3. Calculating pressure from Ko and equilibrium amounts (a) In the following reaction:
2NO2 (a)_] 2NO (g) + O2 (g)
at a temperature of 700K, the amount of each gas present at equilibrium is 0.96 mol of
NO2, 0.04 mol of NO and 0.02 mol of O2. If Ke = 6.8 x 10-6 atm what must the total
pressure have been to obtain this particular equilibrium mixture?
(b) Ke = 3.72 atm at 1000K for the system:
C (s) + H2O (g) 0 Có (g) + H2 (g)
What pressure must be applied to obtain a mixture containing 2.0 mol of CO,
1.0 mol of H2 and 4.0 mol of H2O?

adding or remove a gaseous reactant or product changes the concentrations. if the concentration of reactant or product is increased, the system will shift away from the side in which concentration was increased (i.e. if the concentration of reactants is increased, the system will shift toward the products. if more products are added, the system will shift to form more reactants). conversely, if the concentration of reactant or product is decreased, the system will shift toward the side in which concentration was decreased (i.e. if reactants are removed, the system will shift to form more reactants. if the concentration of products is decreased, the equilibrium will shift toward the products).

explanation:

you did not give any options thus this is the best answer i can give to you with this little information you have given

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може ли да зареждате повече информация, моля