Given the following reactions and their ΔG^∘ values, COCl2(g)+4 NH3(g) ⟶ CO(NH2)2(s)+2 NH4 Cl(s)

step 1 To determine the standard delta G for the following reaction, given three reactions, we need to

Given the following reactions and their ΔG^∘ values,...

Given the following reactions and their $\Delta G^{\circ}$ values, $\mathrm{COCl}_{2}(g)+4 \mathrm{NH}_{3}(g) \longrightarrow$ $$ \begin{aligned} \mathrm{CO}\left(\mathrm{NH}_{2}\right)_{2}(s)+2 \mathrm{NH}_{4} \mathrm{Cl}(s) & \Delta G^{\circ}=-332.0 \mathrm{~kJ} \\ \mathrm{COCl}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow \mathrm{CO}_{2}(g)+2 \mathrm{HCl}(g) \\ \Delta G^{\circ}=-141.8 \mathrm{~kJ} \end{aligned} $$ calculate the value of $\Delta G^{\circ}$ for the reaction $$ \mathrm{CO}\left(\mathrm{NH}_{2}\right)_{2}(s)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow \mathrm{CO}_{2}(g)+2 \mathrm{NH}_{3}(g) $$

Given the following reactions and their $\Delta G^{\circ}$ values, $\mathrm{COCl}_{2}(g)+4 \mathrm{NH}_{3}(g) \longrightarrow$
$$
\begin{aligned}
\mathrm{CO}\left(\mathrm{NH}_{2}\right)_{2}(s)+2 \mathrm{NH}_{4} \mathrm{Cl}(s) & \Delta G^{\circ}=-332.0 \mathrm{~kJ} \\
\mathrm{COCl}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow \mathrm{CO}_{2}(g)+2 \mathrm{HCl}(g) \\
\Delta G^{\circ}=-141.8 \mathrm{~kJ}
\end{aligned}
$$
calculate the value of $\Delta G^{\circ}$ for the reaction
$$
\mathrm{CO}\left(\mathrm{NH}_{2}\right)_{2}(s)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow \mathrm{CO}_{2}(g)+2 \mathrm{NH}_{3}(g)
$$

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Key Concepts

Hess's Law

Hess’s law states that the total Gibbs free energy change for a reaction is independent of the pathway taken; it depends only on the initial and final states. This principle allows one to combine or break down chemical reactions and use their individual ?G° values to determine the ?G° of an overall reaction by adding or subtracting the free energy changes of the component reactions.

Standard Gibbs Free Energy Change (?G°)

The standard Gibbs free energy change, ?G°, indicates the spontaneity of a reaction under standard conditions. A negative ?G° means that the reaction proceeds spontaneously, while a positive ?G° indicates non?spontaneity. This concept is fundamental in predicting whether a reaction, as written, is thermodynamically favorable.

Reaction Manipulation (Reversal and Combination)

To apply Hess’s law effectively, chemical reactions may need to be reversed, scaled, or added together. When a reaction is reversed, the sign of its ?G° is also reversed, and when a reaction is multiplied by a factor, its ?G° is multiplied by the same factor. This manipulation enables the elimination of unwanted species and the construction of the target overall reaction from given steps.

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