Multiple Choice QuestionsIf the value of an equilibrium constant ofr particular reaction is 1.6 x1012 then at equilibrium the system will contains
all reactants
mostly reactants
mostly products
mostly products
The Ksp of Ag2CrO4, AgCl, AgBr and AgI are respectively, 1.1 x 10-12, 1.8 x 10-11, 8.3 x 10-17. Which one of the following salts will precipitate last if AgNO3 solution is added to the solution containing equal moles of NaCl, NaBr, NaI and Na2CrO4?
AgI
AgCl
AgBr
AgBr
For the reversible reaction,
the equilibrium shifts in the forward direction
by increasing the concentration of NH3 (g)
by decreasing the pressure
by decreasing the concentrations of N2 (g) and H2(g)
by decreasing the concentrations of N2 (g) and H2(g)
D.
by decreasing the concentrations of N2 (g) and H2(g)
Any change in the concentration, pressure and temperature of the reaction results in a change in the direction of equilibrium.This change in the direction of equilibrium in governed by Le-Chatelier's principle. According to Le-Chatelier's principle, the equilibrium shifts in the opposite direction to undo the change.
Increasing pressure and decreasing temperature
On increasing pressure, equilibrium shifts in the forward direction where the number of moles decreases while on decreasing temperature. it will move in a forward direction where temperature increases.
For a given exothermic reaction Kp and Kp' are the equilibrium constant at temperatures T1 and T2 respectively. Assuming that heat of reaction si constant in temperature range between T1 and T2 it is readily observed that
Kp> Kp'
Kp< Kp'
Kp = Kp'
Kp = Kp'
pH of a saturated solution of Ba(OH)2 is 12. The value of solubility product Ksp of Ba(OH)2 is
3.3 x 10-7
5.0 x 10-7
4.0 x 10-6
4.0 x 10-6
Equimolar solutions of the following substances were prepared separately, which one of these will record the highest pH value?
BaCl2
AlCl3
LiCl
LiCl
Buffer solutions have constant acidity and alkalinity because
these give unionised acid or base on reaction with added acid or alkali
acids and alkalies in these solutions are shielded from attack by other ions.
they have a large excess of H+ or OH- ions
they have a large excess of H+ or OH- ions
Give that the equilibrium constant for the reaction,
2SO2 (g) + O2 (g) ⇌ 2SO3 (g)
has a value of 278 at a particular temperature. What is the value of the equilibrium constant for the following reaction t the same temperature?
SO3 (g) ⇌ SO2 (g) +1/2 O2 (g)
1.8 x 10-3
3.6 x 10-3
6.0 x 10-2
6.0 x 10-2
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