How much H₂ (in liters)is produced at 45 °C and 770.torr by the reaction of 45.7 g of zinc? Zn(s)+ 2 H⁺(aq)→ Zn²⁺(aq)+ H₂(g) A)139 L B)15.7 L C)18.0 L D)31.4 L E)11.8 L

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First, calculate moles of Zn: 45.7 g Zn / 65.38 g/mol = 0.699 moles Zn. The reaction produces 0.699 moles of H₂. Use the ideal gas law: PV = nRT. Convert 770 torr to atm: 770/760 = 1.013 atm. Convert 45°C to Kelvin: 45 + 273 = 318 K. R = 0.0821 L·atm/mol·K. V = nRT/P = (0.699 mol)(0.0821 L·atm/mol·K)(318 K) / 1.013 atm = 18.0 L.

How Much H2 (In Liters)is Produced at 45 °C and 770.torr

How Much H₂ (In Liters)is Produced at 45 °C and 770.torr