Question

Balance the equation below and determine the mass in grams of N_2 needed to produce 11.35 g of NH_3.

Answer 1

• The balanced chemical reaction:

$3H_2+2N_2\rightarrow 2NH_3$

• The mass of $N_2$ needed is 18.67 grams.

Given:

The unbalanced chemical equation:

$H_2+N_2\rightarrow NH_3$

To find:

The balanced chemical equation and to determine of $N_2$ needed to produce 11.35 g of $NH_3$.

Solution:

The balanced chemical reaction:

$3H_2+2N_2\rightarrow 2NH_3$

Mass of ammonia needed to produce = 11.35 g

Moles of ammonia :

= $\frac{11.35 g}{17.031 g/mol}=0.6664 mol$

    $3H_2+2N_2\rightarrow 2NH_3$

According to the reaction, 2 moles of ammonia is obtained from 2 moles of dinitrogen, then 0.6664 moles of ammonia will be obtained from :

$=\frac{1}{1}\times 0.6664 mol=0.6664 \text{mol of } N_2$

Moles of dinitrogen required = 0.6664 mol

Mass of 0.6664 moles of dinitrogen:

$=0.6664 mol\times 28.0134 g/mol=18.67 g$

The mass of $N_2$ needed is 18.67 grams.

Learn more about the unitary method here:

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