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4.8g of C (diamond) on complete combustion evolves 1584kJ of heat. The standard heat of formation of gaseous carbon is 725 kJ/mol. The energy required for the process a. C(graphite) - - > C(gas) b. C(diamond) - - >C(gas) are 1)725,727 2)727,725 3)725,723
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4.8g of C (diamond) on complete combustion evolves 1584kJ of heat. The...
Energy Changes in Phase Transformations

Heat of Formation
The standard heat of formation of a compound is the change in enthalpy when one mole of the compound is formed from its elements in their standard states. This value is typically given in kJ/mol.

Given Data
- Heat of formation of gaseous carbon (C) = 725 kJ/mol
- Heat evolved on complete combustion of 4.8g of C (diamond) = 1584 kJ

Calculations
- Moles of C (diamond) = 4.8g / 12g/mol = 0.4 mol
- Heat evolved on combustion of 0.4 mol of C (diamond) = 1584 kJ
- Heat evolved on combustion of 1 mol of C (diamond) = 1584 kJ / 0.4 mol = 3960 kJ/mol

Energy Required for the Process
a. C(graphite) - - > C(gas)
- Heat of formation of C(g) = Heat of formation of C(g) - Heat of formation of C(s) = 725 kJ/mol - 0 = 725 kJ/mol
b. C(diamond) - - > C(gas)
- Heat of formation of C(g) = Heat of formation of C(g) - Heat evolved on combustion of C(diamond) = 725 kJ/mol - 3960 kJ/mol = -3235 kJ/mol
Therefore, the correct energy values for the processes are:
a. 725 kJ/mol
b. -3235 kJ/mol
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4.8g of C (diamond) on complete combustion evolves 1584kJ of heat. The standard heat of formation of gaseous carbon is 725 kJ/mol. The energy required for the process a. C(graphite) - - > C(gas) b. C(diamond) - - >C(gas) are 1)725,727 2)727,725 3)725,723 Related: Enthalpy Changes During Phase Transformations?
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