CO2 + H2 yields H20 + CO all are in gaseous state Kc for reaction at 2000K is 5.

Question

CO2  + H2  yields H20 + CO   all are in gaseous state

Kc for reaction at 2000K is 5.0

Initial concentration of H2 = .2 mol/L    Initial concentration of CO2 = .30 mol/L   Initial concentration of H20 and CO = .55 mol/L

When system is cooled to a lower temp, 30.0 % of the CO is converted back to CO2  Calculate value of Kc at this lower temp

In a different experiment .50 mole of H2 is mixed with .50 mole CO2 in 3.0 L vessel at 2000K  Calculate equilibrium concentration in moles/L of CO at this temp

Explanation / Answer

For system being cooled down to lower temperature

Concentration of CO = .55*.7 = .385

Concentration of CO2 = .3 + (.55-.385) = .465

Concentration of H2O = .55*.7 = .385

Concentration of H2 = .2 + .55 - .385 = .365

kc = [H2O][CO]/[H2][CO2]

    = .873

Initial concentration of CO2 = .5/3 mol/l

Initial concentration of H2 = .5/3 mol/l

Assuming final concentration of CO to be x mol/l

Final concentration of CO2 and H2 = .167 - x

Final concentration of H2O = x

kc = (x^2)/(.167 - x)^2 = 5

Solving for x gives

x = .115 moles/L

Related Questions

Navigate

• Browse (All)
• Browse C
• Subjects

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.