Nitric acid decomposes in light to form nitrogen dioxide, water, and oxygen, according to the following chemical equation. 4HNO3 (l â 4NO2(g) + 2H2O (l) + O2(g)

If 2.5 g nitric acid decomposes, what is the total volume of gas produced?

a. 0.050L
b. 0.22
c.0.89
d. 1.1L

b. 0.22 L

Explanation:

Step 1: Write the balanced equation

4 HNO₃(l) ⇒ 4 NO₂(g) + 2 H₂O(l) + O₂(g)

Step 2: Calculate the moles corresponding to 2.5 g of HNO₃

The molar mass of HNO₃ is 63.01 g/mol.

2.5 g × 1 mol/63.01 g = 0.040 mol

Step 3: Calculate the moles of O₂ produced from 0.040 moles of HNO₃

The molar ratio of HNO₃ to O₂ is 4:1. The moles of O₂ produced are 1/4 × 0.040 mol = 0.010 mol.

Step 4: Calculate the volume corresponding to 0.010 moles of O₂

Assuming the reaction takes place at standard temperature and pressure, the volume of 1 mole of O₂ is 22.4 L.

0.010 mol × 22.4L/1 mol = 0.22 L

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