Consider the reaction :

NiO(s) + CO(g) (equlibrium equation arrows going both way) Ni(S)+ CO2(g)

Kc = 4.0 X 10^3 at 1500 K

If the mixture of solid nickle(II) oxide and 0.20 M carbonmonoxide is allowed to come to equilibrium at 1500 K, what will bethe equilibrium concentration of CO2?

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Jean KeelingLv2

13 Dec 2019

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Consider the reaction: NiO(s)+CO(g)âNi(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 0.18000 M carbon monoxide is allowed to come to equilibrium at 1500 K, what will be the equilibrium concentration of CO2?

Consider the following reaction:
{\rm{NiO}}\left( s \right)\; + \;{\rm{CO}}\left( g \right)\;\rightleftharpoons \;{\rm{Ni}}\left( s \right)\; + \;{\rm{CO}}_2\left( g \right)
K_{\rm{c}} = 4.0 \times 10^3 at 1500 \rm K

If a mixture of solid nickel(II) oxide and 0.20 M carbon monoxideis allowed to come to equilibrium at 1500 {\rm K}, what will be theequilibrium concentration of {\rm{CO}}_2?