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a) How many moles of butane , C 4 H 10 ( l ) , must be burned to produce 252 kJ of heat under standard state conditions?

a) How many moles of butaneC4H10(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)


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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

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