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--> kc = [CO2]/[CO]
Adding of CO will shift reaction towards right.
Removal of CO will shift reaction towards left.
Adding of Ni will have no effect.
Increase in volume will shift reaction towards more no. of gaseous molecules. So here, both side gaseous moles are equal hence no effect.
Removal of CO2 will shift reaction towards right.
Addition of CO2 will shift reaction towards left.
Removal of NiO will have no effect.
Option 2 and 6 will shift reaction towards left.
--> reaction is--
2H2S(g) + SO2(g) --> 3S(s) + 2H2O(g)
Kc = [H2O]2/[H2S]2[SO2]
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Consider the following reaction at equilibrium: NiO(s)+CO(g) 2 Ni(s) + CO2(g). Select all of the following...
Consider the reaction: NiO(s)+CO(g)⇌Ni(s)+CO2(g) Kc=4000.0 at 1500 K When calculating the answer, do not round to the appropriate number of significant figures until the last calculation step. Part A If a mixture of solid nickel(II) oxide and 0.11000 M carbon monoxide is allowed to come to equilibrium at 1500 K, what will be the equilibrium concentration of CO2?
For which reaction will Kp = Kc? ONiCO3(s) = NiO(s) + CO2(g) O 2 HgO(s) = Hg(1) + O2(8) OS(s) + O2(8) =SO2(g) K2CO3(s) =K20(s) + CO2(g) O 2 H2O(1) = 2 H2(g) + O2(g) Show transcribed image text
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