How many grams of NO can be produced from the following reaction if 68.2 grams of NO2 is consumed?
3NO2(g) + H2O(l) → 2HNO3(aq) + NO(g) 1. 133 g
2. 314 g 3. 0.148 g 4. 14.8 g

Option 4. 14.8 g

Explanation:

3NO2 + H2O → 2HNO3 + NO

First let us calculate the molar mass of NO2 and NO. This is illustrated below;

Molar Mass of NO2 = 14 + (2x16) = 14 + 32 = 46g/mol

Mass of NO2 from the question = 3 x 46 = 138g.

Molar Mass of NO = 14 +16 = 30g/mol

From the equation,

138g of NO2 reacted to produce 30g of NO

Therefore, 68.2g of NO2 will react to produce = (68.2 x 30)/138 = 14.8g of NO.

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