Equilibrium pressures of gases?

Question

Suppose 1.44 atm of CH4(g), 2.28 atm of C2H6(g), and 16.16 atm of O2(g) are placed in a flask at a given temperature. The reactions are given below.

CH4(g) 2 O2(g) CO2(g) 2 H2O(g) KP = 1.0 104

2 C2H6(g) 7 O2(g) 4 CO2(g) 6 H2O(g) KP = 1.0 108

Calculate the equilibrium pressures of all gases.

PCH4

atm

PC2H6

atm

Answer 1

because both Kp are high,from reactions u get only products,no reactants remaining;O2 is excedentary

pCH4=pC2H6=0

rigouros:verrrrrrrrrrrrrry nasty

and at the temperature necesary to establish eql.other reactions step up.

Answer 2

eq P of all gases are = 10^(1.0X10^4 +1.0X 10^8)