Question

Compounds of boron and hydrogen are remarkable for their unusual bonding (described in Section 14.5) and also for their reactivity. With the more reactive halogens, for example, diborane (B₂H₆) forms trihalides even at low temperatures:
B₂H₆(g) + 6Cl₂(g) → 2BCl₃(g) + 6HCl(g) ΔH = -755.4kJ
What is ΔH per kilogram of diborane that reacts?

Answer 1

9.758 × 10⁴ kJ heat is released when 3.573 kg of diborane reacts.

What is Balanced Chemical Equation ?

The balanced chemical equation is the equation in which the number of atoms on the reactant side is equal to the number of atoms on the product side in an equation.

The given reaction balanced equation is:

B₂H₆(g) + 6Cl₂(g) → 2BCl₃(g) + 6HCl(g)

How to find the number of moles ?

To find the number of moles use the expression:

Number of moles = $\frac{\text{Given mass}}{\text{Molar mass}}$

                              = $\frac{3.573\ kg}{27.66\ \text{g/mol}} \times \frac{1000\ g}{1\ kg}$

                              = 129.18 mol

1 mole of B₂H₆, heat released is -755.4 kJ

For 129.18 mol heat released = -755.4 kJ × 129.18

                                                = -97582.57 kJ

                                                = -9.758 × 10⁴ kJ

Thus from the above conclusion we can say that 9.758 × 10⁴ kJ heat is released when 3.573 kg of diborane reacts.

Learn more about the Balanced chemical equation here: brainly.com/question/26694427

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Disclaimer: The given question is incomplete. Here is the complete question.

Question: Compounds of boron and hydrogen are remarkable for their unusual bonding and also for their reactivity. With the more reactive halogens, for example, diborane (B₂H₆) forms trihalides even at low temperatures:

B₂H₆(g) + 6Cl₂(g) → 2BCl₃(g) + 6HCl(g) ΔH = -755.4kJ

How much heat is released when 3.573 kg of diborane reacts? (Give your answer in scientific notation.)