The rate law for the rearrangement of CH₃NC to CH₃CN at 800 K is rate = (1300 s^-1)[CH₃NC].What is the half-life for this reaction?

Question

Quizplus · Accepted Answer

The half-life (t½) can be calculated using the following formula: t½ = ln(2) / k where k is the rate constant. In this case, the rate law is given as: rate = k[CH₃NC] Comparing with the standard rate law, we can see that: k = 1300 s^-1 Substituting this value of k into the formula for t½, we get: t½ = ln(2) / (1300 s^-1)([CH₃NC]) We don't have a specific value for [CH₃NC], but we can assume an initial concentration of 1 M (for simplicity). Therefore, t½ = ln(2) / (1300 s^-1)(1 M) t½ = 5.3 * 10-10 s = 5.3 × 10-4 s = 5.3 × 10-10 × 106 s = 5.3 × 10-10 × 1,000,000 μs = 0.53 μs Converting to seconds (as per the options) gives us: t½ = 5.3 × 10-10 s = 5.3 × 10-10 × 10^10 s = 5.3 × 10-4 × 10^6 s = 0.53 × 10^6 s = 530000 s Therefore, the best choice is B, with a half-life of 5.3 × 10-10 s or 530000 s.

The Rate Law for the Rearrangement of CH3NC to CH3CN ×\times×

The Rate Law for the Rearrangement of CH₃NC to CH₃CN $\times$