a) How many moles of butane, C4H10(l), must be burned to produce 252 kJ of heat under standard state conditions? (The heat of combustion for butane is −2855.7
b) Calculate ΔH (in kJ/mol) for the reaction described by the equation.
6 NH3(g) + 7 O3(g) → 3 N2O4(g) + 9 H2O(l)
a.) 0.088245... View the full answer
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Given : Heat of combustion of Butane (l) is -2855.7 kJ/mole. I.e. when 1 mole of Butane is burnt there evolves 2855.7 kJ of... View the full answer
a) When 1 mol of butane is burned, 2855.7 kJ of heat is produced Therefore, when 252 kJ of heat is produced, then moles of... View the full answer