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The bond enthalpy of N2(g) is 418.0 kJ/mol. Calculate delta H°f for N(g).?
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given that:
delta H [Cl(g)]=121.3 kJ*mol^(-1) delta H [C(g)]= 716.7 kJ*mol^(-1) delta H [CCl(subscript 4)(g)] =-95.7kJ*mol^(-1)
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The average bond enthalpy for C__H is 413 kJ/mol. In other words, 413 kJ of energy is required to break a mole of CH into atoms:
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Bond enthalpy is the energy required to break a mole of a certain type of bond.
O=O = 495 kj/mol S-F = 327 kj/mol S=O = 523
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Bond enthalpy is the energy required to break a mole of a certain type of bond.
O=O = 495 kj/mol S-F = 327 kj/mol S=O = 523
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