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 pressure of NO2 from 0.2 atm to 0.6 atm

Answer 1

Increasing the pressure of NO₂ from 0.2 atm to 0.6 atm will increase the rate of the reaction, as higher pressure leads to a higher concentration of NO₂, and the rate is directly proportional to this concentration.

Step-by-step explanation:

The rate of the reaction CO(g) + NO₂(g) → CO₂(g) + NO(g) will be affected by changes in the concentrations of the reactants. Since the rate law is given as rate = k [NO₂] [CO], the reaction is first order with respect to both NO₂ and CO, meaning the rate of the reaction depends linearly on the concentrations of both NO₂ and CO.

Specifically, for part (a): Increasing the pressure of NO₂ from 0.2 atm to 0.6 atm will increase the rate of the reaction. This is because when the pressure is increased, assuming ideal gas behavior, the concentration of the gas NO₂ will increase, which, in turn, increases the rate of the reaction proportionally, since the reaction rate is directly proportional to the concentration of NO₂.

Answer 2

Rate will increase by 3 times

Step-by-step explanation:

According to the law of mass action:-

The rate of the reaction is directly proportional to the active concentration of the reactant which each are raised to the experimentally determined coefficients which are known as orders. The rate is determined by the slowest step in the reaction mechanics.

Order of in the mass action law is the coefficient which is raised to the active concentration of the reactants. It is experimentally determined and can be zero, positive negative or fractional.

The order of the whole reaction is the sum of the order of each reactant which is raised to its power in the rate law.

Given that:- Rate law =
`k[NO_2][CO]`

Thus, if the pressure is increased from 0.2 atm to 0.6 atm, means 3 times, rate will also increases 3 times.