Given the following enthalpies of reaction: C + O2 ---> CO2 ΔH = -393.5 kJ H2 + 1/2 O2 ---> H2O ΔH = -285.8 kJ 2C2H6 + 7O2 ---> 4CO2 + 6H2O ΔH = -3119.6 kJ Use the law of Hess to calculat the enthalpy change for the reaction: 2C + 3H2 ---> C2H6 ΔH = ? A. +1559.8 kJ B. -84.6 kJ C. +787 kJ D. -156.3 kJ

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Given the following enthalpies of reaction:
C + O2 ---> CO2 ΔH = -393.5 kJ
H2 + 1/2 O2 ---> H2O ΔH = -285.8 kJ
2C2H6 + 7O2 ---> 4CO2 + 6H2O ΔH = -3119.6 kJ
Use the law of Hess to calculat the enthalpy change for the reaction: 2C +
3H2 ---> C2H6 ΔH = ?
A. +1559.8 kJ
B. -84.6 kJ
C. +787 kJ
D. -156.3 kJ

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This question is answered by using the simple concept of Hess law of constant heat change whether a reaction takes place in single step of a number of steps.

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