Consider the graph below that displays the solubility of KCI in water as a function of temperature. 50 g of KCI is mixed with 100 g of water at 25 °C and is then heated to 50 °C. Select which statement best describes what would be observed as the system proceeds to establish equilibrium. 100 Solubility (g per 100 g H₂O) 80 60 40 20 0 20 KCI 40 60 Temperature (°C) 80 100 O a. A homogeneous solution of hydrated ions is initially observed, when a further 10 g of KCI is added, some of the added KCI is observed to dissolve, but some of the additional KCI remains in solid form. O b. A heterogenous system involving an equilibrium between hydrated KCI ions and solid KCI is observed. O c. A homogeneous solution of hydrated ions is initially observed, when a further 1 g of KCI is added, this additional KCI is also observed to dissolve. O d. A homogeneous solution of hydrated ions is observed before spontaneous crystallisation of KCI occurs when the solution is poured onto a crystal of KCI.

Suppose a 250. mL flask is filled with 0.20 mol of N2 and 2.0 mol of NO. The following reaction becomes possible: N2(g) + O2(g) = 2NO(g) The equilibrium constant K for this reaction is 0.693 at the temperature of the flask. Calculate the equilibrium molarity of N2. Round your answer to two decimal places. Шм

Consider the following equilibria: 2SO3(g)    2SO2(g) + O2(g)                       Kc1 = 2.3 × 10 – 7 2NO3(g) ⟷   2NO2(g) + O2(g)                       Kc2 = 1.4 ×10 – 3 Calculate the equilibrium constant for the reaction: SO2(g) + NO3(g)   ⟷ SO3(g) + NO2(g) A 1.3 × 10 – 2 B 1.6 × 10 – 4 C 78 D 6.1 × 103

Suppose a 250. mL flask is filled with 0.10 mol of CO, 0.30 mol of H,O and 1.8 mol of H,. The following reaction becomes possible: co(g) + H,0(g) =CO,{g)+H2(g) The equilibrium constant K for this reaction is 0.296 at the temperature of the flask. Calculate the equilibrium molarity of H,0. Round your answer to two decimal places.