the following equilibrium exists between molecular and atomic oxygen O2--2O Kp=1.2*10^-10 If 2.00 moles of O2...

the following equilibrium exists between molecular and atomic oxygen

O2--2O

Kp=1.2*10^-10

If 2.00 moles of O2 is placed in a 10L flask and heated to 1800K, how many O atom would be present in the flask at equilibrium

Expert Solution

O2(g)----->2O(g)

KP = Kc(RT)^n

n = 2-1 = 1

T = 1800K

R = 0.0821L-atm/mole-K

KP = Kc(RT)^n

1.2*10^-10 = Kc(0.0821*1800)^1

Kc = 1.2*10^-10/147.78 = 8.12*10^-13

O2(g)----->2O(g)

I 2 0

C -x 2x

E 2-x 2x

Kc = [O]^2/[O2]

8.12*10^-13 = (2x)^2/2-x

8.12*10^-13*(2-x) = 4x^2'

x = 6.37*10^-7

no of moles of O = 6.37*10^-7 moles

no of atoms = no of moles * 6.023*10^23 * atomicity

= 6.37*10^-7*6.023*10^23*2

= 7.67*10^17 atoms >>>>>answer

queen_honey_blossom answered 2 years ago

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