QuestionStep 1: $\quad \mathrm{H}_{2}+\mathrm{IBr} \rightarrow \mathrm{HI}+\mathrm{HBr} \quad$ (slow)
Step 2: $\quad \mathrm{HI}+\mathrm{IBr} \rightarrow \mathrm{I}_{2}+\mathrm{HBr} \quad$ (fast)
A proposed mechanism for the reaction $\mathrm{H}_{2}+2 \mathrm{IBr} \rightarrow \mathrm{I}_{2}+2 \mathrm{HBr}$ is shown above. Two experiments were performed at the same temperature but with different initial concentrations. Based on this information, which of the following statements is correct?
A The rate of the reaction will undergo a 4 -fold increase in the experiment in which the initial concentrations of both HI and IBr were doubled.
B The rate of the reaction will undergo a 2 -fold increase in the experiment in which the initial concentrations of both HI and IBr were doubled.
C The rate of the reaction will undergo a 4 -fold increase in the experiment in which the initial concentrations of both $\mathrm{H}_{2}$ and IBr were doubled.
D The rate of the reaction will undergo a 8 -fold increase in the experiment in which the initial concentrations of both $\mathrm{H}_{2}$ and IBr were doubled.

Studdy Solution

STEP 1

1. The reaction mechanism is given in two steps, with the first step being slow and the second step being fast.
2. The rate-determining step is the slow step.
3. The rate law is determined by the rate-determining step.
4. The initial concentrations of reactants can affect the rate of the reaction.

STEP 2

1. Identify the rate-determining step.
2. Write the rate law based on the rate-determining step.
3. Analyze the effect of doubling the concentrations on the rate of the reaction.
4. Determine which statement is correct based on the analysis.

STEP 3

Identify the rate-determining step:
The rate-determining step is the slow step, which is:
$\mathrm{H}_{2} + \mathrm{IBr} \rightarrow \mathrm{HI} + \mathrm{HBr}$

STEP 4

Write the rate law based on the rate-determining step:
The rate law is determined by the reactants in the slow step:
$\text{Rate} = k[\mathrm{H}_{2}][\mathrm{IBr}]$

STEP 5

Analyze the effect of doubling the concentrations on the rate of the reaction:
- If both $[\mathrm{H}_{2}]$ and $[\mathrm{IBr}]$ are doubled, the rate becomes:
$\text{New Rate} = k[2\mathrm{H}_{2}][2\mathrm{IBr}] = 4k[\mathrm{H}_{2}][\mathrm{IBr}]$
This results in a 4-fold increase in the rate.

STEP 6

Determine which statement is correct based on the analysis:
The correct statement is:
C The rate of the reaction will undergo a 4-fold increase in the experiment in which the initial concentrations of both $\mathrm{H}_{2}$ and $\mathrm{IBr}$ were doubled.

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Studdy Solution

STEP 1

1. The reaction mechanism is given in two steps, with the first step being slow and the second step being fast.
2. The rate-determining step is the slow step.
3. The rate law is determined by the rate-determining step.
4. The initial concentrations of reactants can affect the rate of the reaction.

STEP 2

1. Identify the rate-determining step.
2. Write the rate law based on the rate-determining step.
3. Analyze the effect of doubling the concentrations on the rate of the reaction.
4. Determine which statement is correct based on the analysis.

STEP 3

Identify the rate-determining step:
The rate-determining step is the slow step, which is:
$\mathrm{H}_{2} + \mathrm{IBr} \rightarrow \mathrm{HI} + \mathrm{HBr}$

STEP 4

Write the rate law based on the rate-determining step:
The rate law is determined by the reactants in the slow step:
$\text{Rate} = k[\mathrm{H}_{2}][\mathrm{IBr}]$

STEP 5

Analyze the effect of doubling the concentrations on the rate of the reaction:
- If both $[\mathrm{H}_{2}]$ and $[\mathrm{IBr}]$ are doubled, the rate becomes:
$\text{New Rate} = k[2\mathrm{H}_{2}][2\mathrm{IBr}] = 4k[\mathrm{H}_{2}][\mathrm{IBr}]$
This results in a 4-fold increase in the rate.

STEP 6

Determine which statement is correct based on the analysis:
The correct statement is:
C The rate of the reaction will undergo a 4-fold increase in the experiment in which the initial concentrations of both $\mathrm{H}_{2}$ and $\mathrm{IBr}$ were doubled.

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Studdy Solution

STEP 1

1. The reaction mechanism is given in two steps, with the first step being slow and the second step being fast.2. The rate-determining step is the slow step.3. The rate law is determined by the rate-determining step.4. The initial concentrations of reactants can affect the rate of the reaction.

STEP 2

1. Identify the rate-determining step.2. Write the rate law based on the rate-determining step.3. Analyze the effect of doubling the concentrations on the rate of the reaction.4. Determine which statement is correct based on the analysis.

STEP 3

Identify the rate-determining step:The rate-determining step is the slow step, which is:H2+IBr→HI+HBr \mathrm{H}_{2} + \mathrm{IBr} \rightarrow \mathrm{HI} + \mathrm{HBr} H2​+IBr→HI+HBr

STEP 4

Write the rate law based on the rate-determining step:The rate law is determined by the reactants in the slow step:Rate=k[H2][IBr] \text{Rate} = k[\mathrm{H}_{2}][\mathrm{IBr}] Rate=k[H2​][IBr]

STEP 5

STEP 6

Determine which statement is correct based on the analysis:The correct statement is:C The rate of the reaction will undergo a 4-fold increase in the experiment in which the initial concentrations of both H2\mathrm{H}_{2}H2​ and IBr\mathrm{IBr}IBr were doubled.

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1. The reaction mechanism is given in two steps, with the first step being slow and the second step being fast.
2. The rate-determining step is the slow step.
3. The rate law is determined by the rate-determining step.
4. The initial concentrations of reactants can affect the rate of the reaction.

1. Identify the rate-determining step.
2. Write the rate law based on the rate-determining step.
3. Analyze the effect of doubling the concentrations on the rate of the reaction.
4. Determine which statement is correct based on the analysis.

Identify the rate-determining step:
The rate-determining step is the slow step, which is:
$\mathrm{H}_{2} + \mathrm{IBr} \rightarrow \mathrm{HI} + \mathrm{HBr}$

Write the rate law based on the rate-determining step:
The rate law is determined by the reactants in the slow step:
$\text{Rate} = k[\mathrm{H}_{2}][\mathrm{IBr}]$

Determine which statement is correct based on the analysis:
The correct statement is:
C The rate of the reaction will undergo a 4-fold increase in the experiment in which the initial concentrations of both $\mathrm{H}_{2}$ and $\mathrm{IBr}$ were doubled.