The following equilibrium reaction has a Keq value of 2.5 x 10^7 (smaller/lower) 4
2CO2(g) <--> 2CO(g) + O2(g)
Calculate the equilibrium concentrations of all gases if 0.600 mol of CO2(g) is initially placed in a 3.00 L reaction container
This is for an on-line course and I really need help...I dont know how to do calculate and I dont have a teacher to help me so PLEASE help and thank you in advance
2CO2(g) <--> 2CO(g) + O2(g)
Calculate the equilibrium concentrations of all gases if 0.600 mol of CO2(g) is initially placed in a 3.00 L reaction container
This is for an on-line course and I really need help...I dont know how to do calculate and I dont have a teacher to help me so PLEASE help and thank you in advance
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Ke = {reactants /{products} = {CO2}^2 {O2} / {CO2}^2 = 2.5 x10^-7
(x)^2 (x) / (0.2)^2 = "
(x)^3 = 0.04 x 2.5x10^-7
x = 2.15x10^-3 moles per litre
CO = 4.6M O2 = 2.15M CO2 = 0.04M
(x)^2 (x) / (0.2)^2 = "
(x)^3 = 0.04 x 2.5x10^-7
x = 2.15x10^-3 moles per litre
CO = 4.6M O2 = 2.15M CO2 = 0.04M