Question

Nitrogen and hydrogen react together to form ammonia according to the equation:___N2(g) + ___H2(g) → ___NH3(g) (unbalanced)Balance the equation, and determine how many grams of hydrogen would be required to form 50.0 g of ammonia, assuming there is sufficient nitrogen available.4.46 g5.94 g4.81 g8.91 gnot enough information

Answer 1

`m_(H)=8.89 g`

Step-by-step explanation:

To balance the equation:

1) Asume 1 mol of N2 :

`N_2 (g) + __ H_2 (g) \longrightarrow __ NH_3 (g)`

2) Balance the nitrogen:

`N_2 (g) + __ H_2 (g) \longrightarrow 2 NH_3 (g)`

3) Balance the hydrogen:

`N_2 (g) + 3 H_2 (g) \longrightarrow 2 NH_3 (g)`

To calculate the hydrogen:

`M_(am)= molecular weight of ammonia`

`M_(am)= 14+3*1=17 g/mol`

`n_(am)= mol of ammonia`

`n_(am)= (50g)/(17 g/mol)=2.94 mol`

Due to the equation you need 3 mol of hydrogen per 2 mol of ammonia:

`n_(H)= 2.94 mol (3)/(2)=4.41 mol`

`m_(H)=2.016 (g)/(mol)*4.41 mol=8.89 g`