2. For the reaction: 2HI → H, + I, the 1 d[HI] 2 dt (a) the rate of formation of HI (b) the rate of disappearance of HI (c) the instantaneous rate of the reaction (d) the average rate of the reaction expression, represents 3. For reaction: 4A + B → 2C+2D, the only incorrect statement is (a) The rate of disappearance of B is one-fourth the rate of disappearance of A (b) The rate of appearance of C is half the rate of disappearance of B

2. For the reaction: 2HI → H, + I, the 1 d[HI] 2 dt (a) the rate of formation of HI (b) the rate of disappearance of HI (c) the instantaneous rate of the reaction (d) the average rate of the reaction expression, represents 3. For reaction: 4A + B → 2C+2D, the only incorrect statement is (a) The rate of disappearance of B is one-fourth the rate of disappearance of A (b) The rate of appearance of C is half the rate of disappearance of B

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter11: Chemical Kinetics

Section: Chapter Questions

Problem 1RQ: Define reaction rate. Distinguish between the initial rate, average rate, and instantaneous rate of...

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The hydrolysis of the sugar sucrose to the sugars glucose and fructose, C12H22O11+H2OC6H12O6+C6H12O6 follows a first-order rate equation for the disappearance of sucrose: Rate =k[C12H22O11] (The products of the reaction, glucose and fructose, have the same molecular formulas but differ in the arrangement of the atoms in their molecules.) (a) In neutral solution, k=2.11011s1 at 27 C and 8.51011s1 at 37 C. Determine the activation energy, the frequency factor, and the rate constant for this equation at 47 C (assuming the kinetics remain consistent with the Arrhenius equation at this temperature). (b) When a solution of sucrose with an initial concentration of 0.150 M reaches equilibrium, the concentration of sucrose is 1.65107M . How long will it take the solution to reach equilibrium at 27 C in the absence of a catalyst? Because the concentration of sucrose at equilibrium is so low, assume that the reaction is irreversible. (c) Why does assuming that the reaction is irreversible simplify the calculation in pan (b)?
The label on a bottle of 3% (by volume) hydrogen peroxide, H2O2, purchased at a grocery store, states that the solution should be stored in a cool, dark place. H2O2decomposes slowly over time, and the rate of decomposition increases with an increase in temperature and in the presence of light. However, the rate of decomposition increases dramatically if a small amount of powdered MnO- is added to the solution. The decomposition products are H2O and O2. MnO2 is not consumed in the reaction. Write the equation for the decomposition of H2O2. What role does MnO2 play? In the chemistry lab, a student substituted a chunk of MnO2 for the powdered compound. The reaction rate was not appreciably increased. WTiat is one possible explanation for this observation? Is MnO2 part of the stoichiometry of the decomposition of H2O2?
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What is the difference between average rate, initial rate, and instantaneous rate?
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