- #1
rdayabhai
- 1
- 0
General Chemistry -- Chemical Equilibria
Suppose 1.22 atm of CH4(g), 2.57 atm of C2H6(g), and 15.00 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 = 1.0x10^4
2 C2H6(g) + 7 O2(g) 4 CO2(g) + 6 H2O(g) KP = 1.0x10^8
Calculate the equilibrium pressures of all gases.
---
There seems to one unknown that cannot be solved for! Any help is appreciated! (I'd rather not have you post the answer, but rather the method) Thanks.
Suppose 1.22 atm of CH4(g), 2.57 atm of C2H6(g), and 15.00 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 = 1.0x10^4
2 C2H6(g) + 7 O2(g) 4 CO2(g) + 6 H2O(g) KP = 1.0x10^8
Calculate the equilibrium pressures of all gases.
---
There seems to one unknown that cannot be solved for! Any help is appreciated! (I'd rather not have you post the answer, but rather the method) Thanks.
Last edited: