Consider the reaction 2 NO2(g) ⇌N2 O4(g) For each of the following mixtures of reactants and pro

step 1 I've written out all the information here, and we are given three situations. And in our first s

Consider the reaction 2 NO2(g) ⇌N2 O4(g) For each of the...

Consider the reaction $$2 \mathrm{NO}_{2}(g) \rightleftharpoons \mathrm{N}_{2} \mathrm{O}_{4}(g)$$ 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. $P_{\mathrm{NO}_{2}}=0.29 \mathrm{~atm}, P_{\mathrm{N}_{\mathrm{O}} \mathrm{O}_{4}}=1.6 \mathrm{~atm}$

Consider the reaction
$$2 \mathrm{NO}_{2}(g) \rightleftharpoons \mathrm{N}_{2} \mathrm{O}_{4}(g)$$
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. $P_{\mathrm{NO}_{2}}=0.29 \mathrm{~atm}, P_{\mathrm{N}_{\mathrm{O}} \mathrm{O}_{4}}=1.6 \mathrm{~atm}$

Key Concepts

Chemical Equilibrium

Chemical equilibrium occurs when the forward and reverse reaction rates become equal, resulting in constant concentrations (or partial pressures) for reactants and products. This concept forms the basis for understanding how reactions behave when they are disturbed and subsequently adjust to re-establish a balance.

Reaction Quotient and Equilibrium Constant

The reaction quotient (Q) is calculated by using the current concentrations or partial pressures of the reactants and products, raised to the power of their stoichiometric coefficients. Comparing Q to the equilibrium constant (K) indicates the direction in which a reaction must shift to reach equilibrium; if Q < K, the reaction proceeds forward to form more products, and if Q > K, it shifts in reverse to form more reactants.

Le Châtelier's Principle

Le Châtelier's Principle predicts how a system at equilibrium will respond when subjected to a change in conditions, such as concentration, pressure, or temperature. This principle is essential for determining the direction of the shift in equilibrium to counteract the disturbance and restore balance.

Partial Pressure

In gas-phase reactions, partial pressures represent the individual pressures exerted by each gaseous component. They are analogous to concentrations in solution reactions and are used to formulate the expressions for the reaction quotient (Q) and the equilibrium constant (K) in terms of pressure.

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