Chem1b-E1-Prac

Chem1b-E1-Prac - Chapter 15 Principles of Reactivity:...

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142 Chapter 15 Principles of Reactivity: Chemical Kinetics 1. Rate constants usually a) decrease with time. b) increase with time. c) decrease with temperature. d) increase with temperature. e) are independent of time and temperature. Answer: d 2. Which of the statements concerning relative rates of reaction is correct for the decomposition of dinitrogen pentaoxide? 2 N 2 O 5 (g) 4 NO 2 (g) + O 2 (g) a) The rate of disappearance of N 2 O 5 is 1/2 the rate of appearance of O 2 . b) The rate of appearance of NO 2 is 1/4 the rate of appearance of O 2. c) The rate of disappearance of N 2 O 5 is 1/2 the rate of appearance of NO 2 . d) The rate of appearance of NO 2 equals the rate of appearance of O 2 . e) The rate of disappearance of N 2 O 5 equals the rate of appearance of NO 2 . Answer: c 3. Which of the following relationships are correct for the reaction of peroxydisulfate ion with iodide ion? S 2 O 8 2- (aq) + 3 I - (aq) 2 SO 4 (aq) + I 3 - (aq) a) - - 3 [ I] [ = - tt ∆∆ b) - - 3 [ [ - 3 =    c) - 4 [ I ] [SO] = 2   -     d) 2- - 28 [ = e) - 4 1 [I ] 1 - = 32 Answer: e
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143 4. Which of the following expressions relates the rates of reaction of NO(g) and Cl 2 (g) 2 NOCl(g) 2 NO(g) + Cl 2 (g) a) 2 [NO ] [C l] 2 = tt ∆∆    b) 2 1 [NO ] [C = 2 c) 2 1 [C - = 2 [NO] t t d) 2 - = [NO ] [C e) 2 [C = [NO] t t Answer: b 5. Ammonia can be formed by reacting nitrogen and hydrogen gases. N 2 (g) + 3 H 2 (g) 2 NH 3 (g) If the rate of disappearance of hydrogen is -2.7 × 10 -2 M/s, what is the rate of formation of ammonia? a) 1.8 × 10 M/s b) 2.7 × 10 M/s c) 4.0 × 10 M/s d) 5.4 × 10 M/s e) 8.1 × 10 M/s Answer: a 6. Given the initial rate data for the decomposition reaction, A 2B determine the rate expression for the reaction. [A], M - D [A]/ D t M/s 0.125 5.14 × 10 2 0.175 1.01 × 10 3 0.250 2.06 × 10 3 a) 3 - [A] = 4.11 × 10 [A] t b) 32 = 4.11 × 10 [A] t c) 42 = 3.29 × 10 [A] t d) 2 = 5.14 10 t × e) 4 = 3.29 × 10 [A] t
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144 Answer: c 7. Given the initial rate data for the reaction A + B C, determine the rate expression for the reaction. [A], M [B], M D [C]/ D t (initial) M/s 0.10 0.20 4.20 × 10 -4 0.10 0.40 1.68 × 10 -3 0.20 0.40 3.36 × 10 a) 2 [C] = 0.105[A][B] t b) 2 [C] = 0.0210[A][B] t c) 2 [C] = 0.0210[A ] [B] t d) [C] = 0.105[A][B] t e) 2 [C] = 0.105[A] [B] t Answer: a 8. Given the initial rate data for the reaction A + B C, determine the rate expression for the reaction. [A], M [B], M D [C]/ D t (initial) M/s 0.25 0.15 1.23 × 10 0.25 0.25 3.42 × 10 0.50 0.15 2.46 × 10 a) [C] = 0.0328[A][B] t b) [C] = 0.0547[A][B] t c) 2 [C] = 0.219[A][B] t d) 2 [C] = 0.0547[A][B] t e) 2 [C] = 0.219[A] [B] t Answer: c
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145 9. Given the initial rate data for the reaction A + B C, determine the rate expression for the reaction. [A], M [B], M D [C]/ D t (initial) M/s 0.125 0.105 1.23 × 10 -1 0.125 0.315 3.69 × 10 0.250 0.105 1.23 × 10 a) 2 [C] = 75.0[A] [B] t b) [C] = 1.17[B] t c) 2 [C] = 1.17[A] [B] t d) 2 [C] = 11.2[B] t e) [C] = 11.2[A] t Answer: b 10. What is the overall order of the reaction CO(g) + NO 2 (g) CO 2 (g) + NO(g) if it proceeds via the following rate expression?
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This note was uploaded on 10/27/2010 for the course CHEM 337 taught by Professor Kim during the Fall '10 term at CSU Sacramento.

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Chem1b-E1-Prac - Chapter 15 Principles of Reactivity:...

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