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28 Sep 2019
consider the following equilibrium at 686 deg c
CO2(g) + H2(g) <------> co(g) + H20(g)
the equilibrium concentrations of the reactant species are
[co] = 0.050M, [h2]= 0.045M [co2]=0.096M [h2o]=0.040M
a) calculate kc for the reaction at 686 deg c
b) if the equilibrium concentration of co2 were raised to 0.50M andkc value was determined to be 0.52, what would be the equilibriumconcentrations of all the gases?
consider the following equilibrium at 686 deg c
CO2(g) + H2(g) <------> co(g) + H20(g)
the equilibrium concentrations of the reactant species are
[co] = 0.050M, [h2]= 0.045M [co2]=0.096M [h2o]=0.040M
a) calculate kc for the reaction at 686 deg c
b) if the equilibrium concentration of co2 were raised to 0.50M andkc value was determined to be 0.52, what would be the equilibriumconcentrations of all the gases?
CO2(g) + H2(g) <------> co(g) + H20(g)
the equilibrium concentrations of the reactant species are
[co] = 0.050M, [h2]= 0.045M [co2]=0.096M [h2o]=0.040M
a) calculate kc for the reaction at 686 deg c
b) if the equilibrium concentration of co2 were raised to 0.50M andkc value was determined to be 0.52, what would be the equilibriumconcentrations of all the gases?
Jarrod RobelLv2
29 Sep 2019
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