According to the following reaction, how much energy is evolved during the reaction of 32.5 g B₂H₆ and 72.5 g Cl₂? The molar mass of B₂H₆is 27.67 g mol^-1. B₂H₆(g)+ 6Cl₂(g)→ 2BCl₃(g)+ 6HCl(g)Δ_rH°= -1396 kJ

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Quizplus · Accepted Answer

First, calculate the moles of B2H6: 32.5 g / 27.67 g/mol = 1.175 moles. For Cl2: 72.5 g / 70.90 g/mol = 1.022 moles. The reaction requires 6 moles of Cl2 per mole of B2H6, so Cl2 is the limiting reactant. The reaction produces 1.022/6 = 0.170 moles of B2H6 reacting. Energy evolved = 0.170 moles * 1396 kJ/mol = 238 kJ.

According to the Following Reaction, How Much Energy Is Evolved