Consider the following reaction at equilibrium: N₂O₄(g) ⇌ 2NO₂(g) The ∆H° for this reaction is > 0. If the temperature is increased by 20.0 K while the volume is kept constant, in which direction will the equilibrium shift?

Consider the reaction at equilibrium 2KCl(s) + 3O2(g) ⇌  2KClO3(s). ΔH° for this process is +78.6kJ. Predict whether the reaction will shift left, shift right, or remain unchanged after each disturbance. a) O2(g) is removed from the reaction vessel. b) KCl(s) is added to the reaction vessel c) The volume of the vessel is reduced by 50% d) The temperature of the system is raised

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Consider the following reaction at equilibrium: 2NO₂(g) ⇌ N₂O₄(g) The ∆H° for this reaction is < 0. If the volume of the container is decreased by ½ while the temperature is kept constant, how will K(eq) change?

For the gas-phase equilibrium A(g) + 2 B(g) = C(g) the initial partial pressures of A, B, and C are all 0.300 atm. After equilibrium is established at 25°C, it is found that the partial pressure of C is 0.270 atm. What is AG° for this reaction? (R = 8.314 J/mol · K). kJ/mol 1 3 4 C 7 8 9 +/- x 100 + 2.

(a)        N2(g)               +          O2(g)                           2NO (g)            ∆H298 = + 180 kJ mol-1    From the equilibrium shown above, use Le Chatelier’s Principle to decide what happens to the equilibrium position by:   Increasing the concentration of NO Increasing the pressure Increasing the temperature Increasing the concentration of N2 Adding a catalyst

2 Consider the following equilibrium: A + 2 B 3C +D Are the reactants or K = 1.5 ×10³ products favored at equilibrium?