A sealed 1.00L flask is charged with 0.500 mol of I, and 0.500 mol of Br. An equilibrium reaction ensues: 12 (g) + Br2 (g) = 2 IBr (g) When the container contents achieve equilibrium, the flask contains 0.84 mol of IBr. The value of K is Select one: O a. K= 6.10 O b. K= 2.82 OC K =882 Od. K= 110 2eK=131

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

Consider the equilibrium system described by the chemical reaction below, which has a value of Kc equal to 1.2×10-4 at a certain temperature.  If a solid sample of NH4SH decomposes, what is the equilibrium concentration of NH3 be?

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.