The equilibrium constant for the equation

Question

2 H2(g) + CO(g) CH3OH(g)
Is 19 at a certain temperature. If there are 3.11 x 10-2 moles of H2 and 5.79 x 10-3 moles of CH3OH at equilibrium in a 6.75 L flask. What is the concentration of CO?

At 1280 °C the equilibrium constant for the reaction
Br2(g) 2Br(g)
Is 1.1 x 10-3. If the initial concentrations are [Br2(g)] = 0.0310 M and [Br(g)] = 0.0210 M, calculate the concentrations of these 2 species in equilibrium

Answer 1

a.
Calculate (H2)&(CH3OH) from M = mols/L.
Then substitute these values into K expression and solve for the missing CO in M

b. I assume the K of 1.1E-3 is Kc and not Kp.
.........Br2(g) ==> 2Br(g)
I.....0.0310.......0.210
C........-x..........+2x
E....0.0310-x.......0.210+2x
Substitute the E line into the Kc expression and solve for x, then evaluate the other values.