Consider the following equilibrium system involving SO_2, Cl_2, and SO_2Cl_2 (su

Question

Consider the following equilibrium system involving SO_2, Cl_2, and SO_2Cl_2 (sulfuryl dichloride): SO_2(g) + Cl_2(g) SO_2Cl_2(g) Predict how the equilibrium position would change if (a) Cl_2 gas were added the system; SO_2Cl_2 were removed from system; SO_2 were removed from the system. The temperature remains constant. Heating solid sodium, in a closed vessel establishes the following equilibrium: 2NaHCO_3(s) Na_2CO_3(s) + H_2O(g) + CO_2(&) What would happen to the equilibrium position if some of the CO_2 were removed from the system some solid Na_2CO_3 were added to the system. some of the solid NaHCO_3 were removed from the system? The temperature remains constant. Consider the following equilibrium systems: A 2B delta H degree = 20.0 kJ/mol A + B C delta H degree = -5.4 KJ/mol A B delta H degree = 0.0 kJ/mol Predict the change in the equilibrium constant K_c that would occur in each ease if the temperature the reacting system were raised. What effect Hoes an increase in pressure have on each of the Blowing systems at equilibrium? The temperature is kept constant and, in each cash the reactants are in a cylinder fitted with a movable piston.

Explanation / Answer

a) some of CO2 added equilibrium shifts to the left side

b) solid Na2CO3 added there is no effect on equilibrium

c) solid NaHCO3 removed no effecct on equilibrium

explanation:

on addition of any reactant the equilibrium shifts to the right . on addition of product the equilibrium shifts to left.

there is no effect of solids on equilibrium

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