The equilibrium PC13 + 0.20 composition for the reaction is - PC15 0.40 moles/litre If 0.20 mole of Cl, is added at same temp. Find equilibrium concentration of PC1, (Kc= 20) (A) 0.48 moles (C) 0.56 moles Cl₂ 0.10 (B) 0.38 moles (D) 1.20 moles

b and c please

21. When the system is not at equilibrium, the reaction quotient Q for any reaction ... (A) will indicate if more reactants or products will be made. (B) will go up or down as determined by the equilibrium constant (C) will change over time until it is equal to the equilibrium constant. (D) will depend on the reaction stoichiometry. (E) All of the above.

Iodine and bromine react to give iodine monobromide, IBr. I1 (9) + Brz (9) = 2IB:(9) What is the equilibrium composition of a mixture at 154°C that initially contained 1.10 x 10- mol each of iodine and bromine in a 5.00 L vessel? The equilibrium constant K, for this reaction at 154°C is 130. [1:] =( M [Bra] =( M [IBr] = M

Give a clear handwritten answer with explanation....asap

Please help with this

(a) Determine whether the value of K of an equilibrium system will be affected or, unaffected by the following changes: Changes Value of K (affected or unaffected) (O Decreasing the temperature (1) Increasing the pressure of the system () Decreasing the concentration of reactant (b) The following graph represents the amount of CO formed at two different temperatures, T; and T. The reaction as shown below: C() + H,O(g) = co(g) + H(g) T = 385 K [co) T = 335 K time Based on the graph, determine whether the forward reaction is endothermic or exothermic. Predict if the concentration of H:0 gas increases, decreases or remains the same if the temperature is decreased to 298 K. Explain. A mixture of 0.350 M of H:0, 0.125 M of CO and 0.125 M of H: was prepared and allowed to reach equilibrium in a 1.00 L flask. The equilibrium concentration of H;0 is 0.182 M. Calculate the Ke of the reaction at constant temperature. (H)

Determine the equilibrium concentration of H2S