Question

Consider the following two-step process (unbalanced). How many moles of water can be formed from 0.46 moles of N2?

Answer 1

The question is incomplete, here is the complete question:

Consider the following two-step process (unbalanced). How many moles of water can be formed from 0.680 moles of $N_2$ ?

$N_2+H_2\rightarrow NH3$

$NH_3+O_2\rightarrow NO+H_2O$

Enter your answer numerically to three siginificant figures.

Answer: The amount of water formed from given amount of nitrogen gas is 1.38 moles

Explanation:

We are given:

Moles of nitrogen gas = 0.46 moles

The balanced chemical equation follows:

$N_2+3H_2\rightarrow 2NH3$       .......(1)

$4NH_3+5O_2\rightarrow 4NO+6H_2O$     .......(2)

From equation 1:

By Stoichiometry of the reaction:

1 mole of nitrogen gas produces 2 moles of ammonia

So, 0.46 moles of nitrogen gas will produce = $\frac{2}{1}\times 0.46=0.92mol$ of ammonia

From equation 2:

By Stoichiometry of the reaction:

4 moles of ammonia produces 6 moles of water

So, 0.92 moles of ammonia will produce = $\frac{6}{4}\times 0.92=1.38mol$ of water

Hence, the amount of water formed from given amount of nitrogen gas is 1.38 moles