When 15.0 mL of a 7.21×10-4 M copper(II) chloride solution is combined with 12.0 mL of a 3.67×10-4 M ammonium carbonate solution does a precipitate form? _________  (yes or no)For these conditions the Reaction Quotient, Q, is equal to ________.   When 15.0 mL of a 3.58×10-4 M lead acetate solution is combined with 22.0 mL of a 1.87×10-4 M potassium bromide solution does a precipitate form?___________ (yes or no)For these conditions the Reaction Quotient, Q, is equal to ____________.

Express the equilibrium constant for the following reaction.

1. Solid silver sulfate and solid calcium sulfate are in equilibrium with a solution containing 1 .18×10-2 M silver acetate. Calculate the concentration of calcium ion present in this solution.[calcium] = M   2. Solid cobalt(II) carbonate and solid cobalt(II) sulfide are in equilibrium with a solution containing 7.46×10-3 M sodium carbonate. Calculate the concentration of sulfide ion present in this solution.[sulfide] = M   3. Solid calcium sulfite and solid barium sulfite are in equilibrium with a solution containing 5.98×10-3 M barium acetate. Calculate the concentration of calcium ion present in this solution.[calcium] = M

For the balanced reaction equation given below, 0.500 moles of H2 and 0.500 moles of I2 are placed in a 10.0 L reaction vessel.  At equilibrium the concentration of HI was measure to be 0.078 M.  Determine Kc for this reaction. H2(g) + I2(g)              ↔                  2HI(g)

Consider the general reaction below. 2A(g) + B₂(g) = 2AB(g) K = 6.4 x 10-6 @ 298 K The reaction was initiated by combining 0.70 mol A and 0.90 mol B2 in a 2.0 L container. Calculate the equilibrium concentrations of the components. What is the equilibrium concentration of AB? 10[? ] [AB] = [?] x 10¹ M

What is the equilibrium-constant expression for the following reaction?N2O4 (g)  <--> 2NO2 (g)

For the following reaction :   H2 (g)   +   I2 (g)     2HI (g) it was found that a 13.0L vessel at equilibrium contained 0.852 mol H2, 0.361 mol I2, and 2.99 mol of HI.  A)   Write an expression for Kc. B).  Determine the value of Kc for this reaction.

Nitrogen monoxide, NO, is formed in automobile exhaust by the reaction of N2 and Og (from air). N2 (9) + O2(9) - 2NO(9) The equilibrium constant (K.) is 0.0025 at 2127°C. If an equilibrium mixture at this temperature contains 0.082 mol N, and 0.026 mol O2 per liter, what is the concentration of NO? Concentration = M