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

Rate will increase by 3 times

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 =

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

the positions which points up in upward carbon and down in downward carbon are axial

and vice versa holds true for equatorial positions

so the correct answer with labelled diagram will be

gas

explanation:

smoke is the matter of a gas