Consider the reaction: CO(g)+2 H2(g) ⇌ CH3 OH(g) Kp=2.26 ×10^4 at 25^∘ C Calculate

step 1 In this question, we're going to calculate the delta G value for the equation. C .L. plus 2H2, F

Consider the reaction: CO(g)+2 H2(g) ⇌ CH3 OH(g) ...

Consider the reaction: $$\begin{aligned} \mathrm{CO}(g)+2 \mathrm{H}_{2}(g) \rightleftharpoons & \mathrm{CH}_{3} \mathrm{OH}(g) \\ & K_{\mathrm{p}}=2.26 \times 10^{4} \text { at } 25^{\circ} \mathrm{C} \end{aligned}$$ Calculate $\Delta G_{\mathrm{rxn}}$ for the reaction at $25^{\circ} \mathrm{C}$ under each of the following conditions: a. standard conditions b. at equilibrium c. $P_{\mathrm{CH}_{3} \mathrm{OH}}=1.0 \mathrm{~atm} ; P_{\mathrm{CO}}=P_{\mathrm{H}_{2}}=0.010 \mathrm{~atm}$

Consider the reaction:
$$\begin{aligned}
\mathrm{CO}(g)+2 \mathrm{H}_{2}(g) \rightleftharpoons & \mathrm{CH}_{3} \mathrm{OH}(g) \\
& K_{\mathrm{p}}=2.26 \times 10^{4} \text { at } 25^{\circ} \mathrm{C}
\end{aligned}$$
Calculate $\Delta G_{\mathrm{rxn}}$ for the reaction at $25^{\circ} \mathrm{C}$ under each of the following conditions:
a. standard conditions
b. at equilibrium
c. $P_{\mathrm{CH}_{3} \mathrm{OH}}=1.0 \mathrm{~atm} ; P_{\mathrm{CO}}=P_{\mathrm{H}_{2}}=0.010 \mathrm{~atm}$

Key Concepts

Reaction Quotient

The reaction quotient (Q) is a ratio that compares the current activities or partial pressures of the reactants and products at any given moment, regardless of whether the system is at equilibrium. It is used in the equation ?G = ?G° + RT ln Q to determine the free energy change under non-standard conditions.

Non-Standard Conditions

Under non-standard conditions, the actual free energy change (?G) deviates from the standard free energy change (?G°) due to differences in reactant and product concentrations or pressures. The correction is accounted for by the term RT ln Q in the equation ?G = ?G° + RT ln Q, reflecting how shifts away from standard states affect the reaction's spontaneity.

Chemical Equilibrium

Chemical equilibrium occurs when the forward and reverse reactions occur at the same rate, resulting in constant concentrations or pressures of the reactants and products. At equilibrium, the reaction quotient Q equals the equilibrium constant K and the free energy change ?G for the reaction becomes zero, indicating no net driving force in either direction.

Standard Free Energy Change

The standard free energy change (?G°) is defined for reactions in which all reactants and products are in their standard states (typically 1 bar for gases and 1 M for solutions). It is directly related to the equilibrium constant (K) via the relation ?G° = -RT ln K, linking thermodynamics with equilibrium behavior.

Gibbs Free Energy

Gibbs free energy (?G) measures the maximum reversible work obtainable from a reaction at constant temperature and pressure. It is a key indicator of reaction spontaneity: a negative ?G indicates a spontaneous reaction, while a positive ?G signifies that the reaction is non-spontaneous.

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