## Related questions with answers

Consider the first-order decomposition of cyclobutane at $438^{\circ} \mathrm{C}$ at constant volume: $\mathrm{C}_4 \mathrm{H}_8(g) \rightarrow 2 \mathrm{C}_2 \mathrm{H}_4(g)$ a. Express the rate of the reaction in terms of the change in total pressure as a function of time. b. The rate constant for the reaction is $2.48 \times 10^{-4} \mathrm{~s}^{-1}$. What is the half-life? c. After initiation of the reaction, how long will it take for the initial pressure of $\mathrm{C}_4 \mathrm{H}_8$ to drop to $90 \%$ of its initial value?

Solution

VerifiedThis problem is about the first-order decomposition of cyclobutane at $\theta = 438°\text C$ and constant volume. We need to determine the reaction rate in terms of the change in total pressure as a function of time, the half-life when the rate constant is $2.48\cdot 10^{-4}\ \text s^{-1}$, and the time required for the initial pressure to fall to $90$ percent of its initial values.

The **reaction order** describes the **relationship** between the **concentrations of species** and the **reaction rates**.

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