Predict the direction of a reaction by comparing Q and K
Consider the following reaction and its equilibrium constant: I2 (g) + Cl2 (g) <-- --> 2ICI (g) Kp = 81.9
A reaction mixture contains P I2 = 0.114 atm, P Cl2 = 0.102 atm, P ICI = 0.355 atm. Is the reaction mixture at equilibrium? If not, in which direction will the reaction proceed?
Consider the following reaction and its equilibrium constant: N2O4 (g) <-- --> 2 NO2 (g) Kc = 5.85 X 10^-3
A reaction mixture contains [NO2] = 0.0255M and [N2O4] = 0.0331M. Calculate Qc, and determine the direction in which the reaction will proceed.
For the reaction N2O4 (g) <-- --> 2 NO2 (g), a reaction mixture at a certain temperature initially contains both N2O4 and NO2 in their standard state. If Kp = 0.15, determine the direction in which the reaction will proceed.
Consider the reaction: NH4HS (s) <-- --> NH3 (g) + H2S (g)
At a certain temperature, Kc = 8.5 X 10^-3. A reaction mixture at this temperature containing solid NH4HS has [NH3]= 0.166M and [H2S] = 0.166M. Will more of the solid form or will some of the existing solid decompose as equilibrium is reached?
Silver sulfate dissolves in water according to the reaction:
Ag2SO4(s) <-- --> 2Ag+ (aq) + SO4 ^2- (aq) Kc = 1.1 X 10^-5 at 298K. A 1.5L solution contains 6.55g of dissolved silver sulfate. IF additional solid silver sulfate is added to the solution will it dissolve?