Question

How will each of the following affect the rate of the reaction: CO(g) + NO2(g) ⟶ CO2(g) + NO(g) if the rate law for the reaction is rate = k[NO2][CO]?

a) Increasing the concentration of CO.

b) Decreasing the temperature of the reaction.

c) Adding a catalyst to the reaction.

d) Decreasing the pressure of the system.

Answer 1

Increasing the concentration of CO would increase the rate of the reaction, decreasing the temperature would decrease the rate, adding a catalyst would increase the rate, while decreasing the pressure would have no effect.

Step-by-step explanation:

The rate of a reaction can be affected by several factors, as described by the rate law. Let's analyze each scenario:

1. Increasing the concentration of CO: According to the rate law rate = k[NO₂][CO], increasing the concentration of CO would directly affect the rate of the reaction. As CO is one of the reactants, increasing its concentration would result in a higher rate.
2. Decreasing the temperature of the reaction: Temperature is a factor that affects reaction rates. In general, decreasing the temperature reduces the kinetic energy of the particles, resulting in a slower reaction rate.
3. Adding a catalyst to the reaction: A catalyst increases the rate of a reaction by providing an alternative pathway with lower activation energy. Therefore, adding a catalyst would increase the rate of the reaction.
4. Decreasing the pressure of the system: The given reaction does not involve any gases other than CO and NO₂. Therefore, changing the pressure of the system would have no effect on the rate of the reaction.