Question

Given the reaction: 4 NH3(g) + 5 O2(g) → 4 NO (g) + 6 H2O When 1.20 mole of ammonia reacts, how many moles of water are produced?

Answer 1

Answer:

When 1.20 mole of ammonia reacts, 1.8 moles of water are produced.

Explanation:

The balanced reaction is:

4 NH₃(g) + 5 O₂(g) → 4 NO (g) + 6 H₂O

By stoichiometry of the reaction, the following amounts of moles participate in the reaction:

• NH₃: 4 moles
• O₂: 5 moles
• NO: 4 moles
• H₂O:  6 moles

Then you can apply the following rule of three: if by stoichiometry 4 moles of ammonia produce 6 moles of water, 1.2 moles of ammonia will produce how many moles of water?

$moles of water=\frac{1.2 moles of ammonia*6 moles of water}{4 moles of ammonia}$

moles of water= 1.8 moles

When 1.20 mole of ammonia reacts, 1.8 moles of water are produced.