According to the following reaction, how much energy is evolved during the reaction of 32.5 g B2H6 with excess Cl2? The molar mass of B2H6 is 27.67 g/mol. B2H6(g) + 6 Cl2(g) → 2 BCl3(g) + 6 HCl(g) ΔH°rxn = -1396 kJ

1640.3 kJ of energy is released

Explanation:

Step 1: data given

Mass of B2H6 = 32.5 grams

Cl2 = in excess

The molar mass of B2H6 is 27.67 g/mol.

ΔH°rxn = -1396 kJ

Step 2: The balanced equation

B2H6(g) + 6 Cl2(g) → 2 BCl3(g) + 6 HCl(g)   -1396 kJ

This means when 1 mol of B2H6 reacts with 6 moles of Cl2 there will 1396 kJ of energy be released

Step 3: Calculate the moles of B2H6

Moles B2H6 = mass B2H6 / molar mass B2H6

Moles B2H6 = 32.5 grams / 27.67 g/mol

Moles B2H6 = 1.175 moles

Step 4: Define the limiting reactant

Since Cl2 is in excess, B2H6 will be the limiting reactant.

For 1 mol B2H6 we need 6 moles Cl2 to produce  2 moles BCl3 an 6 moles HCl

For this reaction 1396 kJ of energy will be given off

For 1.175 moles B2H6 the amount of energy released will be:

1.175 * 1396 = 1640.3 kJ

1640.3 kJ of energy is released

NOTE: the negative sign in the question show the energy is released

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the right answer is c i just did the question.