Question

The rate constant for the first-order decomposition of a compound Ain the reaction A → P is kr= 3.56 × 10−7s−1at 25 °C. (a) What is the half-life ofA? (4points)(b) If the initial pressure is33.0 kPa. What will be the pressure of the reactionafterone days

Answer 1

The half-life of the decomposition of O3 can be calculated using the rate constant and the concentration of O3. The half-life is approximately 8.47 x 10^4 hours.

Step-by-step explanation:

The half-life of a reaction can be determined using the rate constant and the order of the reaction. In this case, the decomposition of O3 is a second-order reaction with a rate constant of 50.4 L mol-¹ h¯¹. To find the half-life, we can use the equation:

t1/2 = 1/(k * [A])

where t1/2 is the half-life, k is the rate constant, and [A] is the concentration of A. Plugging in the values, we get:

t1/2 = 1/(50.4 L mol^-1 h^-1 * 2.35 x 10^-6 M)

t1/2 = 8.47 x 10^4 hours