Chemistry Questions and Answers May 30, 2020

Which reagent(s) would you use to accomplish the below reaction CH3 CH3 H3C. CH H3C O 1) Hg(OAc)2, H20, 2) NABH4 O MCPBA O 1) OsO4, 2) H20, NAHSO3 O 1) R2BH, 2) NaOH, H2O2 O HESO4, H20, zSO4 ,Which reagent(s) would you use to accomplish the below reaction CH3 CH3 H3C. CH H3C O 1) Hg(OAc)2, H20, 2) NABH4 O MCPBA O 1) OsO4, 2) H20, NAHSO3 O 1) R2BH,

What physical conditions should be taken into account in the place where the scales are placed?

Indicate which of these instruments are used to contain a volume: Burette, volumetric flask, pipettes, graduated cylinder, Erlenmeyer, Beaker

Incomplete combustion of glucose C 6 H 12 O 6 glucose reacts with oxygen gas O 2 and forms carbon dioxide CO 2 and water H 2 0. How many moles of oxygen gas react with 2.0 g of glucose? 2.0 g of glucose reacts with excess oxygen gas (unlimited amount of oxygen to present). How many grams of water are formed?

Given the following reaction equation: 2Al + 3Cl 2 2AlCl 3 0.230 g of Al reacts with 1.10 g of Cl 2 . How much AlCl 3 can be formed?

At a certain temperature, the equilibrium constant for the chemical reaction shown is 2.54 x 103. At equilibrium, the concentration of AB is 2.325 M, the concentration of BC is 1.525 M, and the concentration of AC is 0.260 M. Calculate the concentration of B at equilibrium. AB(aq) BC(aq) AC(aq) 2 B(aq) B M

Calculate the pH after 0.15 mol of NaOH is added to 1.00 L of the solution that is 0.78 M HF and 1.07 M KF. Calculate the pH after 0.10 mol of HCI is added to 1.00 L of the solution that is 0.78 M HF and 1.07 M KF. 40

An organic compound contains 76.6% by weight of carbon and 6.4% by weight of hydrogen. Its molar mass is 94.1 g/mol. Calculate the chemical formula of the compound.

A reaction has a rate constant of 8.52 x 102s at 12 C and 2.61 x 101s at 45 C. Determine the activation barrier for the reaction. O 3.08 kJ mol 0.152 ki mot O 18.3 k mol 25.6 kJ mol 3.38 kJ mot

Assuming standard conditions, and considering the table of standard reduction potentials for halfreactions, given in your text, rank the following species according to their relative strength as reducing agents. For example, the most powerful reducing agent would be given rank 1, and the least 6. O Ni O Ag OH (basic halfcell solution) H

A sheet of gold weighing 9.8 g and at a temperature of 17.8C is placed flat on a sheet of iron weighing 20.3 g and at a temperature of 59.4C. What is the final temperature of the combined metals Assume that no heat is lost to the surroundings. C

Give the IUPAC of the ff

H3C CH2CH2CH3 CHCHCH2CH3 H3CCH H3

State what point group is obtained by adding a horizontal plane of symmetry (sigmah) to the C3v point group. List all the subgroups contained in the point group you have identified. List all the symmetry classes in this point group and state its order. State the four important rules for Character Tables derived from the Great Orthogonality

what is the percentage of carbon in the organic compound which 0.2g of it burns completely in excess of oxygen gas forming 0.44g of co2 gas ??????

A 25.0 mL aliquot of 0.0660 M EDTA was added to a 46.0 mL solution containing an unknown concentration of V. All of the V present in the solution formed a complex with EDTA, leaving an excess of EDTA in solution. This solution was backtitrated with a 0.0330 M Ga solution until all of the EDTA reacted, requiring 14.0 mL of the Ga solution. What was

How would using malate for the energy source in the citric acid cycle effect hoe many ATP could be produced. please show work/ explain in detail.

9. Would valence bond theory be expected to give a reliable description of the bonding in hex2enoic acid Why or why not 10. In 3 sentences or less, explain how the LCAOMO technique enables molecular orbitals to be constructed.

The latent heat of fusion and vaporization of water is 333.6 Jg and 2256.7 Jg respectively at the normal melting and boiling point. C,4.19 Jg 1K1 for liquid water, density0.917 gcm3 for ice at 1 atm and 0C, density 1.000 gcm3 and 0.958gcm3 for water at 1 atm and 100C respectively. For liquid water, C, varies slightly with T. The value given is an

Mentions that macromolecule is the main component of paper and where it is obtained?

What is the pH of a buffered solution that contains 0.25 M NH, and 0.22 M NH,C

What are the two acids in CH,OH HCoe CH,0 e the reaction () , (B) CH,OH HCOH (C) (D) CHOH HCOE

Which of the following would be a stronger base considering the following pKb values O 1.39 O 3.49 O 2.89 O 3.45

4. The equilibrium constant for O2 20 is 2.4547 (102) atm. at 3100 K. What is the equilibrium constant for the O O2 at the same temperature Clearly show units for the answer.

A solid sample adsorbs 0.63 mg of CO when the pressure of the gas is 36.0 kPa at 300 K. The mass of the gas adsorbed when the pressure is 4.0 kPa at 300 K is 0.21 mg. If the Langmuir isotherm applies for the system, determine the fractional coverage at the two pressures.

A layer of 2.5 in thick firebrick (kb 1.0 Btuhr ft F) is placed between two in. thick steel plates (ks 30 Btuhr ft F). The faces of the brick adjacent to the plates are rough, having solidtosolid contact over only 35 of the total area, with the average height of asperities being L2232 in. If the surface temperatures of the steel plates are 250

What is a polar substance, and a nonpolar nonpolar substance ?, Give examples.

Use table 17.1 below to calculate G at 355 K for the following equation: 2NaCl(s) + F2(g) > 2NaF(s)+ + Cl2(g) State whether the equation is spontaneous or not.

TABLE 17.1 Standard Entropies at 25C (JmolK) of Elements and Compounds at 1 atm, Aqueous lons at 1 M OHT Elements 4 205.0 O2(8) Pb(s) P4(s) S(s) Si(s) Sn(s) Zn(s) 116.1 I2(s) K(s) Mg(s) Mn(s) N2(g) Na(s) Ni(s) 223.0 Cl2(8) Cr(s) Cu(s) F2(8) Fe(s) H2(8) Hg(1) 42.6 64.8 Ag(s) Al(s) Ba(s) Br2(1) C(s) Ca(s) Cd(s) 23.8 64.2 28.3 164.4 32.7 32.0 33.2

Earlier civilizations smelted iron from ore by heating it with charcoal from a wood fire: 2Fe2O3(s) + 3C(s) > 4F(s) + 3CO2(g) a) Write an expression for G as a function of temperature. Prepare a table of Delta G values at 100K intervals between 100K and 500K. b) Calculate the lowest temperature at which the smelting could be carried out.

For the reaction: 2H2O(l) + 2Cl-(aq) > H2(g) + Cl2(g) + 2OH-(aq) a) Calculate G at 25C. b) Calculate G at 25C when pH2 = pCl2 = 0.250 atm, [Cl-] = 0.335 M and the pH of the solution is 11.98.

N2(g) + 3F2(g) > 2NF3(g) H298 = -264kj mol^-1. S298 = -278 JK^-1 mol^-1 The following questions relate to the synthesis reaction represented by the chemical equation and data above. 1) Calculate the value of the standard free energy change for the reaction. 2) Determine the temperature at which the equilibrium constant, Keq, for the reaction is

Average Bond Enthalpy (kj mol) Bond NEN 946 N F 272 F F

If The amount of A 30 in DNA) sample ) so what of the following is correct The amount of T 40 This nitrogen base makes 3 hydrogen ponds with T The amount of G is equal to amount of A none of them

The clinical syndrome of patau syndrome is O 47,13 2n1 trisomy 13 O O O

From table A: Calculate Average, STD, C.V. (%), error, %error.

Table A. Report of balance calibration results. Mass Balance 1 (g) Reference Reference weight Reference weight weight 1 2 3 1 grams 2 grams 5 grams Mass 1 1.0003 2.0003 5.0000 Mass 2 1.0000 2.0005 5.0003 Mass 3 0.9999 2.0002 4.9999 Mass 4 0.9998 1.9999 5.0001 Mass 5 1.0002 2.0000 5.0002

Can you make a EXPERIMENTAL FRAMEWORK and HYPOTHESIS for this experiment? https://youtu.be/b_CrNjlayx4

Can you help me with the ANALYSIS OF RESULT CONCLUSION AND RECOMMENDATION for this experiment? THANK YOU https://youtu.be/b_CrNjlayx4

Can you share your ideas for APPLICATION TO PHYSICAL CHEMISTRY of this experiment? Please include your references if theres one. https://youtu.be/b_CrNjlayx4

I. EXPERIMENT TITLE II. EXPERIMENTAL FRAMEWORK III. HYPOTHESIS IV. MATERIALS V. METHODOLOGY VI. RESULTS VII. ANALYSIS OF RESULTS VIII. CONCLUSION & RECOMMENDATION IX. APPLICATION TO PHYSICAL CHEMISTRY X. REFERENCES https://youtu.be/b_CrNjlayx4

Briefly outline the stepwise reaction routes for the preparation of (2R,3S)-bicyclo[2.2.1]hept-5-ene-2,3- dicarboxylic acid.

Calculate the volume of concentrated HCl with 36% purity and density of 1.19 g / mL needed to prepare 100mL of 0.1 M solution.

What is the structure of the product formed, whose molecular formula is C11H5NO2 and the mechanism that leads to this formation CEN NMe, NaH HO C11H5NO2

Consider the impact and importance of the development of Mega Ports the widening of the Panama Canal and the increased use of the western rivers of the United States as a means of moving large quantities of hazardous chemicals. Read the following article: https://www.law.cornell.edu/cfr/text/33/part-151/subpart-D What are CBRNE threat vectors?

5. The reaction of solid calcium oxide with solid ammonium chloride is endothermic: CaO ( s ) + 2 NH 4 Cl ( s ) 2 NH 3 ( g ) + H 2 O ( g ) + CaCl 2 ( s ) a) Do you expect S rxn to be positive or negative for this reaction? Explain your answer in 1-2 sentences. b) Do you expect this reaction to be always spontaneous, never spontaneous, spontaneous

1. Consider the two molecules below. Propanoic acid Lactic acid 3 2 3 2. H C CC H C CC o H. H 0. H 4 H. H. 5. Produced by bacteria in Produced in the muscle human sweat glands. cells during exercise. Ka 1.3 x 105 Ka 1.4 x 104 a) Identify the most acidic hydrogen atom in each of the two molecules. Explain your choice in 12 sentences. b) Explain

1. Consider the two molecules below. Propanoic acid Lactic acid 3. 3. H 10 C H. H. Produced by bacteria in human sweat glands. Produced in the muscle cells during exercise. K, 1.3 x 105 1.4 x 104 a) Identify the most acidic hydrogen atom in each of the two molecules. Explain your choice in 12 sentences. b) Explain the difference in K, values

31,405 Quiz Exam 2 1. Consider the two molecules below. Propanoic acid 2 3 H H H 2 HO O H ccc C H 0. H 4 5 6 5 4 Produced by bacteria in human sweat glands. Produced in the muscle cells during exercise. Ka 1.3 x 105 Ka 1.4 x 104 a) Identify the most acidic hydrogen atom in each of the two molecules. Explain your choice in 12 sentences. b)

2. Morphine is a weak base with a pk, of 5.80. a) If 25.0 mL of a 0.0700 M morphine solution is titrated with 0.100M hydrochloric acid, what will the pH of the solution be at the equivalence point b) What will the pH of the solution be at the halfequivalence point c) Which of the following indicators would be most appropriate for this titration

3. Calcium phosphate is one of the two main compounds that can precipitate out of urine to form kidney stones. The Ksp of calcium phosphate is 2.07 x 10 33 a) What is the molar solubility of calcium phosphate b) If the Ca2 concentration in a persons urine is 150 mgL, what concentration of phosphate in the urine (in mgL) would be necessary for

4. Ozone decomposes according to the following reaction 2 03 (g) 3 02 (g) a) Use the table below to calculate AG,rxn at 230 K. S (Jmol Compound (kJmol) K) O2 (g) 205.2 O3 (g) 142.7 238.9 b) Calculate AGXO for this reaction taking place in the ozone layer, where Po2 is 4.0 x 10 3 atm, Po3 is 2.0 x 10 atm, and the temperature is 230 K.

Tell the coolest thing about Gibbs free energy and its detail

To maintain a sodium chloride (NaCl) concentration close to water of sea, in an aquarium a solution was prepared containing 3.7 g of NaCl per 100 g of water. What is the mass percent of sodium chloride in the solution?

Lanthanides and actinides. Are they metals or non-metals? Explain

An element has an atomic number Z: 91 and an A: 231 and emits two Beta rays. How many protons would it have in its nucleus?

1. Explain the difference between strong and weak electrolytes.

25 g of copper granules of unknown purity are treated completely with a concentrated acid solution nitric, forming gaseous nitric oxide, cupric nitrate, and water in a liquid state. a) Represent the corresponding chemical equation e equalize using the electron-ion method. b) If 4.7 liters of nitric oxide are obtained under conditions normal

For a SPAD operating in Geiger mode with no impinging photons, a dark count rate of 25 counts/s, and no afterpulsing, draw the voltage output vs time for a period of 100 ms.

Calculate the cost of lime and soda required for softening 1 million litres of water containing: (MgHCO3)2 = 73 mg/L; MgSO4 = 120 mg/L; CaSO4 = 68 mg/L; CaCl2 = 111 mg/L. The cost of lime of 80% purity is Rs. 200 per metric ton and that of soda of 90% purity is Rs. 12,000 per metric ton.

Explain with equations and calculate the quantity of quick lime and soda ash required to soften 30,000 litres of water containing: (i) 290 ppm of magnesium bicarbonate and 211 ppm of sodium chloride: (ii) 30 pm of Mg and 11.3 of HCO3- (iii)2.5 ppm of the free acids, 150 ppm of sulphate ions and 79 ppm of chloride ions.

Prepare a chart with chemical reactions: Lime and soda required for the softening of hard water.

Mass Spectrum (not shown) M 193 (100) mz 3D IR Spectrum (not shown) 3300 (m), 3200 (m) 3060, 2985, 1725, 1600, 1495 cm1 (all listed are strong (s) unless otherwise indicated) H NMR Spectrum (400 MHz, CDC13, 25 C) d (J 8 Hz) d (J 2 Hz) dd (J 8, 2 Hz) br s m 7 6 3 4 PPM 5

Zinc (II) is extracted with 2 x 10^-4 M dithizone in carbon tetrachloride with a pH1/2 value of 3. Calculate the pH at which 90% of zinc in an aqueous solution can be extracted with dithizone. Equal volumes of the aqueous and organic phases are used.

Q.1 Interpret the following IR spectrum by labelling the characteristic absorption peaks and write the name of compound 100 Fingerprint regionc 3000 2000 1500 1000 4000 400 WAVENUMBER em1 TRANSMITTANCE

Q.2 What are the activity coefficients for iron(III) and sulfate in an aqueous solution of 10 mM sulfuric acid, 5 mM calcium sulfate, and 3 mM iron(III) chloride

Substances those are partially dissolved in water are commonly known as a. hydrophilic hydrophobic b. false statement c. hydrophilic d. hydrophobic e. all given choices are incorrect

An amphipathic molecules are those have a Choose the option a. hydrophilic chains and ionic and polar ends b. hydrophilic chains and ionic or polar ends c. hydrophobic chains and ionic or polar ends d. hydrophobic chains and ionic and polar ends n

All of the following are wrong sentences except 1Sports players avoid eating foods that contain cholesterol because it is rich in calories 2The Greek term eicosa is used for the number 22 3Atherosclerosis causes an accumulation of sphingosine 4The fatty acid in the Waxes is always saturated 5Krabbe disease occurs in nerve cells

Choose the correct sentence about cholesterol 1Cholesterol is a long chain of fatty acids 2The double bond in cholesterol is located in the first link between the fifth and sixth carbonates 3Cholesterol contributes to the make of vitamin A 4Apples are a rich source of cholesterol 5All sentences are wrong

The chewing gum can be made from SBR, a rubbery copolymer of styrene and butadiene. Calculate the composition of a mixture of styrene and butadiene monomers to obtain aSBR composition of 25% styrene and 75% butadiene. We give: the constant of A = 0.58 and the constant of B = 1.35 (A: styrene and B:butadiene).

Silver has a density of 10.5 g / cm3. You want to buy a pure silver ring, for this the jeweler weighs the ring (18 g); and then immerses it in a measuring cylinder with water and it is observed that the water level rises 1.5 ml. What is the value of the real density of the jewel and will it be pure silver?

Q1) For a certain diatomic molecule, two of the pure-rotational absorption lines are at 806.65 GHz and 921.84 GHz and there are no pure-rotational lines between these two lines. Find the initial / value for each of these transitions and find the molecular rotational constant B.

Calculate the standard enthalpy of hydrogenation of liquid benzene from its standard enthalpy of combustion (3268 kJ mol1) and the standard enthalpy of combustion of liquid cyclohexane (3920 kJ mol1).

Gather 5 materials that can be food, cleaning, toilet; then classify these materials into homogeneous or heterogeneous with some argumentation that gives meaning to the classification, record the results in a table.

Creams, liquid soaps and hair creams are used daily. Explain how these colloidal products are formed taking into account the states of aggregation of each of their phases.

Why should some products that come in the form of suspensions be shaken, for example, fruit juice?

What volume of 0.230 M HNO3 react with 49.0 ml of 0.330M Na2CO3 in the following Reaction : 2HNO3 (aq) + Na2CO3 (aq) 2NaNO3 (aq) + H2O (l) + CO2 (g

Hydrogen peroxide decomposes to water and oxygen by the following reaction H2O2 H20 O2 At 40C, the following data was taken for initial rates of reactions HO2 molesliter initial rate ( Mmin) 1.93 x 104 3.86 x 104 5.79 x 104 0.1000 0.2000 0.3000 a) What is the order of the reaction b) Write the rate law. c) Calculate the rate constant. d)

Calculate the amount of heat released from combustion of 1g of wood. The heat capacity of the bomb calorimeter is 9.96 kJC. kJ

Indicate the characteristics of the o- in the carbonyl. And an example.

A sample of CO; with n = 2.0 mol has a fixed volume of 15.0 dm' at 300 K. An amount of heat is supplied and it is equal to 2.35 kJ. Due to this addition of heat, the temperature increases to 341 K. Assume that CO2 is described by the van der Waals equation of state, determine AU, AH and W in Joules.

What volume in Liters would a 0.871 gram sample of air occupy if the density of air is 1.29 g/L?

Q.1: Explain various methods of teaching of chemistry? Which method is best for teaching Chemistry and why? Explain with reason.

Explain the difference between Aims and Objectives of teaching chemistry?

Q.3: Explain feature of lesson plane. Give a sample lesson plane of topic from chemistry?

Explain principles of selection of teaching Aids? How these Aids make teaching chemistry effective?

Q.5: Explain the Piagetian theory of cognitive development? Explain its stages.

With relevant equation, show how you could use butyllithium to prepare solutions containing (1) Lithium diethylamine, (2) Lithium 1-hexanolate (3) Lithium benzenethiolate

The initial concentrations for the following reaction are POCI, 0.049 M, H, 0.052 M, PH,1 0.073 M, HCI 0.081 M and H,0 0.060 M. The equilibrium concentration of HCl is 0.063 M. Calculate the equilibrium constant, K. POCI3 (g) 4 H2 (g) PH3 (g) 3 HCI (g) H2O (g)

The ireversible gasphase nonelementary reaction A 2B C is to be carried out isothermally in a constantpressure batch reactor. The feed is at a temperature of 227C, a pressure of 1013 kPa, and its composition is 33.3 A and 66.7 B. Laboratory data taken under identical conditions are as follows (note that at X 0, rA 0.00001) ra (moldm s) x 10

A waste containing 50 mg/L of Zn2+ will be treated by hydroxide precipitation. Ca(OH)2 will be added to precipitate all but 1 mg/L of the zinc. (a) How high the pH must be raised to accomplish this? (b) How much hydroxide sludge with water content of 94% is generated per liter of waste? (c) Calculate the theoretical amount of Ca(OH)2 required per

Fill in the missing products and reagents for each step of the synthetic scheme A G heat HO OH OH 1. B 2. H30 2. H3O F SOCI2 D E OH H2SO4 NH3 HO. P4010,A HO K J H30 1. PhMgBr CHCI3 2. H3O

1-The atomic number of an element A. the whole number nearest to its mass B. the number of protons in its nucleus C. the nearest whole number of hydrogen atoms having the same mass as a single atom of the given element D. the number of neutrons in its nucleus E. its order of discovery 2 -The isotopes of an element A. cannot be separated at all B.

6 -The half -life of a given nuclear disintegration A B A. depends on the initial number of A atoms B. depends on the initial number of B atoms C. is an exponentially increasing function of time D. is an exponentially decreasing function of time E-none of the above 7. Of the three common types of radiation (alpha, beta, gamma) from radioactive

11 -A large collection of nuclei are undergoing alpha decay. The rate of decay at any instant is proportional to: A. the number of un-decayed nuclei present at that instant B. the time since the decays started C. the time remaining before all have decayed D. the half-life of the decay E. the average time between decays 12 .Of the three common

Show graphically what is the effect of temperature on the rate of biological, normal, and explosive reactions.

Write the integrated rate equations for zero-order, first, second and third-order reactions along with plots of integrated rate equations.

Is it justified to compare the free energy change of two reactions and conclude one is more favorable than the other?

What are the activity coefcients for iron(III) and sulfate in an aqueous solution of 10 mM sulfuric acid, 5 mM calcium sulfate, and 3 mM iron(III) chloride?

Calculate the volume in liters that occupies 7.40 grams of NH3 to STP.