20. What will happen to the equilibrium when more SO2 (g) is added to the following system? 2502(g) + O2(g) = 2803(g) A. It will shift to the right. B. It will shift to the left C. no shift of equilibrium D. cannot be determined 21. For the reaction 2A +B2C the appropriate form for the equilibrium constant expression is: A. [A][B12/(C) B. [A][B]/[C2 C. [C²/ [A][B] D. [A][BC] 22. Calculate K for the following reaction given the following equilibrium concentrations of H2, CO, and H₂O. K=? PCIs(g) → PCk3(g) + Cl₂(g) .200 .040 .080 Equilibrium Concentrations (M): A. 0.16 D.16 B.0.016 C.1.6

Consider the equilibrium system described by the chemical reaction below, which has a value of Kc equal to 1.2 x 104 at a certain temperature. If a solid sample of NH.SH decomposes, what will the equilibrium concentration of NH3 be? NH:SH(s) = NH3(g) + H2S(g) 1 2 3 NEXT > Based on the given values, set up ICE table in order to determine the unknown. NH.SH(s) NH:(g) H2S(g) Initial (M) Change (M) Equilibrium (M) RESET 1.2 x 104 +x +2x -2x 1.2 x 104 + x 1.2 x 104 - x 1.2 x 104 + 2x 1.2 x 104- 2x

The equilibrium constant of Br2(g) + F2(g) + 2BRF(g) is 54.7. Calculate the equilibrium concentration of BrF if the initial concentrations of Br2 and F2 are 0.25 mol/L? а. 1.25 b. 0.72 О с. 0.38 O d. 0.555 е. 0.205

Consider the following system at equilibrium at 350 K: ? CHĄ(g) + CCl4(g) 2CH,Cl,(g) When some CCI,(g) is removed from the equilibrium system at constant temperature: The reaction must: 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 CH4 will: | A. Increase. B. Decrease. C. Remain the same.