The equilibrium constant, Kc, for the following reaction is 1.85×10-2 at 708 K. NH4I(s) NH3(g) + HI(g) Calculate Kc at this temperature for the following reaction: NH3(g) + HI(g) NH4I(s)

For the following equilibrium reaction: 2NO2(g) N2O4(g) + Δ What happens if the pressure of the reaction is increased?

The equilibrium constant, Kp. for the following reaction is 55.6 at 698 K. H2(g) + I2(g)2HI(g) If AH° for this reaction is -10.4 kJ, what is the value of K, at 619 K? Kp=

The equilibrium constant, Kc, for the following reaction is 1.48×10-2 at 604 K.COCl2(g) CO(g) + Cl2(g)Calculate Kc at this temperature for:CO(g) + Cl2(g) COCl2(g)Kc =

A mixture of gaseous CO and H2, called synthesis gas, is used commercially to prepare methanol (CH3OH), a compound considered an alternative fuel to gasoline. Under equilibrium conditions at 570.3  K, [H2] = 0.06302  mol/L, [CO] = 0.03125  mol/L, and [CH3OH] = 0.0401 mol/L. What is the value of Kc for this reaction at 570.3  K?

The equilibrium constant is given for two of the reactions below. Determine the value of the missing equilibrium constant. NO(g) +½ Br2(g) = NOBr(g) K = 5.3 2 NO(g) = N2(g) + O2(g) Kc = 2.1 ×1030 N2(g) + Br2(g) + O2(g) = 2 NOBr(g) Kc = = ? Select one: O 1.3 x 10-20 O 0.12 O 1.3 x 10-29 O 2.8 x 104

Consider the following reaction: SO2 Cl2 (g) = SO2 (g) + Cl2 (g) K. = 2.99 x 10-7 at 227 ° C You may want to reference (Page) Section 15.8 while completing this problem.

An equilibrium mixture of dinitrogen tetroxide, N2O4, and nitrogen dioxide, NO2, is 78.3% NO2 by mass at 1.00 atm pressure and 25°C. Calculate Ke at 25°C for the reaction N204 (9) = 2NO2 (g) Ke =

The equilibrium constant, Kc, for the following reaction is 1.20×10-2 at 500 K. Calculate K, for this reaction at this temperature. PCI5(g) PCI3(9) + Cl2(g) Kp

The equilibrium                         4 NH3(g) + 4 O2(g)  ⇆  2 N2O (g) + 6 H2O(l)           ΔHo = −142 kJ/mol Is established in a sealed container with a piston. Which of the following actions will increase the amount of the products present at equilibrium?             I    Increasing the volume of the container             II   Reducing the volume of the container             III  Removing some of the H2O(l) from the container             IV  Adding some NH3(g) to the container             V   Adding N2(g) to the container             VI  Raising the temperature             VII Lowering the temperature