Nitrogen dioxide reacts with carbon monoxide to produce nitrogen monoxide and carbon dioxide. no2(g) + co(g) ⟶ no(g) + co2(g) a proposed mechanism for this reaction is 2no2(g) ⟶ no3(g) + no(g) (fast, equilibrium) no3(g) + co(g) ⟶ no2(g) + co2(g) (slow) what is a rate law that is consistent with the proposed mechanism?

The rate law for the reaction is

Explanation:

Rate law is defined as the expression which expresses the rate of the reaction in terms of molar concentration of the reactants with each term raised to the power their stoichiometric coefficient of that reactant in the balanced chemical equation.

In a mechanism of the reaction, the slow step in the mechanism determines the rate of the reaction.

For the given chemical reaction:

The intermediate reaction of the mechanism follows:

Step 1:  

Step 2:  

As, step 2 is the slow step. It is the rate determining step

Rate law for the reaction follows:

Hence, the rate law for the reaction is written above.

n+h→nh3

we must remember that nitrogen and hydrogen are both diatomic molecules in their standard gas form. this adjusts the equation to

n2+h2→nh3

now we need to adjust coefficients in order to balance the atoms on each side of the equation. currently we have 2 atoms of nitrogen and 2 atoms of hydrogen on the reactant side and 1 atom of nitrogen and 3 atoms of hydrogen on the product side.

we can balance the hydrogens by placing a coefficient of 2 in front of ammonia and a coefficient of 3 in front of the hydrogen.

n2+3h2→2nh3

this gives us 6 hydrogen on each side and coincidentally the nitrogens now equal 2 on each side.

a non redox reaction occurs when there is not a transfer of electrons. for redox reactions, which are reduction-oxidation reactions, a change in the oxidation number occurs. elements that are reduced gain electrons, and elements that are oxidized lose electrons.

explanation: