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 $\mathrm { mol } ^ { - 1 }$ . B₂H₆(g) + 6Cl₂(g) ? 2BCl₃(g) + 6HCl(g)
D_rH°= -1396 kJ

Question

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

\mathrm { mol } ^ { - 1 }

. B₂H₆(g) + 6Cl₂(g) ? 2BCl₃(g) + 6HCl(g)
D_rH°= -1396 kJ

Quizplus · Accepted Answer

At STP, 1 mole of any gas occupies 22.4 L. Therefore, 2.50 L of B2H6 is 2.50/22.4 = 0.1116 moles, and 5.65 L of Cl2 is 5.65/22.4 = 0.2522 moles. The reaction requires 6 moles of Cl2 per mole of B2H6, so Cl2 is in excess. The limiting reagent is B2H6. The reaction of 0.1116 moles of B2H6 releases 0.1116 * 1396 kJ = 155.8 kJ, which rounds to 156 kJ.

According to the Following Reaction,how Much Energy Is Evolved During mol−1\mathrm { mol } ^ { - 1 }mol−1

According to the Following Reaction,how Much Energy Is Evolved During $\mathrm { mol } ^ { - 1 }$