The heat evolved with the [tex]\rm B_2H_6[/tex] has been 58.637 kJ.
From the balanced chemical equation, 1 mole of [tex]\rm B_2H_6[/tex] reacts with 2 moles of Chlorine to give 3 moles of boron chloride and 6 moles of HCl,
The chlorine has been required in double the quantity of boron hexahydride.
The moles of Chlorine has been the limiting reactant.
The chlorine that has been responsible for the reaction with [tex]\rm B_2H_6[/tex] will be:
6 Chlorine = 1 [tex]\rm B_2H_6[/tex]
5.65 L Chlorine = [tex]\rm \dfrac{5.65}{6}[/tex]
5.65 L Chlorine = 0.942 L [tex]\rm B_2H_6[/tex].
The moles of [tex]\rm B_2H_6[/tex] can be calculated as:
1 Mole = 22.4 L
Moles of [tex]\rm B_2H_6[/tex] in 0.942 L = 0.042 mol.
The heat evolved for 1 mole [tex]\rm B_2H_6[/tex] has been -1396 kJ.
The heat evolved for 0.042 mol [tex]\rm B_2H_6[/tex] = 0.042 × -1396 kJ.
The heat evolved = 58.637 kJ.
The heat evolved with the [tex]\rm B_2H_6[/tex] has been 58.637 kJ.
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