Consider the following reaction:

CO(g)+H2O(g)⇌CO2(g)+H2(g)
Kp=0.0611 at 2000 K
A reaction mixture initially contains a CO partial pressure of 1348torr and a H2O partial pressure of 1780torr at 2000 K.

Calculate the equilibrium partial pressure of CO2.
Calculate the equilibrium partial pressure of H2.

pCO = (1348/760) = approx 1.8 atm but you need to do it more accurately.

pH2O = 1780/760 = approx 2.3 atm.
.........CO(g)+H2O(g)⇌CO2(g)+H2(g)
I.......1.8....2.3.....0......0
C.......-x......-x.....x......x
E......1.8-x...2.3-x...x......x

Substitute the E line into Kp expression and solve for x = pCO2 = pH2.

To calculate the equilibrium partial pressures of CO2 and H2, we need to use the given equilibrium constant (Kp) and the initial partial pressures of CO (carbon monoxide) and H2O (water).

Step 1: Write the balanced equation for the reaction.
CO(g) + H2O(g) ⇌ CO2(g) + H2(g)

Step 2: Prepare an ICE (Initial, Change, Equilibrium) table.
Initial: CO = 1348 torr, H2O = 1780 torr, CO2 = 0 torr, H2 = 0 torr
Change: Let x be the change in partial pressure for CO and H2O.
Equilibrium: CO = 1348 - x, H2O = 1780 - x, CO2 = x, H2 = x

Step 3: Determine the expression for the equilibrium constant (Kp).
Kp = (P_CO2 * P_H2) / (P_CO * P_H2O)
Given: Kp = 0.0611

Step 4: Substitute the equilibrium partial pressures into the expression for Kp.
0.0611 = (x * x) / ((1348 - x) * (1780 - x))

Step 5: Solve the equation for x.
Rearrange the equation to make it easier to solve:
0.0611 * (1348 - x) * (1780 - x) = x^2

Expand the equation:
(0.0611 * (1780 - x) * (1348 - x)) - x^2 = 0

Simplify the equation:
x^2 + 41.5348x - 25010.6324 = 0

Now you can solve this quadratic equation for x. Use any method like factoring, completing the square, or the quadratic formula to find the value of x. The positive solution will give you the correct value for equilibrium partial pressure.

Step 6: Calculate the equilibrium partial pressures of CO2 and H2.
Substitute the value of x back into the equilibrium expressions:
CO2 = x
H2 = x

Now, you can calculate the equilibrium partial pressure of CO2 and H2 using the value of x obtained from solving the quadratic equation in Step 5.