Consider the following reversible reaction: H2(g) + I2(g) ⇌ 2HI(g) The rate law for the forward reaction can be expressed as: Rate = k[H2][I2] where k is the rate constant, [H2] is the concentration of hydrogen gas, and [I2] is the concentration of iodine gas. You conduct an experiment to study the kinetics of this reaction at a certain temperature. The initial concentrations of H2 and I2 are both set to 0.100 M, and the concentration of HI is monitored over time. The data collected from the experiment is shown in the table below: Time (s) [HI] (M) 0 0.000 100 0.040 200 0.072 300 0.096 400 0.116 500 0.132 (a) Calculate the average rate of the reaction between 100 s and 200 s. Show your calculations. (b) Determine the rate constant k for the forward reaction at this temperature using the average rate calculated in part (a). Show your calculations.
Consider the following reversible reaction: H2(g) + I2(g) ⇌ 2HI(g)
The rate law for the forward reaction can be expressed as: Rate = k[H2][I2] where k is the rate constant, [H2] is the concentration of hydrogen gas, and [I2] is the concentration of iodine gas.
You conduct an experiment to study the kinetics of this reaction at a certain temperature. The initial concentrations of H2 and I2 are both set to 0.100 M, and the concentration of HI is monitored over time. The data collected from the experiment is shown in the table below:
| Time (s) | [HI] (M) |
|---|---|
| 0 | 0.000 |
| 100 | 0.040 |
| 200 | 0.072 |
| 300 | 0.096 |
| 400 | 0.116 |
| 500 | 0.132 |
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(a) Calculate the average
rate of the reaction between 100 s and 200 s. Show your calculations. (b) Determine the rate constant k for the forward reaction at this temperature using the average rate calculated in part (a). Show your calculations. -
(a) Plot the concentration of HI as a function of time. Based on the shape of the plot, describe the order of the reaction with respect to each reactant (H2 and I2). (b) Using the integrated rate law for the appropriate order of reaction, calculate the half-life of the reaction. Show your calculations.
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(a) Explain why the rate of the reaction decreases over time. (b) If the initial concentration of H2 is doubled while keeping the initial concentration of I2 constant, how will the initial rate of the reaction change? Explain your reasoning.
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