V c) 1.04 V d) 1.07 V

Complete and balance the following metallurgical reactions. Phases are optional. I don't need them balanced, I can do that. I'm just not sure what's on the other side of the arrows.a. MoO3(s) + H2(g) -->b. Cu2S(s) + O2(g) -->

Complete and balance each of the following equations. If no reaction occurs, write NOREACTION. Express your answer as a chemical equation. Identify all of the phases in your answer. 1) KCl (aq) + CaS (aq) --> 2) CrBr2 (aq) + Na2CO2 (aq) --> 3) NaOH (aq) + FeCl3 (aq) --> 4) NaCl (aq) + Hg2(C2H3O2)2 (aq) --> 5) (NH4)2SO4 (aq) + SrCl2

The carbonate ion, CO32-, can best be described as having: octahedral geometry about the carbon a tetrahedral geometry about the C atom a trigonal planar geometry about the C atom a total of 22 valence electrons a bond order of 2

Calculate the theoretical yield for the bromination of both stilbenes and cinamic acid, assuming the presence of excess pyridinium tribromide.Calculate the theoretical yield for the bromination of both stilbenes and cinamic acid, assuming the presence of excess pyridinium tribromide. cinnamic acid 150 mg cisstilbene 100 L trans stilbene 100 mg

Carbonyl Compounds: Complete the following mechanism involvingcyclohexanone Draw a reasonable mechanism for this reaction.

Carbonyl Compounds Complete the following mechanism involving cyclohexanone Part A Draw a reasonable mechanism for this reaction. 15 Interactive 3D display mode Ph Hi PhPCH Ph Edit the reaction by drawing all steps in the appropriate boxes and connecting them with reaction arrows. Add charges where needed. Electron flow arrows should start on an

Calculate the standard cell potential for each of the followingelectrochemical cells. Part A Ni2+( a q )+Mg( s )?Ni( s )+Mg2+( a q ) Express your answer using two decimal places. E ?cell = _____ V Part B 2H+( a q )+Fe( s )?H2( g )+Fe2+( a q ) Express your answer using two decimal places E ?cell =_______ V Part C 2NO?3( a q )+8H+( a q )+3Cu( s

Calculate the rms speed of an oxygen gas molecule, O2, at33.0 o C Express your answer numerically in meters per second I calculated 450.0 m/s and its saying its worng. not sure whatim calulating wrong here...

Calculate ? G ? at 298 K for thefollowing reactions. Part A NH3( g )+HBr( g )?NH4Br( s ) Part C 2KClO3( s )?2KCl( s )+3O2( g ) Part E CH4( g )+3Cl2( g )?CHCl3( g )+3HCl( g ) ? G ?f for CHCl3( g ) is -70.4 kJ/mol Calculate the change in Gibbs free energy for each of thefollowing sets of ? H rxn ?, ? S ?rxn,and T. Answer in kJ. 1.? H ?rxn=? 90. kJ ,

Calculate the frequency of the n = 5 line in the Lyman series of hydrogen.

Classify each substance as either a reactant or product in the chemical reaction. ethanol, carbon dioxide, water, oxygen

Calculate the enthalpy change for the decomposition reaction in kilojoules per mole of N H 4 C l O 4 in kJ/mol? Substance H 2 O ( g ) H C l ( g ) N H 4 C l O 4 ( s ) delta H ( k J / m o l ) -241.82 -92.30 -295.8

Which choice represents a pair of resonance structures View Available Hint(s) OHH and H O NNand BrBr O C and OC ONF and NF

Chlorine gas was first prepared in 1774 by the oxidation of NaCl with MnO2: 2NaCl (s) + 2H2SO4 (l) + MnO2 (s) ---> Na2SO4 (s) + MnSO4 (s) + 2H2O (g) + Cl2 (g) Assume that the gas produced is saturated with water vapor at a partial pressure of 28.7 mm Hg and that it has a volume of 0.597L at 27C and 755 mm Hg pressure.a) What is the mole

(13) Please provide the structure of the major organic product in the reactions below. (32, 4 each) (a) (c) (e) (g) Et 200 Br Me 1g 2nd 3d 4nd 51 61 7 st H 180 160 1. AgO 2. heat 2 3. CHl 4. AgO 5. heat 140 1. NaOMe 2. HBr 3.1BUOK 4. HBr, ROOR Br 1. PhyP OH 2. CH3CHCHCHLi, ether HSO4 120 100 ppm 80 60 40 (b) 20 (d) ON (f) (14) Please propose the

Which choice best describe the polarity of ClF5? a) The molecule is polar and has polar bonds. b) The molecule is nonpolar and has polar bonds. c) The molecule is polar and has nonpolar bonds. d) The molecule is nonpolar and has nonpolar bonds.

Classify each of the following as a property of acids or bases. Taste Sour, Feels Slippery, taste bitter, turn litmus paper red, turn litmus paper blue, dissolve many metals

16) Which of the following statements about matter is FALSE A) Matter occupies space and has mass. B) Matter exists in either a solid, liquid or gas state. C) Matter is ultimately composed of atoms. D) Matter is smooth and continuous. Enone of the above 17) A solid form of matter in which there is long range repeating order is called A) amorphous

Question 15 of 15 Energy Calculator sapling learning. Band theory is an extension of molecular orbital theory. According to band theory, atomic orbitals between atoms in a sample form a nearly continuous band of molecular orbitals. In a metal, the bottom half of the band is composed of bonding molecular orbitals and the top half of the band is

Balance each of the following redox reactions occurring in basicsolution. a)MnO?4( a q )+Br?( a q )?MnO2( s )+BrO?3( a q ) MnO?4( a q )+H2O( l )+Br?( a q )?MnO2( s )+2OH?( a q )+BrO?3( a q ) 2MnO?4( a q )+H2O( l )+Br?( a q )?2MnO2( s )+2OH?( a q )+BrO?3( a q ) 2MnO?4( a q )+H2O( l )+Br?( a q )?2MnO2( s )+OH?( a q )+BrO?3( a q ) MnO?4( a q )+H2O( l

Calculate Kc for the reaction below. 12(g)21(g)Kp6.26x1022 (at 298 K) Express your answer using three significant figures. Kc Part B Calculate Kc for the reaction below. CH4(g)H2O(g)CO(g)3H2(g)Kp7.7x1024 (at 298 K) Express your answer using two significant figures. Kc Part C Calculate Kc for the reaction below. (at 298 K)

b) What was the initialreactant concentration for the reaction described in PartA? c) The reactant concentration in a first-orderreaction was 9.60?10 ?2 M after30.0 ss and 7.80?10 ?3 M after90.0 s . What is the rate constant for thisreaction? d) The reactant concentration in a second-orderreaction was 0.330 M after 265 ss and3.10?10 ?2 M after 865

The integrated rate laws for zero, first, and secondorder reaction may be arranged such that they resemble the equation for a straight line, y mx b. Order 0 1 2 Integrated Rate Law Graph A vs. t A kt Ao lnA kt ln Ao lnA vs. t 1 1 vs. t Ao A 1 kt Slope k k k Part A The reactant concentration in a zeroorder reaction was 0.100 M after 100 s

Calculate ?G?rxn and K for each of the following reactions. Part A The reaction of Cr2+(aq) with Cr2O2?7(aq) in acidsolution to form Cr3+(aq). Calculate ?G?rxn. Part B Calculate K.Express your answer using two significant figures. Part C Thereaction of Cr3+(aq) and Cr(s) to form Cr2+(aq). [The reductionpotential of Cr2+(aq) to Cr(s) is -0.91 V.]

mmyctitemViewassignment ProblemiD62207869offs DAC cars uld y cars, to cles tury that Part A Avogadros Law states that at a given temperature and pressure, what quantity is constant OVn OVXn Submit HA Hints My Answers Give Up Review Part Value MasteringChemistry Gases... X Units Part B If it takes three breaths to blow up a balloon to 1.2 L, and

Calculate the entropy change in the surroundings associated with this reaction occuring at 25 degrees C. Show all your calculations. The change in enthalpy for the reaction is +163.2 kJ.2N2(g) + O2(g) ---> 2N2O(g)

Write a balanced equation for the combustion of gaseous methane?

Part A Another potential future fuel is methanol (CH3OH). Write a balanced equation for the combustion of gaseous methanol Express your answer as a chemical formula. a Submit AH rxn Part B Another potential future fuel is methanol (CH3OH). Use bond energies to calculate the enthalpy of combustion of methanol in kJmol. Express your answer in

Analyze the polarity of each bond in the following organic compound. H a) Which bond, other than the CC bond, is the least polar in the molecule CO CCI CH b) Which carbon atom has the most partial positive character the left C the right C no difference

1) Atomic radius generally increases as we move A) down a group and from left to right across a period B) down a group and from right to left across a period C) up a group and from right to left across a period D) down a group the period position has no effect E) up a group and from left to right across a period

Calculate the change in Gibbs free energy for each of the following sets of Hrxn, Srxn, and T. 1. Harxn81 kj, Srxn 144 JK, T 302 K Express your answer using two significant figures. 2. Harxn 81 kJ, Srxn144 JK, T 755 K Express your answer using two significant figures. 3. HOrxn 81 kj, Srxn144 JK, T 302 K Express your answer using two significant

Calculate the change in Gibbs free energy for each of the following sets of AHorxn, ASorxn, and T. (Assume that all reactants and products are in their standard states.) Part A AHorxn84kJ, ASorxn157JK, T302K Express your answer as an integer. Part B AHorxn84kJ, ASorxn157JK, T860K Express your answer as an integer. Part C AHorxn84kJ, ASorxn157JK,

You are given three bottles labeled A, B, and C. Each bottle contains a white solid. The solid in bottle A melts at 801 C. The solid in bottle B melts at 150 C. The solid in bottle C melts at 825 C. Part A Based on the melting points, classify each compound as ionic or molecular. Drag the appropriate items to their respective bins. View

2. Decompose 1.00 mol HS as follows 2HS (g) 2H (g) S2 (g) at constant total pressure P 1.00 bar. Using the given tables in this subject to take thermodynamic properties, then a Find the equation of ArxnCp as a function of temperature b Find the equation of ArxnH as a function of temperature c Find the equation of Kp as a function of temperature

Partial Question 2 Identify the correct reagents (AG) needed to complete the reactions 14. Choices may be used more than once or not at all. )C 3) HO. 2 3 Br. CECCH CECH i 4) OH A. 1) Hg(OAc), HO 2)NaBH B. Br HO C. Na in NH(1) D. H, Lindiars catalyst E. 1) (Sia)2BH,THF 2) HO HO F. H, Pt G. Cant be accomplished with any reagents listed A 0.380.5

Determine whether or not the mixing of each of the two solutions indicated below will result in a buffer. Part A 75.0 mL of 0.10 MHF; 55.0 mL of0.15 M NaF Part B 150.0 mL of 0.10 MHF; 135.0 mL of0.175 M HCl Part C 165.0 mL of 0.10 MHF; 135.0 mL of0.050 MKOH Part D 125.0 mL of 0.15 M CH3NH2;120.0 mL of 0.25 MCH3NH3Cl Part E 105.0 mL of 0.15 M

Calculate - cell potential - equilibrium constant and - free energy change for Ca (s) + Mn^2+(ag) (1M) -----------> Ca^2+(aq)(1M) + Mn)s) Ca E = -2.87 V Mn^2+ + 2e^- -------> Mn E = -1.18V

Determine the molar solubility of Fe(OH) 2 in purewater. K sp for Fe(OH) 2 )= 4.87 10 -17 .

Describe the hybrid orbitals used by the central atomand the type(s) of bonds formed inI 3 - . sp sp 2 sp 3 sp 3 d Number of bonds: Number of bonds:

Part A Write a single Lewis structure for SO3. Draw the Lewis dot structure for SO3. Include all lonepairs of electrons. Part B Determine the hybridization at the S atom. Determine the hybridization at the atom. s p s p 2 s p 3 s p 3 d s p 3 d 2 Part C Are there other equivalent Lewis structures for themolecule? There are other equivalent Lewis

The density of solid Ni is 8.90 g/cm3. How many atoms arepresent per cubic centimeter of Ni? atoms/cm^3 As a solid, Ni adopts a face-centered cubic unit cell. How manyunit cells are present per cubic centimeter of Ni? unitcells/cm^3 What is the volume of a unit cell of this metal? cm^3 What is the edge length of a unit cell of Ni? cm

Consider the following elementary reaction equation. NO3 (g) + CO (g) yields NO2 (g) + CO2 (g) What is the order with respect of NO3? What is the overall order of the reaction? Classify the reaction as unimolecular, bimolecular, or termolecular

Compound Ksp Iron(II) sulfide 3.7210-19 Magnesium hydroxide 2.0610-13 Lead(II) bromide 4.6710-6 A) Use the ksp values in the table to calculate the molar solubility of FeS in pure water. S= ____M B)Use the ksp values in the table to calculate the molar solubility of PbBr2 in pure water. S=___M

Complete the half reactions for the cell shown here, and show the shorthand notation for the cell by dragging labels to the correct position. The electrode on the left is the anode, and theone on the right is the cathode. Anode half reaction: Pb(s) + 2Cl- --> PbCl2(s) + 2e- Cathode half reaction: 2AgCl(s) + 2e- --> Ag(s) + 2Cl- shorthand

At constant pressure, which of these systems do work on the surroundings? Check all that apply. a. 2A(g)+3B(g) --> 4C(g) b. A(s)+B(g) --> 2C(g) c. A(g)+B(g) --> 3C(g) d. A(s)+2B(g) --> C(g)

D) Write balanced net ionic equation for the following reaction.CaS(aq)+CuCl2(aq)?CuS(s)+CaCl2(aq) Express your answer as a chemical equation including phases. E) Write balanced complete ionic equation for the followingreaction. NaOH(aq)+HNO3(aq)?H2O(l)+NaNO3(aq) Express your answer asa chemical equation including phases. F) Write balanced net

6 g sample of a subtance was heated from 21 C to 62 C rquiring 113 J to do so. What is the specific heat of the substance NOTE round your answer to 2 decimal

Consider a generic redox reaction then suppose that thecoefficients in the redox reaction are doubled. How will thefollowing quantities be affected for a voltaic cell undernonstandard conditions, will they be Doubled, Halved, Squared, orNo Change. Note that n is written as ?e in some documents. X(s) + Y+(aq) ? X+(aq) + Y(s) A) E? B) n C) E D) Q E)

Consider the galvanic cell described by (N and M aremetals): N( s )|N2+( aq )||M+( aq )|M( s ) If E o cathode = 0.182 V and E o anode = 1.411 V, and [N2+(aq)] = 0.931 M and[M+(aq)] = 0.655 M, what is E cell, using the Nernstequation? ____ V (the answer is supposed to be 1.233 but I don't understandhow)

Consider the following isomerization reactions of some simplesugars and values for their standard Gibbs freeenergy ? G ?: reaction A:reaction B:glucose-1-phosphatefructose-6-phosphate??glucose-6-phosphate,glucose-6-phosphate, ? G ?=?7.28 kJ/mol ? G ?=?1.67 kJ/mol Part A Calculate ? G ? for the isomerization ofglucose-1-phosphate to

Combine these amino acids into a tripeptide. Add or remove atoms and bonds as needed. H H NE H2C CH2 CH2 H H N t CH2 CH H3C CH3 H H 1 H OH H

What descriptive term is applied to the type of diene represented by 2,4-hexadiene? A. Cumulated diene B. Conjugated diene C. Alkynyl diene D. Isolated diene E. None of the above

Consider a galvanic (voltaic) cell that has the generic metals X and Y as electrodes. If X is more reactive than Y (that is, X more readily reacts to form a cation than Y does), classify the following descriptions by whether they apply to the X or Y electrode. anode cathode electrons in the wire flow toward electrons in the wire flow away cations

Cyclopropane is a highly strained molecule. why? Select all thatapply a) The cyclopropane CH2 group are staggered with each other,leading to torsional strain b) The bond angle of cyclopropane are 60, leading the anglestrain c) The bond angle ofcyclopropane are 120, leading the angle strain d) The cyclopropane is unable to puckerand relieve some

Match the following solutions with their pH values. H1 x 107 M OH 1 x 1012 M pOH 1 Neutral Solution Acidic Solution A pH2 B. pH 7 C.pH 13 D.pH 7

Classify each of the characteristics as lock-and-key model or induced-fit model or both. 1) active site is rigid 2) enzyme is substrate specific 3) substrate shape is modified 4) active site is flexible 5) enzyme returns to initial shape after catalysis 6) active site-substrate interaction induces an optimal fit for

25. Calculate the standard enthalpy change for the following chemical equation. 4FeO (s) + O2 (g) 2Fe2O3 (s) Use the following thermochemical equations to solve for the change in enthalpy. Fe (s) + O2 (g) FeO (s) H =-269 kJ/mol 2Fe (s) + 3/2O2 (g) Fe2O3 (s) H= -825 kJ/mol -2726 kJ/mol 556 kJ/mol -556 kJ/mol 574 kJ/mol -574 kJ/mol

Circle the correct answer for each question 1. In which reaction does the oxidation number of oxygen increase a. Ba(NO3)2(aq)KSO4(aq) BaSO4(s)2KNO3(aq b. HCl(aq)NaOH(aq) NaCl(aq)HO(l) c. MgO(s)HO(l) Mg(OH) (s) d. 250(g) O(g) 2503(g) e. 2HO(l) 2H(g)O(g) 2. Which of the following is an oxidationreduction reaction a. Cu(s)2AgNO3(aq)

2) Draw the Lewis structure of the given compound, determine the formal charge of each element and decide the most stable form. a) CH3CHNH2 (ethylamine) b) CH3COOH (acetic acid) c) HCSNH2 d) NH2CONH2 e) CICHCHNH2 223 Fall 5 ipol Univer

Calculate the entropy of each of the following states. I think we are using S=k*lnW State (a) is equal to 0, but I still dont know how to get b and c. b) State (b) c) State (c)

(a) (b) (c)

Consider the process of converting liquid water to steam:H2O(l)H2O(g) What is true for this reaction? Select all that are true. It is exothermic It releases heat It absorbs heat H = 0 It has a + H It has a H It is endothermic

Consider the molecule below. Determine the hybridization at each of the 3 labeled atoms. Along with the hybridization determine how many bonds and how many bonds each of those 3 atoms can have. I'm really not sure how to do this problem? I don't get how to tell how many bonds and bonds there are? I also don't understand how to get the

19 6 H

Compound air (unretained) 631800 tr, min W, min 1.07 5.25 5.93 0.68 0.71 2.631800030 20557950 The following data was obtained by gas chromatography on a 10.0m capillary column. Vs 19.6 mL and VM 62.6 mL Calculate (a) the retention factor for A (b) the selectivity factor for the two compounds (c) the average number of theoretical plates (d) the