How many liters of O₂ gas at 25°C and 1.00 atm pressure are needed to react with 60.25 grams of potassium hydride according to the chemical equation shown below?
2 KH(s) + O₂(g) → H₂O(l) + K₂O(s)

Question

Quizplus · Accepted Answer

1. Convert 60.25 grams of KH to moles: 60.25 g KH (1 mol KH/39.10 g KH) = 1.54 mol KH 2. According to the balanced chemical equation, 2 moles of KH react with 1 mole of O₂: 2 mol KH : 1 mol O₂ 3. Therefore, we need 0.77 moles of O₂ to react with 1.54 moles of KH: 0.77 mol O₂ = (PV)/(RT) PV = (0.77 mol)(0.0821 L atm/mol K)(298 K) P = 1 atm V = (0.77 mol)(0.0821 L atm/mol K)(298 K) / (1 atm) V = 18.4 L (rounded to one decimal place) So, we need 18.4 liters of O₂ gas to react with 60.25 grams of KH. Therefore, the best choice is B.

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