Equilibrium Tes...

Which factor, when decreased will cause a reaction to proceed more quickly?

What happens when a chemical reaction system is stressed by an 'increase in the concentration of the reactants?

Equilibrium constant for the reaction,  $$NH_{4}OH + H^{+}\rightleftharpoons NH_{4}^{+} + H_{2}O$$ is $$1.8\times 10^{9}$$. Hence, equilibrium constant for $$NH_{3}(aq) + H_{2}O \rightleftharpoons NH_{4}^{+} + OH^{-}$$ is:

Given the reaction $$2A(g) + B(g) + heat \rightleftharpoons 3C(g) + D(g)$$, what could be done to the reaction to shift the equilibrium so that more $$D$$ is made?

Which of the following will form a buffer solution of 1L solution?

For a reaction if $$K_p > K_c$$, the forward reaction is favoured by:

Very strong acids, such as $$HNO_3$$ and $$HCl$$, appear to be equally strong in water. This "leveling effect" of water is because

Assertion: When a non-volatile solute is added to pure water, the vapor pressure of the water will decrease.
Reason: All solutes dissociate into positive and negative ions.

Assertion: Water makes a good buffer.
Reason: A good buffer will resist changes in $$\displaystyle pH$$.

A litre of solution is saturated with $$AgCl$$. To this solution if $$1.0\times { 10 }^{ -4 }$$ mole of solid $$NaCl$$ is added, what will be the $$\left[ { Ag }^{ + } \right] $$ assuming no volume change?