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

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. B2H6 is the limiting reactant. The reaction releases 1396 kJ per mole of B2H6. Thus, 0.1116 moles of B2H6 will release 0.1116 * 1396 kJ = 155.7 kJ, which rounds to 156 kJ.

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