Problem: Glycine, C2H5O2N. is important for biological energy. The combustion reaction of glycine is given by the equation: 4C2H5O2N(s) + 9O2(g) → 8CO2(g) + 10H2O(l) + 2N2(g) ΔH°rxn = -3857 kJ. Given that ΔH°f[CO2(g)] = -393.5 kJ/mol and ΔH°f[H2O(I)] = -285.8 kJ/mol, calculate the enthalpy of formation of glycine. a) -537.2 kJ/mol b) -268.2 kJ/mol c) -2,149 kJ/mol d) 3,178 e) -964 kJ/mol

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Glycine, C2H5O2N. is important for biological energy. The combustion reaction of glycine is given by the equation:

4C2H5O2N(s) + 9O2(g) → 8CO2(g) + 10H2O(l) + 2N2(g) ΔH°rxn = -3857 kJ.

Given that ΔH°f[CO2(g)] = -393.5 kJ/mol and ΔH°f[H2O(I)] = -285.8 kJ/mol, calculate the enthalpy of formation of glycine.

a) -537.2 kJ/mol

b) -268.2 kJ/mol

c) -2,149 kJ/mol

d) 3,178

e) -964 kJ/mol

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