Given CO (g) + H2O (g) <=> CO2 (g) + H2 (g) At a given temperature, Kp= 2.7. If

Question

Given CO (g) + H2O (g) <=> CO2 (g) + H2 (g)

At a given temperature, Kp= 2.7. If 0.13 mol of CO, 0.56 mol of H2O, 0.62 mol of CO2, and 0.43 mol of H2 are put into a 2.5 L flask, in which direction does the reaction proceed?

I tried finding the partial pressures by mol fraction= mol x/ mol total and then solving for Kp.
is this the correct method or do I just use the moles given as the mole fraction? Example: is the mole fraction of CO in this problem 0.13 mol CO / mol total = 0.74, or is the mole fraction just the amount of moles given in the question, 0.13 mol? Any help is appreciated.

Explanation / Answer

The mole fraction would be the mole of the chemical divided my total moles. so mole fraction of CO = .13/1.74 similarly mole fraction for H2O , CO2 and H2O are 0.56 / 1.74 , 0.62/1.74 and 0.43 / 1.74. also Q of reaction = 0.62*0.43 / 0.13*0.56 = 3.66 as conc. of product is more than that calculated by Kp so backward reaction would proceed. i.e. reaction from CO2 to CO

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