Advertisements
Advertisements
Question
Consider the following reversible reaction at equilibrium,
\[\ce{A + B <=> C}\],
If the concentration of the reactants A and B are doubled, then the equilibrium constant will
Options
be doubled
become one fourth
be halved
remain the same
Solution
remain the same
APPEARS IN
RELATED QUESTIONS
Mention various applications of equilibrium constant.
If x is the fraction of PCl5 dissociated at equilibrium in the reaction
\[\ce{PCl5 <=> PCl3 + Cl2}\]
then starting with 0.5 mole of PCl5, the total number of moles of reactants and products at equilibrium is
In the reaction
\[\ce{Fe(OH)3(S) <=> Fe^{(3+)} (aq) + 3OH- (aq)}\]
if the concentration of OH– ions is decreased by 1/4 times, then the equilibrium concentration of Fe3+ will
Equimolar concentrations of H2 and I2 are heated to equilibrium in a 1 liter flask. What percentage of the initial concentration of H2 has reacted at equilibrium if the rate constant for both forward and reverse reactions are equal
If there is no change in concentration, why is the equilibrium state considered dynamic?
Explain how will you predict the direction of an equilibrium reaction.
For a reversible reaction, if the concentrations of the reactants are doubled, then the equilibrium constant value ______.
