Question

The synthesis of methanol from carbon monoxide and hydrogen gas is described by the following chemical equation:

CO(g)+2H2(g)⇌CH3OH(g)CO(g)+2H2(g)⇌CH3OH(g)

The equilibrium constant for this reaction at 25 ∘C∘C is Kc=2.3×104Kc=2.3×104. In this tutorial, you will use the equilibrium-constant expression to find the concentration of methanol at equilibrium, given the concentration of the reactants.

1. a. Suppose that the molar concentrations for COCO and H2H2 at equilibrium are [CO][CO] = 0.04 MM and [H2][H2] = 0.04 MM. Use the formula you found in Part B to calculate the concentration of CH3OHCH3OH.

Express your answer to one decimal place and include the appropriate units.

b. Consider the reaction:
CO(g)+H2O(g)⇌CO2(g)+H2(g)CO(g)+H2O(g)⇌CO2(g)+H2(g)
An equilibrium mixture of this reaction at a certain temperature was found to have [CO][CO]= 0.0213 MM , [H2O][H2O]= 0.0125 MM , [CO2][CO2]= 0.205 MM , and [H2][H2]= 0.0314 MM .

What is the value of the equilibrium constant at this temperature?

c.

An equilibrium mixture of the following reaction was found to have [I2]=0.0375M[I2]=0.0375M at 1200 ∘C∘C: I2(g)⇌2I(g)I2(g)⇌2I(g) Keq=1.0×10−2Keq=1.0×10−2 at 1200 ∘C

What is the concentration of I? Express your answer using two significant figures.

Answer 1

a) (018) + 2H₂(g) (H₂OH (9) ķ= 2.3x104 [CH OH] = ? ; [co] = 0.04M , [ty] = 0.04M ka= [CH₂OH] [CH OH] = kx [co] [Hz]2 = 2.3 X 10" x 10.04) 10.04? 1) [co] [H₂]2 => [Ch404) = 0.0001472 x 10 = 1.472 Concentratim = [CHOH) = 1.5 M =[CH, OH 7 = 1.5M | of methand b) Colo+ho (g) (O₂(g) + H₂19) [co] = 0.0213M [ho] = 0.0125M; [CO₂] = 0.205M; CH] = 0.0314M Ka - [103] [Hz] (0.20 54 (0.03148 - 24.1765258 [co] [H0] (0.0213M) (0.0125M) [Kc = 24.18 equilibrium constant c) I, 21(9) ; [[2] = 0.0375m, Keg. = 10x102 Keq. = [1927 (I)? = keq. (Ie] 7 [1] = d Key. [In] =) (1.0X10%)x (0.0315) = 0.0193649 [I] = 0.0194 concentration of I = | [1] = 0.019