at a certain temperature the rate of this reaction is first order in clch₂ch₂cl with a rate constant of…

at a certain temperature the rate of this reaction is first order in clch₂ch₂cl with a rate constant of 0.00161 s⁻¹. clch₂ch₂cl(g) → ch₂chcl(g) + hcl(g) suppose a vessel contains clch₂ch₂cl at a concentration of 0.590 m. calculate the concentration of clch₂ch₂cl in the vessel 680. seconds later. you may assume no other reaction is important. round your answer to 2 significant digits.

at a certain temperature the rate of this reaction is first order in clch₂ch₂cl with a rate constant of 0.00161 s⁻¹. clch₂ch₂cl(g) → ch₂chcl(g) + hcl(g) suppose a vessel contains clch₂ch₂cl at a concentration of 0.590 m. calculate the concentration of clch₂ch₂cl in the vessel 680. seconds later. you may assume no other reaction is important. round your answer to 2 significant digits.

Answer

Explanation:

Step1: Recall first - order reaction formula

For a first - order reaction, the integrated rate law is $\ln\left(\frac{[A]_t}{[A]_0}\right)=-kt$, where $[A]_0$ is the initial concentration, $[A]_t$ is the concentration at time $t$, $k$ is the rate constant, and $t$ is the time.

Step2: Rearrange the formula to solve for $[A]_t$

We can rewrite the formula as $[A]_t = [A]_0e^{-kt}$. Given $[A]_0 = 0.590M$, $k=0.00161s^{-1}$, and $t = 680s$.

Step3: Substitute the values into the formula

First, calculate the exponent: $-kt=-0.00161s^{-1}\times680s=- 1.0948$. Then, find $e^{-1.0948}\approx0.335$. Multiply by the initial concentration: $[A]_t=0.590M\times0.335 = 0.19765M$.

Step4: Round to 2 significant digits

Rounding $0.19765M$ to 2 significant digits gives $0.20M$.

Answer:

$0.20M$