# The reaction between ammonia and nitrous oxide is given below: 2 NH3(g) + 3 N2O(g) ? 4 N2(g) + 3...

## Question:

The reaction between ammonia and nitrous oxide is given below:

2 NH3(g) + 3 N2O(g) ? 4 N2(g) + 3 H2O(g)

We therefore know that which of the following reactions can also occur?

a. 4 NH3(g) + 6 N2O(g) ? 5 N2(g) + 6 H2O(g)

b. CO_2 (g) + H_2 (g) ? CO (g) + H_2O (l)

c. 5 N_2 (g) + 6 H_2O (g) ? 4 NH_3 (g) + 6 NO (g)

d. None of the above

## The Balanced Equations

The balanced equation represents the mole ratio of the reactants needed to react and the mole ratio of the product to be produced. If the reaction is not balanced yet, there is no information about the relationship of the amount of molecule between reactants and products.

{eq}2 NH3(g) + 3 N2O(g) \rightarrow 4 N2(g) + 3 H2O(g) {/eq}

That means, when two molecules of {eq}NH_{3} {/eq} reacts, we will produce four molecules of {eq}N_{2} {/eq}. Then, the mole ratio between {eq}NH_{3} {/eq} and {eq}N_{2} {/eq} is 1:2.

In option A. {eq}4 NH3(g) + 6 N2O(g) \rightarrow 5 N2(g) + 6 H2O(g) {/eq}

The mole ratio between {eq}NH_{3} {/eq} and {eq}N_{2} {/eq} is 4:5. Since we know the mole ratio is 1:2. Then, the reaction in option c is not a proportional mole. Therefore, the atoms of N is not balance in the reaction and the products should be 8 molecules of {eq}N_{2} {/eq}, not 5 molecules of {eq}N_{2} {/eq}. That means the reaction can not occur to produce 5 molecules of {eq}N_{2} {/eq}

In option B. {eq}CO_2 (g) + H_2 (g) \rightarrow CO (g) + H_2O (l) {/eq}.

Since that is already balance reaction. That means the reaction can occur.

In option C. {eq}5 N_2 (g) + 6 H_2O (g) \rightarrow 4 NH_3 (g) + 6 NO (g) {/eq}

Since we know the mole ratio between {eq}N_{2} {/eq} and {eq}NH_{3} {/eq} is 2:1. Then, if 5 molecules of {eq}N_{2} {/eq} reacts, we will get 2.5 molecules of {eq}NH_{3} {/eq}. But in the option, the molecules of {eq}NH_{3} {/eq} is 4. Then, the reaction in option c is not balance and the reaction will not occur.

Therefore, the following reactions can also occur is b. {eq}CO_2 (g) + H_2 (g) \rightarrow CO (g) + H_2O (l) {/eq} 