Question

Calculate the equilibrium concentrations of all species. (Use Kc equilibrum equation). Please show work, thank you!

2CO2(g) 2C0(g) O2(g) 20. Ke 2.00 x 10 If 2.0 mol CO2 is initially placed into a 5.0 L vessel, calculate the equilibrium concentrations of all species. 2 ME

Answer 1

Given reaction is

2CO_2(g)$\rightleftharpoons$ 2CO_(g) + O_2(g)

Lets see the initial concentration of CO₂

[CO₂ ] = 2.0 mol / 5.0 L = 0.4 M

now lets see the ICE table for given reaction

...................................2CO_2(g)......$\rightleftharpoons$_........2CO_(g)......+.....O_2(g)

Initial.......................0.4 M........................0....................0

Change ..................-2x............................+2x..................+x

At Equilibrium........0.4-2x.........................2x....................x

Now equilibrium constant for reaction is

Kc = [CO]²[O₂] /[CO₂]²  

2.00 $\times$ 10^-4 = (2x)²$\times$ (x) / (0.4-2x)² = 4x³ /  (0.4-2x)²

as x <<< 0.4 we can neglect 0.4-2x = 0.4 then

2.00 $\times$ 10^-4 = 4x³ /  (0.4)² = 4x³ / 0.16

x³ = 0.16 $\times$ 2.00 $\times$ 10^-4 / 4 = 0.08 $\times$ 10^-4

Lets take the cube root on both the sides we get

x = 0.02 M

then at equilibrium

[CO] = 2x = 2 $\times$ 0.02 = 0.04 M

[O₂]= x = 0.02 M

[CO₂] = 0.4 -2x = 0.4 - 2 $\times$ 0.02 = 0.36 M

Answer 2

2.0+2xCO2 2.0+x CO 2.0-xO2 That was equilibrium now let us solve for x Use the equilibrium equation K concentration /Q concentration

Answer 3

2.0+2xCO2 2.0+x CO 2.0-xO2 That was equilibrium now let us solve for x Use the equilibrium equation K concentration /Q concentration