For the reaction 2C → A + B, 0.02 mol of A is formed during the first 15 seconds of the reaction. Assuming that the rate of reaction remains constant for 2 min, which of the following statements is true?

Question

Quizplus · Accepted Answer

First, we can use the given information to calculate the rate of the reaction using the formula:

rate = (change in concentration of A) / time

rate = (0.02 mol) / (15 s) = 0.00133 mol/s

Since we are assuming the rate remains constant for 2 min (120 s), we can use this rate to determine the amount of B and C produced or consumed during that time.

For every 2 mol of C that react, 1 mol of A and 1 mol of B are produced. Therefore, for every 1 mol of A produced, 1 mol of C is consumed.

Amount of C consumed = rate x time = (0.00133 mol/s) x (120 s) = 0.16 mol

Amount of B produced = 0.5 x amount of A produced = 0.5 x 0.02 mol = 0.01 mol

Therefore, the total amount of C consumed after 2 min is 0.16 mol and the total amount of B produced after 2 min is 0.01 mol.

Therefore, the correct statement is C) After 2 min, 0.16 mol of B was produced and 0.32 mol of C was consumed.

For the Reaction 2C → a + B, 0