Additional solid silver sulfate, a slightly soluble solid, is added to a solution of silver ion and sulfate ion at equilibrium with solid silver sulfate.2Ag+(aq) + SO4 2−(aq) ⇌ Ag2 SO4(s)Which of the following will occur?(a) Ag+ or SO4 2− concentrations will not change.(b) The added silver sulfate will dissolve.(c) Additional silver sulfate will form and precipitate from solution as Ag+ ions and SO4 2− ions combine.(d) The Ag+ ion concentration will increase and the SO4 2− ion concentration will decrease.

Expectation:investigate the qualitative and quantitative nature of chemical systems at equilibrium, and solve related problems.

The equilibrium constant, Ke, for the following reaction is 1.89×10-2 at 718 K. 2HI(g) H,(g) + I2(g) Calculate K. at this temperature for: H2(g) + I2(g) 2HI(g) Ke

C2,H2905S- (ag) + NH,CI (ag) → C2,H29O5SH (ag) + NH3 (aq) Yellow Blue Reaction after it reaches equilibrium appears Green A. Assume the reaction mixture is at equilibrium, appearing green in color, and at room temperature before each of the following disturbances. Explain which direction the reaction shifts to re-establish equilibrium and predict how the color of the solution will change 1.100 mL of water, H2O is added to the reaction mixture. 2. Solid platinum, Pt, is added to the reaction mixture. It reacts with NH3 to form N and H2 gasses. B. When the green reaction mixture at equilibrium is heated the color changes to green-blue, and then eventually, a dark blue color. When the green reaction mixture at equilibrium is placed in an ice water bath the solution color changes to a yellow-green, and eventually a bright yellow color. Is the reaction exothermic or endothermic? |