CO(g ) + H2O(g ) <---> CO2(g ) + H2(g ), Kc = 0.0611 at 2000 K . A reaction mixture initially contains a CO partial pressure of 2.50 atm, an H2O partial pressure of 2.50 atm, a CO2 partial pressure of 1.00 atm, and an H2 partial pressure of 1.00 atm at 2000 K. Calculate the equilibrium partial pressure of CO

 Thus equilibrium partial pressure of CO is 1.306 atm

Explanation:

is the constant of a certain reaction at equilibrium.

For the given chemical reaction:

at t=0     2.50      2.50                  1.00         1.00

at em     (2.50-x)    (2.50-x)         (1.00+x)       (1.00+x)

The expression of for above equation follows:

Putting values in above equation, we get:

Thus equilibrium partial pressure of CO = (1.00+x) = (1.00+ 0.306) = 1.306 atm

the positions which points up in upward carbon and down in downward carbon are axial

and vice versa holds true for equatorial positions

so the correct answer with labelled diagram will be