Glycine, C₂H₅O₂N, is important for biological energy. The combustion reaction of glycine is given by the equation 4C₂H₅O₂N(s) + 9O₂(g) $\rarr$ 8CO₂(g) + 10H₂O(l) + 2N₂(g) $\Delta$ H°_rxn = -3857 kJ/mol
Given that $\Delta$ H°_f[CO₂(g) ] = -393.5 kJ/mol and $\Delta$ H°_f[H₂O(l) ] = -285.8 kJ/mol, calculate the enthalpy of formation of glycine.

Question

Glycine, C₂H₅O₂N, is important for biological energy. The combustion reaction of glycine is given by the equation 4C₂H₅O₂N(s) + 9O₂(g)

\rarr

8CO₂(g) + 10H₂O(l) + 2N₂(g)

\Delta

H°_rxn = -3857 kJ/mol
Given that

\Delta

H°_f[CO₂(g) ] = -393.5 kJ/mol and

\Delta

H°_f[H₂O(l) ] = -285.8 kJ/mol, calculate the enthalpy of formation of glycine.

Quizplus · Accepted Answer

The enthalpy of formation of glycine can be calculated using Hess's law. The equation is: ΔH°rxn = ΣΔH°f(products) - ΣΔH°f(reactants). Plugging in the values: -3857 kJ/mol = [8(-393.5) + 10(-285.8) + 2(0)] - 4(x). Solving for x gives -537.2 kJ/mol.

Glycine, C2H5O2N, Is Important for Biological Energy →\rarr→ 8CO2(g)+ 10H2O(l)+ 2N2(g) Δ\DeltaΔ

Glycine, C₂H₅O₂N, Is Important for Biological Energy $\rarr$ 8CO₂(g)+ 10H₂O(l)+ 2N₂(g) $\Delta$