Consider the following chemical reaction: CO (g) + 2H₂(g) CH₃OH(g)
At equilibrium in a particular experiment,the concentrations of CO and H₂ were and respectively.What is the equilibrium concentration of CH₃OH?
The value of K_eq for this reaction is 14.5 at the temperature of the experiment.

Question

Consider the following chemical reaction: CO (g) + 2H₂(g)

Consider the following chemical reaction: CO (g) + 2H<sub>2</sub>(g) CH<sub>3</sub>OH(g) At equilibrium in a particular experiment,the concentrations of CO and H<sub>2</sub> were and respectively.What is the equilibrium concentration of CH<sub>3</sub>OH? The value of K<sub>eq</sub> for this reaction is 14.5 at the temperature of the experiment. A) 14.5 B) 7.61 × 10<sup>-3</sup> C) 2.82 × 10<sup>-1</sup> D) 3.72 × 10<sup>-3</sup> E) 1.34 × 10<sup>-3</sup>

CH₃OH(g)
At equilibrium in a particular experiment,the concentrations of CO and H₂ were

and

respectively.What is the equilibrium concentration of CH₃OH?
The value of K_eq for this reaction is 14.5 at the temperature of the experiment.

Quizplus · Accepted Answer

Using the balanced chemical equation, we can set up an ICE table: CO (g) + 2 H₂(g) <--> CH₃OH(g) I 11ea7e7c_6154_23a1_9a0a_cd51236e2dcd_TB1194_11 11ea7e7c_6154_23a3_9a0a_4b4a1c4d1e45_TB1194_11 0 C -x -2x +x E (at equilibrium) 11ea7e7c_6154_23a1_9a0a_cd51236e2dcd_TB1194_11 - x 11ea7e7c_6154_23a3_9a0a_4b4a1c4d1e45_TB1194_11 - 2x x We can use the equilibrium constant expression to solve for x: K_eq = [CH₃OH]/[CO][H₂]2 14.5 = x/[(11ea7e7c_6154_23a1_9a0a_cd51236e2dcd_TB1194_11)(11ea7e7c_6154_23a3_9a0a_4b4a1c4d1e45_TB1194_11)2] x = (14.5)(11ea7e7c_6154_23a1_9a0a_cd51236e2dcd_TB1194_11)(11ea7e7c_6154_23a3_9a0a_4b4a1c4d1e45_TB1194_11)2 x = 2.82 x 10^-1 Therefore, the equilibrium concentration of CH₃OH is 2.82 x 10^-1. The correct answer choice is C.

Consider the Following Chemical Reaction: CO (G)+ 2H2(g) CH3OH(g)

Consider the Following Chemical Reaction: CO (G)+ 2H₂(g) CH₃OH(g)