For the first-order reaction A(g) - 3B(g) + 2C(g) with rate constant k = 1.386 x 10⁻² min⁻¹, 2 mol of A is taken initially in a 12.5 L closed vessel at 298 K and the reaction is allowed to proceed at constant pressure. Find the concentration of B after 100 min.

Question

For the first-order reaction A(g) -> 3B(g) + 2C(g) with rate constant k = 1.386 x 10⁻² min⁻¹, 2 mol of A is taken initially in a 12.5 L closed vessel at 298 K and the reaction is allowed to proceed at constant pressure. Find the concentration of B after 100 min.

Accepted Answer

None of these. kt = 1.386, so fraction remaining = e⁻¹.386 = 0.25; A reacted = 0.75 x 2 = 1.5 mol, giving B = 3 x 1.5 = 4.5 mol. At constant pressure the volume expands as moles rise, so [B] does not equal any of the simple listed constant-volume values, making 'None of these' the answer.

For the first-order reaction A(g) -> 3B(g) + 2C(g) with rate constant k = 1.386 x 10⁻² min⁻¹, 2 mol of A is taken initially in a 12.5 L closed vessel at 298 K and the reaction is allowed to proceed at constant pressure. Find the concentration of B after 100 min.

Solution

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