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Calculate the carbon carbon double bond energy in ethane from the following reaction, H2C=CH2(g) + H2(g) –> H3C−CH3(g) ΔH = −138 kJ/mol. If Bond enthalpies are: C−C = 348; H−H = 436; C−H = 412 in KJ/mol.

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MCQs on thermodynamics terms and applications, calorimetry measurement, enthalpy change, enthalpies for reactions types, spontaneity, gibbs energy change and equilibrium.


Calculate the carbon carbon double bond energy in ethane from the following reaction, H<sub>2</sub>C=CH<sub>2</sub>(g) + H<sub>2</sub>(g) –> H<sub>3</sub>C−CH<sub>3</sub>(g) ΔH = −138 kJ/mol. If Bond enthalpies are: C−C = 348; H−H = 436; C−H = 412 in KJ/mol.






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