Question

2 N2O(g) --> 2 N2(g) O2(g) The decomposition of N2O(g) to N2(g) and O2(g) is represented by the equation above. The t1/2 for this reaction is 3.58 x 103 minutes at 730 C. What is the value of the rate constant, k, for the decomposition of N2O(g)

Answer 1

The value of the rate constant, k, for the decomposition of N2O(g) is 1.935 x 10⁻⁴ min⁻¹.

Step-by-step explanation:

The rate constant, k, for the decomposition of N2O(g) can be calculated using the half-life (t₁/₂) of the reaction. The half-life equation for a first-order reaction is given by:

t₁/₂ = 0.693 / k

Plugging in the given t₁/₂ value of 3.58 x 10³ minutes, we can solve for k:

3.58 x 10³ minutes = 0.693 / k

k = 0.693 / (3.58 x 10³ minutes) = 1.935 x 10⁻⁴ min⁻¹