The volume of a closed reaction vessel in which the equilibrium $$2SO_2(g) + O_2(g) \rightleftharpoons 2SO_3(g)$$ sets is halved now:
$$2 SO_2(g) + O_2(g)\rightleftharpoons 2SO_3(g)$$ In this reaction three moles (or volumes`) of reactants are converted into two moles (or volumes) of products i.e. there is a decrease in volume and so if the volume of the reaction vessel is halved the equilibrium will be shifted to the right i.e. more product will be formed and the rate of forward reaction will increase i.e.double that of reverse reaction.
Liquid $$NH_3$$ ionises to a slight extent. At a certain temperature, its ionization constant $$K_{SIC{(NH_3)}} = 10^{-30}$$. The number of $$NH_4^+$$ ions present per $$100\space cm^3$$ of pure liquid is:
The rate constant of forward and backward reactions for certain hypothetical reaction are $$1.1\, \times\, 10^{-2} $$ and $$1.5\, \times\, 10^{-3}$$ respectively. The equilibrium constant of the reaction is:
The value of equilibrium constant for the reaction represented by the equation : $$AgCl (s)\rightleftharpoons Ag^+ (aq) + Cl^- (aq)$$ is ____.
The following data for the equilibrium composition of the reaction. $$2 Na (g) \rightleftharpoons Na_2 (g)$$ at $$1.013$$ $$MP_a$$ pressure and $$1482.53 K$$ have been obtained. mass % Na (monomer gas) = $$71.3$$ mass % $$Na_2$$ (dimer gas) = $$28.7$$ Calculate the equilibrium constant $$K_p$$ :
. Consider the following reversible chemical reactions: $$A_2(g)+Br_2(g) {\rightleftharpoons {2AB}}(g)....(1) {K_1}$$ $$6AB(g) {\rightleftharpoons {3A_2}}(g)+ 3B_2 ....(2) {K_2}$$ The relation between $$K_1$$ and $$K_2$$ is:
In a chemical reaction, $$A + 2B \overset {K}{\rightleftharpoons} 2C + D$$, the initial concentration of $$B$$ was $$1.5$$ times of the concentration of $$A$$, but the equilibrium concentrations of $$A$$ and $$B$$ were found to be equal. The equilibrium constant $$(K)$$ for the aforesaid chemical reaction is:
A solid $$XY$$ kept in an evacuated sealed container undergoes decomposition to form a mixture of gases $$X$$ and $$Y$$ at temperature $$T$$. The equilibrium pressure is $$10$$ bar in this vessel. $${K}_{p}$$ for this reaction is:
For the reaction, N2(g)+3H2(g)⇌2NH3(g), the unit of K is :
The reaction, 2A(g) + B(g) ⇌ 3C(g) + D(g) is begun with the concentrations of A and B both at an initial value of 1.00 M. When equilibrium is reached the concentration of D is measured and found to be 0.25 M. What is the value of the equilibrium constant for the given reaction?
At a certain temperature and total pressure of $$\displaystyle { 10 }^{ 5 }\ Pa$$, iodine vapour contains $$40\%$$ by volume of I atoms. $$\displaystyle { I }_{ 2 }\left( g \right) \rightleftharpoons 2I\left( g \right) $$ Calculate $$\displaystyle { K }_{ p }$$ for the equilibrium.