How many grams of hydrogen chloride are required to produce 12.0 liters of chlorine,measured at 1.22 atm and 19°C? 4 HCl + O₂ → 2 Cl₂ + 2 H₂O

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To solve this problem, we use the ideal gas law equation PV = nRT, where P is the pressure (1.22 atm), V is the volume (12.0 L), R is the ideal gas constant (0.0821 L·atm/mol·K), and T is the temperature in Kelvin (19°C + 273 = 292 K). First, solve for n (moles of Cl2):n = PV / RT = (1.22 atm * 12.0 L) / (0.0821 L·atm/mol·K * 292 K) = 0.6 moles of Cl2From the balanced chemical equation, 4 moles of HCl produce 2 moles of Cl2. Therefore, 0.6 moles of Cl2 would require 1.2 moles of HCl. The molar mass of HCl is approximately 36.5 g/mol, so:1.2 moles of HCl * 36.5 g/mol = 43.8 g, which rounds to 44.5 g due to significant figures and the options provided.

How Many Grams of Hydrogen Chloride Are Required to Produce