Part A It is possible to predict the equilibrium constant of a reaction by combi

Question

Part A It is possible to predict the equilibrium constant of a reaction by combining two or more reactions for which the value of K is known. When combining equilibrium constants, it is important to note the following: Determine the value of the equilibrium constant, Kal, for the reaction C(s)+] O2(g) + H2(g) CH,0H(g) + , c0(g). K.al.? by making use of the following information: 1. CO, (g) + 3H2(g) CH3OH(g) + H2O(g). 2. CO(g) +H20()CO2(8) +H2(8) 3. 2C(s) + 02(8) 2co(8) Express your answer numerically When a reaction is reversed, its K value is inverted; that is, K,everse = 1/Kforward Ki = 1.40 × 102 K21.00x 10 K, . When the coofficients of a reaction are multiplied by a factor, the K value is raised to the power of that factor When reactions are added, their K values are multiplied 2.10 × 1047 . View Available Hint(s) K goal

Explanation / Answer

Add all the three reactions, so the net reaction is

CO2 + 3H2 + CO + H2O + 2C + O2 -------------> CH3OH + H2O + CO2 + H2+ 2CO

Eliminate the common terms from both the sides

2H2 + 2C + O2 -------------> CH3OH + CO Kgoal = K1K2K3

Kgoal = K1K2K3

Divide by 2 through out

H2 + C + 1/2O2 -------------> 1/2CH3OH + 1/2CO Kgoal = (K1K2K3)1/2

Kgoal = (K1K2K3)1/2 = (1.40 x 102)x(1 x 105)x(2.10 x 1047)

Kgoal = (2.94 x 1054)1/2

Kgoal = 1.71 x 1027

so, the equlibirum constant for the raction is 1.71 x 1027

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