Given the following equilibrium, which of the following will result in an increased amount of Cl2(g)? 2SO3(g) + 2C12(g) = 2SO2C12(g) + O2(g) a. decrease the volume of the system, which increases the total pressure. O b. add some SO3(g) О с. SO3(g) remove some O d. remove some O2(g)

Consider the following equilibrium with K = 2.3 x 10-6: N2 ) + 3H2 (g) 2NH3 (g) 0.1 moles of N2, 0.1 moles of H2, and 0.01 moles of NH3 are placed in a 1 L container. Which of the following is true? O Q > K, the reaction will produce more products O Q = K, the reaction is at equilibrium O Q K, the reaction will produce more reactants

1C. Please don't write on a paper. I can't understand handwritten.

Consider the following reaction at equilibrium:2SO2(g) + O2 (g) <==> 2SO3(g)Determine if the following changes will increase, decrease or not affect the partial pressure of SO2.a. Decreasing the amount of oxygen in the systemb. Decreasing the volume of the systemc. Decreasing the temperature of the systemd. Decreasing the pressure of the systeme. Adding a catalyst to the reaction system

4. A. An important reaction in the commercial production of hydrogen is  CO(g) + H2O(g) --><-- H2(g) + CO2(g) How will the system at equilibrium shift in each of the five following cases? (Use arrows or write "right" , "left" , or "no shift").  a. Gaseous carbon monoxide is removed b. In rigid reaction container, a catalyst is added. c. The temperature is decreased (the reaction is exothermic). d. The reaction container volume is doubled. e. Hydrogen gas is added. B. The equation above has a Kc value of 7.5 x 102. If 2.0 moles of each reactant and product are put into the same sealed 4.0 L container, determine the concentrations of all species present at equilibrium. Please answer A with sub parts and B.

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.

23 and 24 please

For the equilibrium system below, which of the following would result in an increase in the quantity of CO(g)? 2H₂(g) + CO(g) CH3OH(g) + 92 kJ A. decreasing temperature B. decreasing the volume of the container C. adding some CH3OH D. both a and b E. both b and c 101

4. The hypothetical reaction shown below has a Kc = 4.0 x 103 at 500 K. The equilibrium partial pressures for A2 and AB3 are 2.0 atm and 1.3 atm, respectively. What is the equilibrium partial pressure of B2? * A2(g) +3 B2(g) 2 AB3(g) O 0.71 atm O 0.09 atm O 0.06 atm O 0.94 atm