Question

In a study to determine the rate of the following reaction:

Answer 1

Answer:

The rate of reaction is - 2.868 * 10^-4 M/S

Explanation:

In the following reaction: 2 NO + O2 → 2NO2

NO will be consumed, when adding O2.

This means it will disappear. This is confirmed by the concentration at 5 seconds and 650 seconds.

A = -Δ[A] / ΔT   = [A2] - [A1] / T2 - T1

(0.225 - 0.04) / (650 - 5) = 0.185 / 645 = 2.868 * 10^-4 M/S

Since it will disappear, this number will be negative : - 2.868 * 10^-4 M/S

The rate of reaction is - 2.868 * 10^-4 M/S

Answer 2

Answer:

1.36x10⁻⁵ M/s

Explanation:

The reaction rate can be calculated by the rate of disappearing of a reactant or by the rate of formation of a product, divided by the stoichiometry coefficient. The rate is the velocity, so it's the variation of the concentration divided by the time variation. The rate is always positive, so for the reactants, we must put a minus signal before the equation, so:

r = -(1/2)xΔ[NO]/Δt

r = -(1/2)x$\frac{0.0225 - 0.0400}{650 - 5}$

r = 1.36x10⁻⁵ M/s