Consider the reaction I2(g) ⇌ 2 I(g), which is endothermic as written. What would be the effect on the equilibrium position of removing I(g)?   A. Reaction would go to the left, making more "products"   B. No change on the equilibrium position   C. Reaction would go to the right, making more "products"   D. Reaction would go to the right, making more "reactants"   E. Reaction would go to the left, making more "reactants"

Consider the following exothermic reaction: C (s)   +   2 Cl2 (g)   ⇋⇋   CCl4 (g) How would the equilibrium shift if the reaction mixture is heated? Select one: a. The reaction would shift towards the products. b. The reaction would shift towards the reactants. c. The equilibrium would not be affected.

Consider the following system at equilibrium at 600 K:COCl2(g) =CO(g) + Cl2(g)When some COCl2(g) is added to the equilibrium system at constant temperature: The reaction must: fill in the blank 1 A. Run in the forward direction to restablish equilibrium.     B. Run in the reverse direction to restablish equilibrium.     C. Remain the same. Already at equilibrium.   The concentration of CO will: fill in the blank 2 A. Increase.     B. Decrease.     C. Remain the same.

The decomposition of PCl5 occurs by the equilibrium process          PCl5(g) = PCl3(g) + Cl2(g)             DH, = 92.5 kJ mol–1   If the reaction is initially at equilibrium, explain what happens when the temperature is lowered. Select one: a. The equilibrium shifts left b. The concentration of Cl2(g) will increase c. No change d. The equilibrium shifts right

Assume that the following exothermic chemical reaction is at equilibrium. CuO (s) + H2 (g) ⇌ H2O (g) + Cu (s). Which of the following statements is CORRECT? Choose one option. a. Increasing the concentration of H2 (g) will cause the reaction to proceed in the backward direction (shift to left), increasing the equilibrium concentration of H2O (g). b. Decreasing the temperature will cause the reaction to proceed in the forward direction (shift to right), increasing the equilibrium concentration of H2O (g). c. Increasing the amount of CuO(s) will cause the reaction to proceed in the forward direction, increasing the equilibrium concentration of H2O (g). d. Increasing the temperature will cause the reaction to proceed in the forward direction (shift to right), increasing the value of the equilibrium constant of this reaction. e. The value of the equilibrium constant for this reaction will stay the same after the temperature is increased.

23 and 24 please

Which reaction, when at equilibrium, would be unaffected by a change in pressure? A. N2(g) + O2 (g) = 2NO(g) B. 2CO(g) + O2 = 2CO2(g) C. COBr2(g) = CO(g) + Br2(g) D. N2O4(g) = 2NO2 (g)

Mechanistic arrows always show.... A) Electron movement from nucleophiles to electrophiles B) Proton transfer from Lewis bases to Lewis acids C) Proton transfer from Brønsted-Lowry bases to Brønsted-Lowry acids D) Atom movement when new bonds are being made

Consider the following exothermic reaction: C (s)   +   2 Cl2 (g)   ⇋⇋   CCl4 (g) How would the equilibrium shift if the reaction mixture is heated? Select one: a. The reaction would shift towards the products. b. The reaction would shift towards the reactants. c. The equilibrium would not be affected.