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) + 6 Cl2(g) → 2 BCl3(g) + 6 HCl(g) Δ Hrxn = −755.4 kJ How much heat is released when 4.465 kg of diborane reacts? (Give your answer in scientific notation.)

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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) + 6 Cl2(g) → 2 BCl3(g) + 6 HCl(g) Δ Hrxn = −755.4 kJ How much heat is released when 4.465 kg of diborane reacts? (Give your answer in scientific notation.)

Answers

Answer:Amount of energy released = [tex]1.22\times 10^5\ kJ[/tex]Explanation:For [tex]B_2H_6[/tex]  :-Mass of [tex]B_2H_6[/tex]  = 4.465 kg = 4465 g ( 1 kg = 1000 g)Molar mass of [tex]B_2H_6[/tex]  = 27.66 g/molThe formula for the calculation of moles is shown below:[tex]moles = \frac{Mass\ taken}{Molar\ mass}[/tex]Thus,[tex]Moles= \frac{4465\ g}{27.66\ g/mol}[/tex][tex]Moles\ of\ B_2H_6= 161.42\ mol[/tex]From the reaction, [tex]B_2H_6_{(g)} + 6 Cl_2_{(g)}\rightarrow 2 BCl_3_{(g)}+ 6 HCl_{(g)} \Delta\ H_{rxn}=-755.4 kJ[/tex]1 mole of [tex]B_2H_6[/tex] releases 755.4 kJ of energy161.42 moles of [tex]B_2H_6[/tex] releases 755.4*161.42 kJ of energyAmount of energy released = [tex]1.22\times 10^5\ kJ[/tex]

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