The rate constant for the reaction 2 ClO(g)$\to$ Cl₂(g)+ O₂(g)is 7.22 $\times$ 10⁹ M^-1s^-1 at a particular temperature.Suppose 0.0250 atm ClO is initially present in reaction vessel containing air at STP (1 atm,273 K).What is the half-life of this reaction?

Question

Quizplus · Accepted Answer

To find the half-life of the reaction, we need to use the first-order integrated rate law equation:

ln([ClO]t/[ClO]0) = -kt

where [ClO]t is the concentration at time t, [ClO]0 is the initial concentration, k is the rate constant, and t is time. To find the half-life, we can set [ClO]t = 0.5[ClO]0 and solve for t:

ln(0.5) = -kt1/2

where t1/2 is the half-life. Rearranging, we get:

t1/2 = ln(2)/k

Plugging in the given values, we get:

t1/2 = ln(2)/(7.22 x 10^10 s^-1) = 1.24 x 10^-10 s

Therefore, the correct answer is B, 1.24 x 10^-10 s.

The Rate Constant for the Reaction 2 ClO(g) →\to→ Cl2(g)+ O2(g)is 7

The Rate Constant for the Reaction 2 ClO(g) $\to$ Cl₂(g)+ O₂(g)is 7