Question

Given the following balanced equation, determine the rate of reaction with respect to

If the rate of O₂ loss is 2.64 x 10³ M/s, what is the rate of formation of SO₃?
2 SO₂(g) + O₂/g) -→ 2 50₃(g)
A) 2.64 x 10³ M/s
B) 1.32 x 10³ M/s
C) 5.28 x 10³ M/s
D) 4.20 x 10³ M/s

Answer 1

To find the instantaneous rate of decomposition of acetaldehyde in a second order reaction, square the concentration and multiply it by the rate constant. The rate will be expressed in molarity per second (M/s).

Step-by-step explanation:

The question asks for the instantaneous rate of decomposition of acetaldehyde, which is a second order reaction. The rate constant provided is 4.71 × 10^-8 L mol^-1 s^-1, and the concentration of acetaldehyde is 5.55 × 10^-4 M. For a second order reaction, the rate can be found using the formula rate = k[A]^2, where k is the rate constant and [A] is the concentration of the reactant. In this case, substituting the provided values into the formula yields the rate:

rate = (4.71 × 10^-8 L mol^-1 s^-1) * (5.55 × 10^-4 M)^2

Thus, to calculate the rate, square the concentration of acetaldehyde and multiply it by the rate constant. The resulting rate will be in units of molarity per second (M/s), as that is the appropriate unit for the rate of a chemical reaction.