Consider the reaction: NiO (s) + CO (g) <=> Ni (s) + CO2(g) Kc=4.0*10^3 (at 1500...

Consider the reaction: NiO (s) + CO (g) <=> Ni (s) + CO2(g) Kc=4.0*10^3 (at 1500 K) If a mixture of 1.00 mol nickel (II)oxide and 0.20 mol carbon monoxide in 2.00 L flask are allowed to come to equilibrium, what is the equilibrium concentration of carbon dioxide?

Expert Solution

NiO (s) + CO (g) <=> Ni (s) + CO2(g)

at t=0 I (1mol/2L) (0.2mol/2L) 0 0

= 0.5M = 0.1M 0 0

C -x +x

E (0.1-x) x

expression for Kc = [CO2(g)]/ [CO (g) ]

Given Kc = 4.0*10^3

therefore 4.0*10^3 = x/(0.1-x)

by simplifying 4.0*10^2 - 4.0*10^3 x = x

=> 4.0*10^2 = x (4001)

=> x= 0.0999 that is 0.010

hence equilibrium concentration of CO2 (g) is 0.010M

queen_honey_blossom answered 1 year ago

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Question

Consider the reaction: NiO (s) + CO (g) <=> Ni (s) + CO2(g) Kc=4.0*10^3 (at 1500...

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Expert Solution

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