Consider the reaction 2 NO2(g) ⇌N2 O4(g) 2 H2 S(g)+SO2(g) ⇌3 Sthombic (s)+2 H2 O(g)For each of t

step 1 So continuing on with some work based on thermodynamics, the first step we have here is to calcu

Consider the reaction 2 NO2(g) ⇌N2 O4(g) 2 H2 S(g)+SO2(g) ⇌3...

Consider the reaction $$2 \mathrm{NO}_{2}(g) \rightleftharpoons \mathrm{N}_{2} \mathrm{O}_{4}(g)$$ $$2 \mathrm{H}_{2} \mathrm{S}(g)+\mathrm{SO}_{2}(g) \rightleftharpoons 3 \mathrm{S}_{\text {thombic }}(s)+2 \mathrm{H}_{2} \mathrm{O}(g)$$For each of the following mixtures of reactants and products at $25^{\circ} \mathrm{C},$ predict the direction in which the reaction will shift to reach equilibrium. a. $P_{\mathrm{NO}_{2}}=P_{\mathrm{N}_{2} \mathrm{O}_{4}}=1.0 \mathrm{atm}$ b. $P_{\mathrm{NO}_{2}}=0.21 \mathrm{atm}, P_{\mathrm{N}_{2} \mathrm{O}_{4}}=0.50 \mathrm{atm}$ c. $P_{\mathrm{NO}_{2}}=0.29 \mathrm{atm}, P_{\mathrm{N}_{2} \mathrm{O}_{4}}=1.6 \mathrm{atm}$

Consider the reaction $$2 \mathrm{NO}_{2}(g) \rightleftharpoons \mathrm{N}_{2} \mathrm{O}_{4}(g)$$ $$2 \mathrm{H}_{2} \mathrm{S}(g)+\mathrm{SO}_{2}(g) \rightleftharpoons 3 \mathrm{S}_{\text {thombic }}(s)+2 \mathrm{H}_{2} \mathrm{O}(g)$$For each of the following mixtures of reactants and products at $25^{\circ} \mathrm{C},$ predict the direction in which the reaction will shift to reach equilibrium.
a. $P_{\mathrm{NO}_{2}}=P_{\mathrm{N}_{2} \mathrm{O}_{4}}=1.0 \mathrm{atm}$
b. $P_{\mathrm{NO}_{2}}=0.21 \mathrm{atm}, P_{\mathrm{N}_{2} \mathrm{O}_{4}}=0.50 \mathrm{atm}$
c. $P_{\mathrm{NO}_{2}}=0.29 \mathrm{atm}, P_{\mathrm{N}_{2} \mathrm{O}_{4}}=1.6 \mathrm{atm}$

Key Concepts

Partial Pressure in Gaseous Equilibria

In reactions involving gases, partial pressure is a measure of the individual gas's contribution to the total pressure, and it is a key component in writing and understanding the equilibrium constant expression. Since only gases (and not pure solids or liquids) typically appear in the equilibrium expression, the partial pressures help in determining the reaction quotient and predicting the shift of the reaction under non-equilibrium conditions.

Le Chatelier’s Principle

Le Chatelier’s Principle states that if a dynamic equilibrium is disturbed by changing the conditions, such as pressure, concentration, or temperature, the system will adjust itself to partially counteract the disturbance and re-establish equilibrium. This principle helps predict the direction in which the reaction will shift when the concentrations, pressures, or other conditions are altered.

Equilibrium Constant (K)

The equilibrium constant, K, is a fixed value at a given temperature that expresses the ratio of the concentrations or partial pressures of products to reactants at equilibrium. In gaseous reactions, K may be expressed in terms of partial pressures and is used as a reference point to determine whether the system is at equilibrium or if the reaction needs to shift in a particular direction to achieve equilibrium.

Reaction Quotient (Q)

The reaction quotient, Q, is a measure of the ratio of the concentrations or partial pressures of products to reactants at any point in time, not just at equilibrium. Comparing Q to the equilibrium constant, K, allows us to predict the direction in which the reaction will shift in order to reach equilibrium. If Q is less than K, the reaction will proceed in the forward direction to produce more products; if Q is greater than K, it will shift in the reverse direction to produce more reactants.

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