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Consider the reaction 4HNO3(l) + 3KCl(s) → Cl2(g) + NOCl(g) + 2H2O(g) + 3KNO3(s) The amount of HNO3 required to produce 110.0 g of KNO3 is : (Given : Atomic masses of H, O, N and K are 1, 16, 14 and 39, respectively.)

1. 32.2 g
2. 69.4 g
3. 91.5 g
4. 162.5 g

Correct answer: 91.5 g

Solution

To find the amount of HNO3 needed, we first determine the moles of KNO3 produced from 110.0 g, which is approximately 0.79 moles. According to the balanced equation, 4 moles of HNO3 are required for every 3 moles of KNO3, leading to the calculation of about 0.79 moles of KNO3 needing 1.05 moles of HNO3. Converting this to grams using the molar mass of HNO3 (63 g/mol) gives approximately 91.5 g.

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