Question

N2 + 3H2 → 2NH3 How many grams of hydrogen are necessary to react completely with 853.42g of nitrogen in the above reaction?

Answer 1

Answer: 182.87 grams of hydrogen are necessary to react completely with 853.42g of nitrogen.

Step-by-step explanation:

The balanced chemical reaction is :

`N_2+3H_2\rightarrow 2NH_3`

`\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}`

`\text{Number of moles of nitrogen}=(853.42g)/(28g/mol)=30.479moles`

According to stoichiometry:

1 mole of
`N_2` react with = 3 moles of
`H_2`

30.479 moles of
`N_2` will react with=
`(3)/(1)* 30.479=91.437moles` of
`H_2`

Mass of
`H_2` =
`moles* {\text {Molar mass}}=91.437mol* 2g/mol=182.87g`

Thus 182.87 grams of hydrogen are necessary to react completely with 853.42g of nitrogen.