Estimate the rate of the reaction, H*(aq) + OH (aq) – H20() given that the rate law for the reaction is rate = (1.3 x 1011 L mol1s1)[OH¯][H*] for neutral water, where [H*] = 1.0 x 104 M and [OH] = 1.0 x 1o 10 M. (Express your answer in units of mol L1 s1.) rate = mol L-1s1

Estimate the rate of the reaction, H(aq) + OH (aq) – H20() given that the rate law for the reaction is rate = (1.3 x 1011 L mol1s1)[OH¯][H] for neutral water, where [H*] = 1.0 x 104 M and [OH] = 1.0 x 1o 10 M. (Express your answer in units of mol L1 s1.) rate = mol L-1s1

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

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Cc.83.
Under certain conditions the rate of this reaction is zero order in ammonia with a rate constant of 0.0078 M·s: 2 NH; (g) → N, (g) +3 H, (g) Suppose a 400. mL flask is charged under these conditions with 150. mmol of ammonia. How much is left 10. s later? You may assume no other reaction is important. Be sure your answer has a unit symbol, if necessary, and round it to 2 significant digits.
Consider the following reaction:2 NO(g) + 2 H2(g)--->N2(g) + 2 H2O(g)(a) The rate law for this reaction is first order in H2 andsecond order in NO. Write the rate law. (b) If the rateconstant for this reaction at 1000 K is 6.0 x 104 M-2 s-1,what is the reaction rate when [NO] = 0.035 M and[H2] = 0.015 M? (c) What is the reaction rate at 1000 Kwhen the concentration of NO is increased to 0.10 M,while the concentration of H2 is 0.010 M? (d) What is thereaction rate at 1000 K if [NO] is decreased to 0.010 M and[H2] is increased to 0.030 M?
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Consider the following reaction: 2 NO(g) + 2 H2(g) N2(g) + 2 H2O(g) (a) The rate law for this reaction is second order in NO(g) and first-order in H2(g). What is the rate law for this reaction? (b) If the rate constant for this reaction at a certain temperature is 9.70e+04, what is the reaction rate when [NO(g)] = 0.0560 M and [H2(g)] = 0.119 M?Rate = M/s.(c) What is the reaction rate when the concentration of NO(g) is doubled, to 0.112 M while the concentration of H2(g) is 0.119 M?Rate = M/s
15.For the reaction, 2H,S(g) + 0,(g) 2S(s) + 2H,0(1), which one of the following statements is absolutely true? (a) The reaction is first order with respect to H,S and second order with respect to O (b) The reaction is fourth order overall. (c) The rate law is: rate = k[H,S][0,]. %3D (d) The rate law is: rate = k[H,S][O,]. %3D (e) The rate law cannot be determined from the information given.
If tripling the concentration of a single reactant R in a multi-reactant reaction (while leaving all other conditions unchanged) leads to a nine−fold increase in rate, it can be deduced
The reaction O₂(g) + 2 NO(g) → 2 NO₂(g) was studied at a certain temperature with the following results: (a) What is the rate law for this reaction? O Ratek [0₂(9)] [NO(g)] O Ratek [0₂(9)]² [NO(g)] O Rate = k [0₂(9)] [NO(g)]² O Ratek [0₂(9)]² [NO(g)]² O Ratek [0₂(9)] [NO(g)]³ O Rate = k [O₂(g)]* [NO(g)] (b) What is the value of the rate constant? Experiment [0₂(9)] (M) 0.0235 0.0235 0.0470 0.0470 [NO(g)] (M) 0.0235 0.0470 0.0235 0.0470 Rate (M/S) 0.158 0.633 0.317 1.27 (c) What is the reaction rate when the concentration of O₂(g) is 0.0318 M and that of NO(g) is 0.0649 M if the temperature is the same as that used to obtain the data shown above?
The rate law for the reaction 2NO(g) + 2H₂(g) → N₂(g) +2H₂O(g) is rate = k[NO]²[H₂] If the rate of reaction is 7.00 x 10-3 mol L¹s ¹ when the concentrations of NO and H₂ are both 1.8 x 106 mol L-1, what is the value of the rate constant and what are the units for the rate constant?, k= i 3.8 x 1015 L³ mol-3 s-1 L² mol-² 5-1 S-1 OL mol-¹ s-1 mol L-15-1 e Textbook and Media Hint Save for Later Attempts: 3 of 15 used Submit Answer
rate constant 1 H₂(g) + 2NO(g) N₂O(g) + H₂O(g) k₁ 2 H₂(g) + N₂O(g) → N₂(g) + H₂O(g) k₂ Suppose also k₁«k₂. That is, the first step is much slower than the second. Write the balanced chemical equation for the overall chemical reaction: Write the experimentally- observable rate law for the overall chemical reaction. rate = k Note: your answer should not contain the concentrations of any intermediates. Express the rate constant k for the overall chemical reaction in terms of k1, K₂, and (if necessary) the rate constants k-1 and k-2 for the reverse of the two elementary reactions in the mechanism. step elementary reaction t k = A 00 X
The reaction 2A + 2B → M+ N has the rate law: Rate = k[A]². At 25°C, k = 0.0107 L mol-1 s1. If the initial concentrations of A and B are 0.314 M and 0.582 M, respectively Your answer is correct. (a) What is the half-life of the reaction? 297. seconds Hint Assistance Used Your answer is partially correct. (b) What will be the concentrations of A and B after 30.0 minutes? [A] = 0.0446 M [B] = i 0.048 ! M
The gas phase decomposition of dinitrogen pentoxide at 335 K N2O5(g) → 2 NO,(g)+% 02(g) is first order in N,Og. During one experiment it was found that when the initial concentration of N,0, was 8.25x10 M, the concentration of N,Os dropped to 1.42x10 M after 251.0 s had passed. Based on this experiment, the rate constant for the reaction is