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Question

The substances nitrogen monoxide and hydrogen gas react to form nitrogen gas and water.

1. Unbalanced equation:  NO (g) + H₂ (g) N₂ (g) + H₂O (l)

In one reaction, 54.2 g of H₂O is produced. What amount (in mol) of H₂ was consumed? What mass (in grams) of N₂ is produced?

___ mol H₂ consumed

___ g N₂ produced

Answer 1

2NO (g) + 2H₂ (g) N₂ (g) + 2H₂O (l)

to balance the equation

balance N by adding 2 in front of NO

balance O by adding 2 in front of H₂O

balance H by adding 2 in front of H₂

Calculation

What amount (in mol) of H₂ was consumed?

You have a mass of H₂O, change the mass to moles using molar mass then use the mole ratio from the balanced equation. Use dimensional analysis.

54.2 g H₂O x (1 mol H₂O/18.02 g H₂O) x (2 mol H₂/2 mol H₂O) = 3.01 mol H₂ consumed

↑ ↑

change mass to mol mol ratio

What amount (in mol) of N₂ was consumed?

You have a mass of H₂O, change the mass to moles using molar mass, use the mole ratio from the balanced equation and then change moles to mass. Use dimensional analysis.

54.2 g H₂O x (1 mol H₂O/18.02 g H₂O) x (1 mol N₂/2 mol H₂O) x (28.02 g N₂/1 mol N₂) =

↑ ↑ ↑

change mass to mol mol ratio change mol to mass

42.0 g N₂ is produced