What is the equilibrium constant, K, at 400K if 3.00 moles of CO2(g) introduced into a 2 liter container are 20.0% dissociated at equilibrium?
2 CO2(g) « 2CO(g) + O2(g)
A. (0.30)2(0.15) / (1.20)2 mol/liter
B. (1.20)2 / (0.30)2(0.15) mol/liter
C. (0.60)2(0.30) / (2.40)2 mol/liter
D. (2.40)2 / (0.60)2(0.30) mol/liter
E. (0.30)2(0.15) / (2.40)2 mol/liter
Answer is A can anyone explain this step by step...i'm having trouble with the mole conversion..thanks!
2 CO2(g) « 2CO(g) + O2(g)
A. (0.30)2(0.15) / (1.20)2 mol/liter
B. (1.20)2 / (0.30)2(0.15) mol/liter
C. (0.60)2(0.30) / (2.40)2 mol/liter
D. (2.40)2 / (0.60)2(0.30) mol/liter
E. (0.30)2(0.15) / (2.40)2 mol/liter
Answer is A can anyone explain this step by step...i'm having trouble with the mole conversion..thanks!