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20 Multiple Choice Questions on General Chemistry ll | CHEM 1120, Exams of Chemistry

Roane State Community College Chemistry

Material Type: Exam; Class: General Chemistry II; Subject: Chemistry; University: Roane State Community College; Term: Spring 2006;

Typology: Exams

Pre 2010

Uploaded on 08/17/2009

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CHEM 1120 - test 2 - spring 2006 Page 1

Circle the correct answer on the answer sheet. Here’s some information you might need:

F = 96 487 C mol

–1

R = 8.314 J mol

–1

E = E

– 0

log

Q at 25EC

1. Copper has a molar heat capacity of 23.9 J mol

--1

–1

. How much heat would it take to raise

the temperauture of 150 g of copper from 25EC to 150EC?

a. 0.295 kJ b. 4.48 kJ c. 7.05 kJ d. 2.32 kJ e. 8.46 kJ

Partial preview of the text

Download 20 Multiple Choice Questions on General Chemistry ll | CHEM 1120 and more Exams Chemistry in PDF only on Docsity!

Circle the correct answer on the answer sheet. Here’s some information you might need:

F = 96 487 C mol–1^ R = 8.314 J mol–1^ K–1^ E = E E – 0.^05 n^92 log 10 Q at 25EC

Copper has a molar heat capacity of 23.9 J mol--1K–1^. How much heat would it take to raise the temperauture of 150 g of copper from 25EC to 150EC? a. 0.295 kJ b. 4.48 kJ c. 7.05 kJ d. 2.32 kJ e. 8.46 kJ

At cruising speed of 70 mph on flat interstate a certain automobile engine produces 20 kJ s–1. The amount of power used to keep the steady speed is 5 kJ s–1. What is the heat flow with respect to the cooling system to maintain a steady engine temperature? a. –5 kJ s–1^ b. 15 kJ s–1^ c. –25 kJ s–1^ d. 25 kJ s–1^ e. –15 kJ s–

For the following reaction ∆Ho^ = –444.26 kJ mol–1^ and the ∆So^ = –60.4 J mol–1^ K–1^ and 298 K. Calculate the ∆Go^ at 298K. CH 3 CH 2 OH (g) + 8Cl 2 (g)! 2CCl 4 (g) + 6HCl (g) + Cl 2 O (g) The answer in kJ mol–1^ is: a. –504.7 b. –426.3 c. –462.3 d. +17.5 × 10^3 e. +17.

Calculate the ∆Ho^ at 298 K for the following reaction: CH 4 (g) + 2O 2 (g)! CO 2 (g) + 2H 2 O (g) The answer in kJ mol–1^ is: a. –951.9 b. –890.3 c. –560.5 d. –802.3 e. –597.

Calculate the equilibrium constant at 298 K for the following reaction given that the ∆Go^ = 27.15 kJ mol– CH 3 COOH (aq) ºººº CH 3 COO-^ + H+ a. 5.75 × 10^4 b. 1.74 × 10-5^ c. 1.011 d. 0.989 e. 2.71 × 10-

8. From bond energies, calculate the ∆H for the reaction: H 2 C=CH 2 + 3O 2! 2CO 2 + 2H 2 O

What is the relationship between the molar Gibbs’ free energy and the molar Gibbs’ free energy at standard conditions? a. ∆G = ∆G"^ – RT ln Q b. ∆E = q + w c. ∆H = ∆E – P∆V d. ∆G = ∆H"^ + T∆S" e. ∆G = ∆G"^ + RT ln Q

Calculate the standard cell potential (EE) for the following electrochemical cell at 25EC. Ag | Ag+(0.025 M) || Cu2+(2.0 M) | Cu a. +1.1415 V b. +0.4577 V c. –0.4577 V d. –1.1415 V e. +0.3419 V

How long must one run an electrochemical cell to plate out 50.0 g of nickel from a nickel sulfamate bath if the current used is 10.0 A? The reaction is: Ni(SO 3 NH 3 ) 2 + 2e–^ + 2H+^! Ni + 2HSO 3 NH 3 a. 34.6 min b. 9.14 hr c. 91.4 hr d. 4.57 hr e. 18.8 hr

What is the definition of standard conditions in thermodynamics? a. For gasses 1 atm, for solutes 1M, for solvents, solid and liquids 1 mole fraction b. For gasses 1 atm pressure and 273 K for all others 1 mole fraction c. 1 atm pressure and 298 K. d. For a closed system 1 atm pressure. For an open system 1 m^3 volume. e. For solids 0 K, for liquids or gasses 0 EC.

For the reaction N 2 + 3H 2! 2NH 3 the ∆H""""^ is –92.2 kJ mol–1^ and the ∆S""""^ is –198.7 J mol–1^ K–1^. What is the slope for the van’t Hoff plot? a. –1.11 × 10^4 K b. +1.11 × 10^4 K c. 11.1 K d. +23.9 K e. –23.9 K

What is the equation that one uses to calculate the equilibrium constant from thermodynamic data?

a. ln K = ∆ H ^ + T∆S

b. K = ∆ H ^ − T∆S

K e RT

−∆^ θ

d. K = E + P ∆V

e. K = eE^ θ^ +^ P^ ∆V

Which of the following is the cell diagram for the Leclanché dry cell? a. Cd | Cd(OH) 2 | OH–^ | Ni(OH) 2 | NiO 2 (s)| inert (Ni) b. Zn | Zn2+^ || NH 4 +^ , NH 3 | Mn 2 O 3 | MnO 2 | inert (C) c. Pb | PbSO 4 (s)| H 2 SO 4 | PbSO 4 (s) | PbO 2 | Inert(Pb) d. Zn(Hg) | ZnO | OH- | HgO | Hg(l) e. Cu(impure) | Cu2+^ | Cu(purer)

What should be the entropy of pure zinc in J mol–1^ K–1^ at 0 K? a. 41.6 b. 12.4 c. 0.140 d. 20.8 e. 0