SO₂Cl₂decomposes in the gas phase by the reaction SO₂Cl₂(g) →SO₂(g) + Cl₂(g)
The reaction is first order in SO₂Cl₂and the rate constant is 3.0 × 10^-⁶s^-¹at 600 K. A vessel is charged with 3.3 atm of SO₂Cl₂at 600 K. The partial pressure of SO₂at 3.0 × 10⁵s is _ _ atm.

Question

Quizplus · Accepted Answer

The integrated rate law for a first-order reaction is:ln(P(t)) - ln(P(0)) = -ktwhere P(t) is the partial pressure of SO2Cl2 at time t, P(0) is the initial partial pressure of SO2Cl2, k is the rate constant, and t is time.Substituting the given values into the integrated rate law, we get:ln(P(3.0 × 10^5 s)) - ln(3.3 atm) = -(3.0 × 10^-6 s^-1)(3.0 × 10^5 s)ln(P(3.0 × 10^5 s)) = -0.9P(3.0 × 10^5 s) = e^-0.9 = 0.406 atmThe partial pressure of SO2 at 3.0 × 10^5 s is 0.406 atm.

SO2Cl2 decomposes in the Gas Phase by the Reaction SO2Cl2

SO₂Cl₂decomposes in the Gas Phase by the Reaction SO₂Cl₂