Consider the following balanced reaction. How many grams of water are required to form 75.9 g of HNO₃? Assume that there is excess NO₂ present. The molar masses are as follows:
H₂O = 18.02 g mol^-1, HNO₃ = 63.02 g mol^-1. 3NO₂(g) + H₂O(l) → 2HNO₃(aq) + NO(g)

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Quizplus · Accepted Answer

To find the grams of water required, first calculate the moles of HNO3 formed: 75.9 g / 63.02 g/mol = 1.204 moles. According to the balanced equation, 1 mole of H2O produces 2 moles of HNO3. Therefore, 1.204 moles of HNO3 require 0.602 moles of H2O. Convert moles of H2O to grams: 0.602 moles * 18.02 g/mol = 10.9 g.

Consider the Following Balanced Reaction