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# Combustion of glycine enthalpy?

The combustion reaction of glycine is given by the equation:

4 C2H5O2N(s) + 9 O2(g) --> 8 CO2(g) + 10 H2O(l) + 2 N2(g)

where (delta)Hrxn = -3857 kJ/mol.

Given that (delta)H degrees F[CO2(g)] = -393.5 kJ/mol and (delta)H degrees F[H2O(l)] = -285.8 kJ/mol, calculate the enthalpy of formation of glycine.

### 1 Answer

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- Anonymous2 months ago
-3857 kJ/mol = (8 * (-393.5 kJ/mol) + 10 * (-285.8 kJ/mol) + 2 * 0) - (4 * (heat of formation of glycine))

the math will tell you if the sign is + or -

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