For a reversible reaction involving two reactants,if the concentration of the reactants is doubled,the equilibrium constant will:

If a system is at equilibrium,the rate of the forward reaction compared to the reverse reaction is:

Identify which of the following reactions represent homogeneous and heterogeneous equilibria:
$(a)$ $H_{2(g)} + I_{2(g)} \rightleftharpoons 2HI_{(g)}$
$(b)$ $Ca(OH)_{2(s)} \rightleftharpoons Ca^{2+}_{(aq)} + 2OH^{-}_{(aq)}$
$(c)$ $CaCO_{3(s)} \rightleftharpoons CaO_{(s)} + CO_{2(g)}$
$(d)$ $Ag_{2}O_{(s)} + 2H^{+}_{(aq)} \rightleftharpoons H_{2}O_{(l)} + 2Ag^{+}_{(aq)}$
$(e)$ $NH_{3(g)} + H_{2}O_{(l)} \rightleftharpoons N{H_{4}}^{+}_{(aq)} + OH^{-}_{(aq)}$
$(f)$ $CH_{3}COOC_{2}H_{5(l)} + H_{2}O_{(l)} \rightleftharpoons CH_{3}COOH_{(l)} + C_{2}H_{5}OH_{(l)}$

The equilibrium constant for the reaction $N_{2(g)} + O_{2(g)} \rightleftharpoons 2NO_{(g)}$ is $4 \times 10^{-4}$ at $2000 \ K$. In the presence of a catalyst,equilibrium is attained ten times faster. Therefore,the equilibrium constant in the presence of the catalyst at $2000 \ K$ is:

Explain chemical equilibrium by giving an example of a general reaction.

In the chemical reaction $A \rightleftharpoons B$,the system will be known to be in equilibrium when: