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ladessa [460]
3 years ago
12

Ammonia is formed according to the reaction below. A chemist mixes 21 grams of nitrogen gas and 18 grams of hydrogen gas in a 2.

0 L vessel. How many grams of hydrogen gas will be consumed?
Chemistry
1 answer:
Rama09 [41]3 years ago
5 0

Answer : The mass of hydrogen gas consumed will be, 4.5 grams

Explanation : Given,

Mass of N_2 = 21 g

Mass of H_2 = 18 g

Molar mass of N_2 = 28 g/mole

Molar mass of H_2 = 2 g/mole

First we have to calculate the moles of N_2 and H_2.

\text{Moles of }N_2=\frac{\text{Mass of }N_2}{\text{Molar mass of }N_2}=\frac{21g}{28g/mole}=0.75moles

\text{Moles of }H_2=\frac{\text{Mass of }H_2}{\text{Molar mass of }H_2}=\frac{18g}{2g/mole}=9moles

Now we have to calculate the limiting and excess reagent.

The balanced chemical reaction is,

N_2(g)+3H_2(g)\rightarrow 2NH_3(g)

From the given balanced reaction, we conclude that

As, 1 mole of N_2 react with 3 moles of H_2

So, 0.75 moles of N_2 react with 3\times 0.75=2.25 moles of H_2

From this we conclude that, H_2 is an excess reagent because the given moles are greater than the required moles and N_2 is a limiting reagent because it limits the formation of product.

The moles of hydrogen gas consumed = 2.25 mole

Now we have to calculate the mass of hydrogen gas consumed.

\text{Mass of }H_2=\text{Moles of }H_2\times \text{Molar mass of }H_2

\text{Mass of }H_2=(2.25mole)\times (2g/mole)=4.5g

Therefore, the mass of hydrogen gas consumed will be, 4.5 grams

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