Textbook Question
Consider a hypothetical reaction between A, B, and C that is first order in A, zero order in B, and second order in C. (e) By what factor does the rate change when the concentrations of all three reactants are tripled?
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Ch.14 - Chemical Kinetics
Chapter 14, Problem 31
Consider the following reaction: CH3Br(aq) + OH-(aq) → CH3OH(aq) + Br-(aq). The rate law for this reaction is first order in CH3Br and first order in OH-. When [CH3Br] is 5.0 * 10^-3 M and [OH-] is 0.050 M, the reaction rate at 298 K is 0.0432 M/s. (c) What would happen to the rate if the concentration of OH- were tripled? (d) What would happen to the rate if the concentration of both reactants were tripled?
Verified step by step guidance1
Identify the rate law for the reaction: The rate law is given as rate = k[CH3Br][OH^-], where k is the rate constant.
Determine the effect of tripling [OH^-]: Since the reaction is first order in OH^-, tripling [OH^-] will triple the rate of the reaction.
Calculate the new rate with tripled [OH^-]: Substitute the new concentration of OH^- (3 * 0.050 M) into the rate law to find the new rate.
Determine the effect of tripling both [CH3Br] and [OH^-]: Since the reaction is first order in both reactants, tripling both will increase the rate by a factor of 3 * 3 = 9.
Calculate the new rate with tripled [CH3Br] and [OH^-]: Substitute the new concentrations of both reactants (3 * 5.0 * 10^-3 M and 3 * 0.050 M) into the rate law to find the new rate.
Related Practice
Textbook Question
The decomposition reaction of N2O5 in carbon tetrachloride is 2 N2O5¡4 NO2 + O2. The rate law is first order in N2O5. At 64 C the rate constant is 4.82 * 10-3 s-1. (a) Write the rate law for the reaction.
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Textbook Question
Consider the following reaction: 2 NO1g2 + 2 H21g2¡N21g2 + 2 H2O1g2 (d) What is the reaction rate at 1000 K if [NO] is decreased to 0.010 M and 3H24 is increased to 0.030 M?
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Textbook Question
The react ion between ethyl bromide 1C2H5Br2 and hydroxide ion in ethyl alcohol at 330 K, C2H5Br1alc2 + OH- 1alc2¡ C2H5OH1l2 + Br - 1alc2, is first order each in ethyl bromide and hydroxide ion. When 3C2H5Br4 is 0.0477 M and 3OH- 4 is 0.100 M, the rate of disappearance of ethyl bromide is 1.7 * 10-7 M>s. (a) What is the value of the rate constant?
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Textbook Question
The react ion between ethyl bromide 1C2H5Br2 and hydroxide ion in ethyl alcohol at 330 K, C2H5Br1alc2 + OH- 1alc2¡ C2H5OH1l2 + Br - 1alc2, is first order each in ethyl bromide and hydroxide ion. When 3C2H5Br4 is 0.0477 M and 3OH- 4 is 0.100 M, the rate of disappearance of ethyl bromide is 1.7 * 10-7 M>s. (c) How would the rate of disappearance of ethyl bromide change if the solution were diluted by adding an equal volume of pure ethyl alcohol to the solution?
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1
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Textbook Question
The iodide ion reacts with hypochlorite ion (the active ingredient in chlorine bleaches) in the following way: OCl- + I- → OI- + Cl- . This rapid reaction gives the following rate data:
[OCl4-] (M) [I-] (M) Initial Rate (M,s)
1.5 * 10-3 1.5 * 10-3
1.36 * 10-4 3.0 * 10-3 1.5 * 10-3 2.72 * 10-4
1.5 * 10-3 3.0 * 10-3 2.72 * 10-4
(a) Write the rate law for this reaction.
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