Question

The substances nitrogen monoxide and hydrogen gas react to form nitrogen gas and water. Unbalanced equation: NO (g) + H2 (g) N2 (g) + H2O (l) In one reaction, 76.2 g of H2O is produced. What amount (in mol) of H2 was consumed? What mass (in grams) of N2 is produced?

Answer 1

H2 consumed 4.22 mol

N2 produced 59.107 g

Step-by-step explanation:

Balanced equation:

2NO (g) + 2H2 (g) N2 (g) + 2H2O (l)

• To perform the calculations, the molecular weights of the following compounds must be known:

H2O MW = 18.02 g/mol

N2 MW = 28.01 g/mol

To determine the moles of H2O produced, the following formula should be used:

`MW=(mass)/(mol)`

The value of moles is cleared:

`mol=(mass)/(MW) =(76.2g)/(18.02(g)/(mol) ) =4.22 mol`

• Now, to calculate the grams of N2 consumed, we look at the balanced equation and note that 2 moles of H2 produce 1 mole of N2. Therefore, through said observation, the amount of moles of H2 consumed can be determined.

2 mol H2 ⇒ 1 mol N2

4.22 mol H2 ⇒ X

`X=(4.22mol*1 mol)/(2 mol) =2.11 mol`

To calculate the mass of H2 consumed, the molecular weight equation is used again:

`mass=MW*mol=28.013(g)/(mol)*2.11mol=59.107g`