This reaction is endothermic. C(s) + CO2(g) =2 CO(g) Predict the effect (shift right, shift left, or no effect) of increasing and decreasing the reaction temperature. How does the value of the equilibrium constant depend on temperature?

Suppose the following exothermic reaction UO2(s)+4HF(g) UFA(g) + 2H20(g) has already reached equilibrium. Predict the effect that each of the following changes will have on the equilibrium position. State whether the equilibrium will shift to the reactants, will shift to the products, or will not be affected. Explain your answer using Le Chatelier's Principle. a. The system was cooled. b. The reaction vessel was quadrupled. C. Uranium (IV) oxide was added to the reaction. d. The partial pressure of Uranium (IV) fluoride was decreased.

The reaction is at equilibrium at some temperature, T, and the following equilibrium concentrations are measured: [SO2] = 0.90 M, [O2] = 0.35 M, and [SO3] = 1.1 M. Write the equilibrium expression for this reaction. Calculate Keq for the reaction at temperature, T.

For the following reaction, the equilibrium constant Keq is 6.40 x 10-7 at 2000°C. 2CO2 (g)  2CO (g) + O2 (g) If 0.250 moles of CO2(g) is introduced into a 1.00 L vessel, calculate the equilibrium concentrations of CO(g) and O2(g) at this temperature.