Textbook Question
Consider the reaction A + B → C + D. Is each of the following statements true or false? (c) If the reaction is an elementary reaction, the rate law of the reverse reaction is first order.
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Ch.14 - Chemical Kinetics
Chapter 14, Problem 92
You perform a series of experiments for the reaction A → B + C and find that the rate law has the form rate = k[A]^x. Determine the value of x in each of the following cases: (a) There is no rate change when [A] is tripled. (b) The rate increases by a factor of 9 when [A] is tripled. (c) When [A] is doubled, the rate increases by a factor of 8.
Verified step by step guidance1
Step 1: Understand the rate law expression. The rate law for the reaction is given as rate = k[A]^x, where k is the rate constant, [A] is the concentration of reactant A, and x is the order of the reaction with respect to A.
Step 2: Analyze case (a). If there is no rate change when [A] is tripled, it implies that the rate is independent of [A]. Therefore, x must be 0, as any change in [A] does not affect the rate.
Step 3: Analyze case (b). If the rate increases by a factor of 9 when [A] is tripled, set up the equation: (3[A])^x = 9[A]^x. Simplify to find x by solving 3^x = 9.
Step 4: Analyze case (c). If the rate increases by a factor of 8 when [A] is doubled, set up the equation: (2[A])^x = 8[A]^x. Simplify to find x by solving 2^x = 8.
Step 5: Conclude the values of x for each case based on the simplified equations from steps 2, 3, and 4.
Related Practice
Textbook Question
The reaction 2 NO(g) + O2(g) → 2 NO2 (g) is second order in NO and first order in O2. When [NO] = 0.040 M, and 3O24 = 0.035 M, the observed rate of disappearance of NO is 9.3⨉10-5 M/s. (b) What is the value of the rate constant?
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Textbook Question
The reaction 2 NO(g) + O2(g) → 2 NO2 (g) is second order in NO and first order in O2. When [NO] = 0.040 M, and 3O24 = 0.035 M, the observed rate of disappearance of NO is 9.3⨉10-5 M/s. (c) What are the units of the rate constant?
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Textbook Question
Consider the following reaction between mercury(II) chloride and oxalate ion: 2 HgCl21aq2 + C2O4 2 - 1aq2¡2 Cl - 1aq2 + 2 CO21g2 + Hg2Cl21s2 The initial rate of this reaction was determined for several concentrations of HgCl2 and C2O4 2 -, and the following rate data were obtained for the rate of disappearance of C2O4 2 - : Experiment 3HgCl2 4 1M 2 3C2o4 24 1M 2 Rate 1M,s2 1 0.164 0.15 3.2 * 10-5 2 0.164 0.45 2.9 * 10-4 3 0.082 0.45 1.4 * 10-4 4 0.246 0.15 4.8 * 10-5 (c) What is the reaction rate when the initial concentration of HgCl2 is 0.100 M and that of C2O4 2- is 0.25 M if the temperature is the same as that used to obtain the data shown?
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Open Question
The following kinetic data are collected for the initial rates of a reaction 2X + Z → products: Experiment [X] (M) [Z] (M) Rate (M/s) 1 0.25 0.25 4.0 * 10^1 2 0.50 0.50 3.2 * 10^2 3 0.50 0.75 7.2 * 10^2. (c) What is the reaction rate when the initial concentration of X is 0.75 M and that of Z is 1.25 M?
Textbook Question
The reaction 2 NO2¡2 NO + O2 has the rate constant k = 0.63 M- 1s - 1. (b) If the initial concentration of NO2 is 0.100 M, how would you determine how long it would take for the concentration to decrease to 0.025 M?
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