Equilibrium Tes...

The concentration of $$\left[ {{H^ + }} \right]$$ and concentration of $$\left[ {{OH^ + }} \right]$$ of a $$0.1\,M$$ aqueous solution of $$2\% $$  ionised weak acid is [ionic product of water $$ = 1 \times {10^{ - 14}}$$]

The reaction $${ 2HI }_{ \left( g \right)  }\rightleftharpoons { H }_{ 2\left( g \right)  }+{ I }_{ 2\left( g \right)  }$$ is initiated within a flask with 0.2 atm pressure of HI. If the partial pressure of $${ HI }_{ \left( g \right)  }$$ at equilibrium is 0.04 atm the equilibrium constant of the reaction is

Addition of sodium acetate solution to acetic acid causes the following change-

Predict the direction in which the following equilibrium will shift backward.

Which of the following pair will show common ion effect?

In which manner will increases of pressure affect the following equation ? 
$$C(s)+{ H }_{ 2 }O(g)\rightleftharpoons CO(g)+{ H }_{ 2 }(g)$$

Which changes increase the rate of reaction of an exothermic reaction?
1.Temperature increase
2.Temperature decrease

For a reaction: A$$\rightleftharpoons$$B; $$\Delta H^o < 0$$ and $$\Delta S^o > 0$$. Which of the following plots describes accurately the variation of logarithmic and equilibrium constant with temperature?

Solubility of $$MX_{ 2 }$$ type electrolytes is $$0.5\times 10^{ -4 } mol/L$$, Then find out $${ K }_{ sp }$$ of electrolytes.

In a $$5.76$$ L vessel, $$0.5$$ moles of $$ H_2 $$ gas and $$0.5$$ moles of $$ I_2 $$ vapours are allowed to react to from HI(g) at $$ 447^0 C $$, then total pressure of gases at equilibrium would be ( R =0.08 L-atm /K-mol )