According to the following reaction,how much energy is evolved during the reaction of 2.50 L B₂H₆ and 5.65 L Cl₂?(Both gases are initially at STP.)The molar mass of B₂H₆is 27.67 g/mol. B₂H₆(g)+ 6 Cl₂(g)→ 2 BCl₃(g)+ 6 HCl(g)ΔH°_rxn= -1396 kJ A) 58.7 kJ B) 156 kJ C) 215 kJ D) 352 kJ E) 508 kJ

Question

Quizplus · Accepted Answer

At STP, 1 mole of gas occupies 22.4 L. Therefore, 2.50 L of B2H6 is 0.1116 moles and 5.65 L of Cl2 is 0.2522 moles. The reaction requires 6 moles of Cl2 per mole of B2H6, so Cl2 is the limiting reactant. The reaction of 0.2522 moles of Cl2 releases (0.2522/6) * 1396 kJ = 58.7 kJ.

According to the Following Reaction,how Much Energy Is Evolved During