Chemistry balancing equations! how many liters of nh3 at stp will react with 5.3g o2 to form no2 and water? 4nh3(g) + 7o2(g) -> 4no2 + 6h2o(g) a. 0.00423l b. 2.12l c.3.03l d. 6.49l

B. 2.12 L  

Step-by-step explanation:

We know we will need a balanced chemical equation with masses and molar masses, so, let's gather all the information in one place.

M_r:                   32.00

        4NH₃(g) + 7O₂(g) ⟶ 4NO₂ + 6H₂O(g)

m/g:                      5.3

(a) Moles of O₂

Moles of O₂ = 5.3 × 1/32.00

Moles of O₂ =0.166 mol

(b) Moles of NH₃

The molar ratio is 4 mol NH₃= 7 mol O₂.

Moles of NH₃ = 0.166 × 4/7

Moles of NH₃ = 0.0946 mol NH₃

(c) Volume of NH₃ at STP

STP is 1 bar and 0 °C. At STP, the molar volume of a gas is 22.71 L.

Volume of NH₃ = 0.0946 ×22.71/1

Volume of NH₃ = 2.15 L

It looks as if you are using the old (pre-1982) definition of STP.

Under that definition, the molar volume of a gas at STP was 22.41 L.

The volume of NH₃ is then 2.12 L.