Question

Consider the following reaction:

4 NH₃ + 5O₂   ->   4NO   +   6 H₂O

How many moles of O₂ are needed to react with 4.2 mol NH₃?

How many moles of H₂O can be produced from 1.34 mol O₂?

How many grams of NH₃ will react with 43.4 g O₂?

How many grams of O₂ are needed to produce 56 g NO?

Answer 1

How many moles of O2 are needed to react with 4.2 mol NH3?

From given equation,

Mol of O2 = (5/4)* mol of NH3

= (5/4)*4.2

= 5.25 mol

How many moles of H2O can be produced from 1.34 mol O2?

From given equation,

Mol of H2O = (6/5)* mol of O2

= (6/5)*1.34

= 1.61 mol

How many grams of NH3 will react with 43.4 g O2?

Mol of O2 = mass of O2 / molar mass of O2

= 43.4/32

= 1.356 mol

From given equation,

Mol of NH3 = (4/5)*mol of O2

= (4/5)*1.356

= 1.085 mol

Mass of NH3 = mol of NH3 * molar mass of NH3

= 1.085 mol * 17 g/mol

= 18.4 g

How many grams of O2 are needed to produce 56 g NO?

Mol of NO = mass/molar mass

= 56/30

= 1.87 mol

According to given equation,

Mol of O2 = (5/4)* mol of NO

= (5/4)*1.87

= 2.33 mol

Mass of O2 = number of mol * molar mass

= 2.33 * 32

= 74.7 g