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

Chapter12: Chemical Kinetics

Section: Chapter Questions

Problem 5ALQ: Consider the following statements: In general, the rate of a chemical reaction increases a bit at...

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Consider the following statements: In general, the rate of a chemical reaction increases a bit at first because it takes a while for the reaction to get warmed up. After that, however, the rate of the reaction decreases because its rate is dependent on the concentrations of the reactants, and these are decreasing. Indicate everything that is correct in these statements, and indicate everything that is incorrect. Correct the incorrect statements and explain.
If a textbook defined a catalyst as "a substance that increases the rate of a reaction," would that definition be adequate?
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The reaction NO(g) + O,(g) — NO,(g) + 0(g) plays a role in the formation of nitrogen dioxide in automobile engines. Suppose that a series of experiments measured the rate of this reaction at 500 K and produced the following data; [NO] (mol L ’) [OJ (mol L 1) Rate = -A[NO]/Af (mol L_1 s-1) 0.002 0.005 8.0 X 10"'7 0.002 0.010 1.6 X 10-'6 0.006 0.005 2.4 X IO-'6 Derive a rate law for the reaction and determine the value of the rate constant.
Give at least two physical properties that might be used to determine the rate of a reaction.
The reaction 2 NO(g) + 2 H2(g) N2(g) + 2 H2O(g) was studied at 904 C, and the data in the table were collected. (a) Determine the order of the reaction for each reactant. (b) Write the rate equation for the reaction. (c) Calculate the rate constant for the reaction. (d) Find the rate of appearance of N2 at the instant when [NO] = 0.350 mol/L and [H] = 0.205 mol/L.
11.102 Suppose that you are studying a reaction and need to determine its rate law. Explain what you would need to measure in order to accomplish this in a single experiment, and how you could use graphical methods to get from the experimental data to a complete rate law.
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The hypothetical reaction, A + B —*C, has the rate law Rate = When [A] is doubled and [B] is held constant, the rate doubles. But the rate increases fourfold when [B] is doubled and [A] is held constant. What are the values of'x and y?
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In Chapter 3, we discussed the conversion of biomass into biofuels. One important area of research associated with biofuels is the identification and development of suitable catalysts to increase the rate at which fuels can be produced. Do a web search to find an article describing biofuel catalysts. Then, write one or two sentences describing the reactions being catalyzed, and identify the catalyst as homogeneous or heterogeneous.