For the reaction equation below, experimentally determined rate law is R = k [X] [Y₂1². Drag and drop the appropriate choices to fill in the correct answers for the following questions at a given temperature: X (g) + Y2 (g) XY (g) + Y (g) a) b) c) What would happen to the rate of the reaction if [Y₂] is tripled? What would happen to the rate of the reaction if [X] is doubled? What would happen to the rate of the reaction if [X] decreased by half and [Y₂] is doubled? B

For the reaction equation below, experimentally determined rate law is R = k [X] [Y₂1². Drag and drop the appropriate choices to fill in the correct answers for the following questions at a given temperature: X (g) + Y2 (g) XY (g) + Y (g) a) b) c) What would happen to the rate of the reaction if [Y₂] is tripled? What would happen to the rate of the reaction if [X] is doubled? What would happen to the rate of the reaction if [X] decreased by half and [Y₂] is doubled? B

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

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
5.) For the reaction X + Y ↓ Z; the reaction rate is found to depend only upon the concentration of X. A plot of 1/[X] verses time gives a straight line. What is the rate law for this reaction?
H2 reacts with ClF. Someone thinks this is the mechanism: H2(g) + ClF(g) → HCl(g) + HF(g) HCl(g) + ClF(g) → Cl2(g) + HF(g) (a) Write the balanced equation for the overall reaction. (b) Identify any intermediates in the mechanism, if any. (c) identify and catalysts in the mechanism, if any. (d) Write rate laws for each elementary reaction in the mechanism. (e) If the first step is slow and the second one is fast, what rate law do you expect to be observed for the overall reaction?
A proposed mechanism for the decomposition of hydrogen peroxide consists of three elementary steps: (1) H₂O2(g) →>> 2OH(g) (2) H₂O2(g) + OH(g) → H₂O(g) + HO₂(g) (3) HO₂(g) + OH(g) → H₂O(g) + O₂(g) If the rate law for the reaction is first order in H₂O2, which step in the mechanism is the rate-determining step? O Step 1 O None of the steps O Step 3 O Impossible to determine Steps 1 and 2 O All of the steps O Step 2 Hint: The slowest step in a mechanism determines the rate law. From each elementary reaction we can write a rate-law expression. Submit Question
Consider the following balanced chemical equation: H2O2 (aq) + 3 r (aq) + 2 H (aq) >l (aq) + 2 H,O (I) If the concentration of iodide (la) decreases from 0.718 M to 0.426 M in the first 15 seconds, what is the rate of reaction? (A) (B) (C) (D) (E) 0.0195 M/s 0.292 M/s -0.00195 M/s 0.00649 M/s 0.0973 M/s
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 rate = k (X]/[Y]/² [Z] -1 (b) 1/2 X Y Overall (c) rate = k [Y] X Y Overall
The following mechanism has been proposed for the atmospheric destruction of ozone, O3 (g):O3 (g) + NO (g) --> O2 (g) + NO2 (g) (slow)NO2 (g) + O (g) --> NO (g) + O2 (g) (fast)a) Write the equation for the overall balanced reaction. b) Write the rate law predicted by this reaction mechanism.
2.) The reaction below was found to have the rate law, rate = k[A][B] 2. For EACH of the scenarios below indicate by what factor the rate of reaction will increase: 2 A + B ↓ products a.) While holding the concentration of A constant, the concentration of B was increased from x to 3x. b.) While holding the concentration of B constant, the concentration of A was increased from x to 3x.c.) The concentrations of BOTH A and B were increased from x to 3x at the same time.
Gen Chemistry : Please see attached image
1)The reaction A -> product is second order. If the initial concentration of A is 0.436 M and, after 52.8 seconds have elapsed, the concentration of A has fallen to 0.0476 M, what is the rate constant of the reaction? 2) consider the following reaction at equilibrium.2CO2 (g) ->_<-- 2CO (g) + O2 (g) H° = -514 kJLe Châtelier's principle predicts that the equilibrium partial pressure of CO (g) can be maximized by carrying out the reaction ________.