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The combustion of B2H6 occurs according to the following equation. Using the enthalpies of formation, calculate the energy (kJ) released when 4.00 g of B2H6 reacts.
(Atomic weights: B = 10.81, O = 16.00, H = 1.008).
B2H6(g) + 3 O2(g) B2O3(s) + 3 H2O(g)
Ho B2H6(g) = -57.4 kJ/mole
Ho B2O3(s) = -1273 kJ/mole
Ho H2O(g) = -241.8 kJ/mol
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