How much H₂ (in liters)is produced at 65 °C and 670.torr by the reaction of 75.7 g of zinc? Zn(s)+ 2 H⁺(aq)→ Zn²⁺(aq)+ H₂(g) A)188 L B)2.33 L C)9.22 L D)36.4 L E)95.8 L

Question

Quizplus · Accepted Answer

To find the volume of H₂ produced, first calculate the moles of Zn: 75.7 g Zn / 65.38 g/mol = 1.158 moles Zn. Since the reaction produces 1 mole of H₂ per mole of Zn, 1.158 moles of H₂ are produced. Use the ideal gas law (PV=nRT) to find the volume at 65°C (338 K) and 670 torr (0.881 atm): V = (1.158 mol)(0.0821 L·atm/mol·K)(338 K) / 0.881 atm = 36.4 L.

How Much H2 (In Liters)is Produced at 65 °C and 670.torr

How Much H₂ (In Liters)is Produced at 65 °C and 670.torr