2(a) Carbonic acid decomposes to water and carbon dioxide according to the following reaction: H₂CO3 → H₂O + CO₂ Write the equation of the reaction rate for this reaction in terms of the disappearance of H2CO3. 2(b) Does the value of the rate constant, k, depend on the concentration of the reactants? Briefly explain your answer (or show an equation that explains your answer). 2(c) Doubling the concentration of a reactant increases the rate of the reaction four times. What is the order of the reaction with respect to that reactant? (Show your calculation)

2(a) Carbonic acid decomposes to water and carbon dioxide according to the following reaction: H₂CO3 → H₂O + CO₂ Write the equation of the reaction rate for this reaction in terms of the disappearance of H2CO3. 2(b) Does the value of the rate constant, k, depend on the concentration of the reactants? Briefly explain your answer (or show an equation that explains your answer). 2(c) Doubling the concentration of a reactant increases the rate of the reaction four times. What is the order of the reaction with respect to that reactant? (Show your calculation)

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...

See similar textbooks

Similar questions

Consider the following reaction: 1. 2 N,O5 (g) → 4 NO, (g) + O, (g) The initial concentration of N2O5 was 0.48 mol/L, and 25 minutes after initiating the reaction, all of the N,Os has been consumed. (a) Calculate the average rate of the reaction over this 25-minute time interval. (b) Is it correct to assume that the rate law is Rate = k[N,O5]² based on the balanced chemical equation? Briefly explain your answer.
4. Although the depletion of stratospheric ozone threatens life on Earth today, its accumulation was one of the crucial processes that allowed life to develop in prehistoric times: ( WRITE YOUR ANSWERS IN YOUR SOLUTIONS PAGE) 302(g) → 203 (g) (a) Express the reaction rate in terms of [02] and [03]. (b) At a given instant, the reaction rate in terms of [02] is 2.17.10-5 mol/L-s. What is it in terms of [03]?
Although the depletion of stratospheric ozone threatens life on Earth today, its accumulation was one of the crucial processes that allowed life to develop in prehistoric times: 3O₂(g) →2O₃(g) (a) Express the reaction rate in terms of [O₂] and [O₃].(b) At a given instant, the reaction rate in terms of [O₂] is 2.17X10⁻⁵mol/L s. What is it in terms of [O₃]?
How will each of the following affect the rate of the reaction, CO(g) + NO2(g) → CO2(g) + NO(g), if the rate law for the reaction is rate = k [NO2] [CO]? (a) increasing the pressure of NO2 from 0.4 atm to 1.2 atm (b) increasing the concentration of CO from 0.03 M to 0.09 M
Assume that the formation of nitrogen dioxide: 2NO(g) + O2(g) 2NO2(g) is an elementary reaction. (a) Write the rate law for this reaction. (b) A sample of air at a certain temperature is contaminated with 2.0 ppm of NO by volume. Under these conditions, can the rate law be simplified? If so, write the simplified rate law. (c) Under the conditions described in part (b), the half-life of the reaction has been estimated to be 6.4 × 103 min. What would the half-life be if the initial concentration of NO were 10 ppm?
In a reaction, A + B → product, rate is doubled when the concentration of B is doubled, and rate increases by a factor of 8 when the concentration of both the reactants (A and B) are doubled, rate law for the reaction can be written as (a) rate = k[A][B]² (b) rate = k[A][B]² (d) rate= k[4][B] (c) rate k[A][B] =
Which of the following statements about rate laws is FALSE? A) Rate laws can only be determined experimentally. B) Rate laws tell us information about the mechanism of the chemical reaction under study. C) The rate law for the chemical reaction A + B + 20 –D must be rate = k[A][B][C]² %3D D)A rate law can only be written for the elementary reactions of a given chemical reaction.
For each of the rate laws below, what is the order of the reaction with respect to the hypothetical substances X, Y, and Z? What is the overall order? (For each answer, enter an exact number as an integer or decimal.) (a) rate = k [X][Y][Z]² X Y Overall (b) rate = k (X]5 [Y]1.5Z]-1 Y Overall (c) rate = k [z]* Y Overall
6) For the reaction 3A + 2B2C + D + E, the initial reaction rate was measured for various initial concentrations of reactants. The following data were collected: Rate (M/s) 1.9 x 108 [A] (M) [B] (M) 1.0 x 10¹2 1.0 x 10¹1 9.5 x 108 5.0 x 10¹2 1.0 x 1011 3 5.7 x 108 1.0 x 10¹2 3.0 x 10¹1 a) Write the rate law for this reaction. rate=[A]*[B]Y 3 3.0 x 10" 1.0 x10¹2 y = ²/ 5.0×10 1.0x1010 X = = 1 1.0x10" 1.0 ×1010 5 3=1 b) What is the overall order of the reaction? c) Calculate the rate law constant, k (including units). x = = 1.0x10" 1.0 x 10" 1 lom C²
You and your lab partner are studying the rate of a reaction, A + B --> C. You make measurements of the initial rate under the following conditions: (b) For a reaction of the form, A + B + C --> reaction from the choices below. (a) Which of the following reactant concentrations could you use for experiment 3 in order to determine the rate law, assuming that the rate law is of the form, Rate = k [A] [B]Y? Choose all correct possibilities. O [A] = 0.2 and [B] = 1.0 O [A] = 0.4 and [B] = 1.0 O [A] = 0.8 and [B] = 0.5 O [A] = 0.6 and [B] = 0.5 O [A] = 0.2 and [B] = 1.5 O [A] = 0.4 and [B] = 0.5 O [A] = 0.4 and [B] = 1.5 O [A] = 1.0 and [B] = 0.5 O Rate = K[A][B][C] O Rate = K[A][C] O Rate = K[A]²[C] T O Rate = k[A][C]² O Rate = K[A]²[C]² O Rate = K[A]³ [c] O Rate = K[A][C]³ the following Experiment [A] (M) [B] (M) Rate (M/s) 0.5 0.5 The rate will be the original rate multiplied by a factor of 0.2 0.4 (c) By what factor will the rate of the reaction described in part (b) above change if the…
3(a) Substance A reacts according to a first order rate law with k = 5.0 x 10-5 s-13(a)(i) If the initial concentration of A is 1.00 M, what is the initial rate of the reaction? 3(a)(ii) What is the rate after 1 hour?
6. The rate constant for the reaction, 2 N₂O5 (g) → 4 NO2 (g) + O2 (g), doubles when the temperature is raised from 295.65 K to 300.62 K. (a) Determine the activation energy (in kJ/mol) for the reaction, assuming that the pre- exponential factor, A, in the Arrhenius equation is independent of temperature. (b) At what temperature would you predict this rate constant to increase by another factor of 10 relative to its value at 300.62 K?