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2. A first order reaction has a half-life of 5.0 seconds. If the concentration of the reactant was originally 8.00 M, how long will it take to reach a concentration of 1.00 M? (A) 3.0 seconds (B) 15. seconds (C) 8.0 seconds (D) None of these

2. A first order reaction has a half-life of 5.0 seconds. If the concentration of the reactant was originally 8.00 M, how long will it take to reach a concentration of 1.00 M? (A) 3.0 seconds (B) 15. seconds (C) 8.0 seconds (D) None of these

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Solve question 2. They deal with the first order reaction. 

1. The rate constant of a reaction has units of 1/M-s. What is the order of its rate law? (A) O (B) 1 (C) 2 (D) Some other order 2. A first order reaction has a half-life of 5.0 seconds. If the concentration of the reactant was originally 8.00 M, how long will it take to reach a concentration of 1.00 M? (A) 3.0 seconds (B) 15. seconds (C) 8.0 seconds (D) None of these (A) It is doubled (C) It is four times as fast 3. The rate expression for a reaction is: rate = k [A] [B]. The temperature is held constant. The initial concentrations are changed. [A] is halved. How does the new initial rate compare to the old initial rate? (B) It is one quarter as fast (D) It is halved (E) It is not changed 4. For the chemical equation, A + 2B 3 C, the rate of disappearance of B was measured and found to be 0.500 M/s. What is the rate of appearance of C? (A) 0.500 M/s (B) 0.250 M/s (C) 0.750 M/s (D) 0.333 M/s 5. Step 1, NO (g) + O. (g) → NO₂ (g) + O₂(g) Step 2, O (g) + NO₂ (g) → NO (g) + O₂ (g) If the reaction, O(g) + O. (g) → 2 O₂ (g) occurs using the above 2 step process, which of the following is true?
Transcribed Image Text:1. The rate constant of a reaction has units of 1/M-s. What is the order of its rate law? (A) O (B) 1 (C) 2 (D) Some other order 2. A first order reaction has a half-life of 5.0 seconds. If the concentration of the reactant was originally 8.00 M, how long will it take to reach a concentration of 1.00 M? (A) 3.0 seconds (B) 15. seconds (C) 8.0 seconds (D) None of these (A) It is doubled (C) It is four times as fast 3. The rate expression for a reaction is: rate = k [A] [B]. The temperature is held constant. The initial concentrations are changed. [A] is halved. How does the new initial rate compare to the old initial rate? (B) It is one quarter as fast (D) It is halved (E) It is not changed 4. For the chemical equation, A + 2B 3 C, the rate of disappearance of B was measured and found to be 0.500 M/s. What is the rate of appearance of C? (A) 0.500 M/s (B) 0.250 M/s (C) 0.750 M/s (D) 0.333 M/s 5. Step 1, NO (g) + O. (g) → NO₂ (g) + O₂(g) Step 2, O (g) + NO₂ (g) → NO (g) + O₂ (g) If the reaction, O(g) + O. (g) → 2 O₂ (g) occurs using the above 2 step process, which of the following is true?
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