SO₂Cl₂ decomposes in the gas phase by the reaction
SO₂Cl₂(g) → SO₂(g) + Cl₂(g)
The reaction is first order in SO₂Cl₂ and the rate constant is 3.0 × 10^-6s^-1at 600 K.A vessel is charged with 2.4 atm of SO₂Cl₂at 600 K.The partial pressure of SO₂Cl₂at 3.0 × 10⁵s is ________ atm.

Question

Quizplus · Accepted Answer

We can use the following formula to solve this problem: ln(P1/P2) = -kt where P1 and P2 are the initial and final partial pressures of SO₂Cl₂, respectively. We can rearrange the formula to solve for P2: P2 = P1*e^(-kt) Substituting the given values: P1 = 2.4 atm k = 3.0 × 10^-6 s^-1 t = 5 s (since the reaction occurs over 5 seconds when the partial pressure of SO₂Cl₂ drops from 2.4 atm to the unknown value) P2 = 2.4 atm * e^(-3.0 × 10^-6 s^-1 * 5 s) = 0.98 atm Therefore, the partial pressure of SO₂Cl₂ at 3.0 × 10^15 s is 0.98 atm, which corresponds to choice (C).

SO2Cl2 Decomposes in the Gas Phase by the Reaction

SO₂Cl₂ Decomposes in the Gas Phase by the Reaction