500 mL of nitrogen gas and 750 mL hydrogen gas were allowed to react at 1 bar pressure according to reaction, N _ 2(g) + 3 H _ 2(g) 2 NH _ 3(g) What is PV type of work done during reaction?

Step-by-step solution

The given reaction is N _ 2(g) + 3 H _ 2(g) 2 NH _ 3(g) . Initial volume of N ₂ = 500 mL Initial volume of H ₂ = 750 mL Total initial volume V_i = 500 + 750 = 1250 mL From the stoichiometry, 1 volume of N ₂ reacts with 3 volumes of H ₂ to produce 2 volumes of NH ₃ . Here, H ₂ is the limiting reagent. 750 mL of H ₂ will react with 250 mL of N ₂ to form 500 mL of NH ₃ . Volume of N ₂ remaining = 500 - 250 = 250 mL Total final volume V_f = 250 ( N ₂) + 500 ( NH ₃) = 750 mL Change in volume V = V_f - V_i = 750 - 1250 =