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 25.0 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 1.50 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(g) + B(g) → 3 C(g), b. when A is decreasing at a rate of 0.100 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. a. Use the graph to calculate each quantity: (ii) the instantaneous rate of the reaction at 25 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?

a. first-order reaction

b. second-order reaction

c. zero-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)? d. By what factor does the reaction rate change if [B] is doubled (and the other reactant concentrations are held constant)? e. By what factor does the reaction rate change if [C] is doubled? f. By what factor does the reaction rate change if the concentrations of all three reactants are doubled?

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. c. By what factor does the reaction rate change if [A] is doubled (and the other reactant concentrations are held constant)? d. By what factor does the reaction rate change if [B] is doubled? e. By what factor does the reaction rate change if [C] is doubled? f. By what factor does the reaction rate change if [C] is doubled (and the other reactant concentrations are held constant)?