Consider the reaction:

2 HBr (g) → H₂ (g) + Br₂ (g)

a. Express the rate of the reaction in terms of the change in concentration of each of the reactants and products.

Consider the reaction:

2 HBr (g) → H₂ (g) + Br₂ (g)

b. In the first 20.0 s of this reaction, the concentration of HBr dropped from 0.600 M to 0.512 M. Calculate the average rate of the reaction during this time interval.

Consider the reaction:

2 HBr (g) → H₂ (g) + Br₂ (g)

c. If the volume of the reaction vessel in part b was 1.25 L, what amount of Br₂ (in moles) was formed during the first 15.0 s of the reaction?

Consider the reaction: 2 N₂O( g) → 2 N₂(g) + O₂(g) a. Express the rate of the reaction in terms of the change in concentration of each of the reactants and products.

For the reaction 2 A(g) + B(g) → 3 C(g), a. Determine the expression for the rate of the reaction in terms of the change in concentration of each of the reactants and products.

For the reaction 2 A(gg) + B(g) → 3 C(g), b. when A is decreasing at a rate of 0.200 M/s, how fast is B decreasing? How fast is C increasing?

Consider the reaction: 8 H₂S(g) + 4 O₂(g) → 8 H₂O(g) + S₈(g) Complete the table.

Consider the reaction: C₄H₈( g) → 2 C₂H₄( g) The tabulated data were collected for the concentration of C₂H₄ as a function of time: a. What is the average rate of the reaction between 0 and 10 s? Between 40 and 50 s?

Consider the reaction: NO₂(g) → NO(g) + 1/2 O₂(g) The tabulated data were collected for the concentration of NO₂ as a function of time: a. What is the average rate of the reaction between 10 and 20 s? Between 50 and 60 s?

Consider the reaction: NO₂(g) → NO(g) + 1/2 O₂( g) The tabulated data were collected for the concentration of NO2 as a function of time: b. What is the rate of formation of O₂ between 50 and 60 s?

Consider the reaction: H₂(g) + Br₂(g) → 2 HBr(g) The graph shows the concentration of Br₂ as a function of time.

a. Use the graph to calculate each quantity: (i) the average rate of the reaction between 0 and 25 s

Consider the reaction: H₂(g) + Br₂(g) → 2 HBr(g) The graph shows the concentration of Br₂ as a function of time. a. Use the graph to calculate each quantity: (iii) the instantaneous rate of formation of HBr at 50 s

Consider the reaction: H₂( g) + Br₂( g) → 2 HBr( g) The graph shows the concentration of Br₂ as a function of time.

b. Make a rough sketch of a curve representing the concentration of HBr as a function of time. Assume that the initial concentration of HBr is zero

Consider the reaction: 2 H₂O₂(aq) → 2 H₂O(l ) + O₂( g) The graph shows the concentration of H₂O₂ as a function of time. Use the graph to calculate each quantity: d. If the initial volume of the H₂O₂ is 1.5 L, what total amount of O₂ (in moles) is formed in the first 50 s of reaction?

This graph shows a plot of the rate of a reaction versus the concentration of the reactant A for the reaction A → products. a. What is the order of the reaction with respect to A?

This graph shows a plot of the rate of a reaction versus the concentration of the reactant A for the reaction A → products. c. Write a rate law for the reaction including an estimate for the value of k.

This graph shows a plot of the rate of a reaction versus the concentration of the reactant.

a. What is the order of the reaction with respect to A?

This graph shows a plot of the rate of a reaction versus the concentration of the reactant.

b. Make a rough sketch of a plot of [A] versus time

This graph shows a plot of the rate of a reaction versus the concentration of the reactant.

c. Write a rate law for the reaction including the value of k.

What are the units of k for each type of reaction? b. second-order reaction

This reaction is first order in N₂O₅: N₂O₅(g) → NO₃(g) + NO₂(g) The rate constant for the reaction at a certain temperature is 0.053/s. a. Calculate the rate of the reaction when [N₂O₅] = 0.055 M

This reaction is first order in N₂O₅: N₂O₅(g) → NO₃(g) + NO₂(g) The rate constant for the reaction at a certain temperature is 0.053/s. b. What would the rate of the reaction be at the concentration indicated in part a if the reaction were second order? Zero order? (Assume the same numerical value for the rate constant with the appropriate units.)

A reaction in which A, B, and C react to form products is first order in A, second order in B, and zero order in C. b. What is the overall order of the reaction?

A reaction in which A, B, and C react to form products is first order in A, second order in B, and zero order in C c. By what factor does the reaction rate change if [A] is doubled (and the other reactant concentrations are held constant)?

A reaction in which A, B, and C react to form products is zero order in A, one-half order in B, and second order in C. a. Write a rate law for the reaction.

A reaction in which A, B, and C react to form products is zero order in A, one-half order in B, and second order in C. e. By what factor does the reaction rate change if [C] is doubled (and the other reactant concentrations are held constant)?

Consider the tabulated data showing the initial rate of a reaction (A → products) at several different concentrations of A. What is the order of the reaction? Write a rate law for the reaction including the value of the rate constant, k.

[A] (M) Initial Rate (M/s)

0.050 0.100

0.075 0.225

0.090 0.324

The tabulated data were collected for this reaction: CH3Cl( g) + 3 Cl2( g) ¡ CCl4( g) + 3 HCl( g

Write an expression for the reaction rate law and calculate the value of the rate constant, k. What is the overall order of the reaction?

Indicate the order of reaction consistent with each observation. a. The half-life of the reaction gets shorter as the initial concentration is increased.

Indicate the order of reaction consistent with each observation c. The half-life of the reaction gets longer as the initial concentration is increased.