# Quiz | Chemical Equilibrium

Which of the following statements about the equilibrium constant is correct?

It changes with changes in the temperature

It changes by the addition of a catalyst

It always remains the same at different reaction conditions

It increases if the concentration of one of the reactants or products is increased

Which of the following statements is correct?

At the equilibrium, sum of [reactant] = sum of [product]

At the equilibrium the forward and reverse reactions still occur

A chemical equilibrium can be attained only starting from a mixture

Chemical equilibrium is a static equilibrium, [reactant] = constant and [product] = constant

What is the equilibrium constant expression K_{C} of the reaction: N_{2 }(g) + 3 H_{2 }(g) $\rightleftarrows $ 2 NH_{3 }(g)?

$\frac{\left[{\mathrm{N}}_{2}\right]\left[{\mathrm{H}}_{2}\right]}{\left[{\mathrm{NH}}_{3}\right]}$

$\frac{\left[{\mathrm{NH}}_{3}\right]}{\left[{\mathrm{N}}_{2}\right]\left[{\mathrm{H}}_{2}\right]}$

$\frac{\left[{\mathrm{N}}_{2}\right]{\left[{\mathrm{H}}_{2}\right]}^{3}}{{\left[{\mathrm{NH}}_{3}\right]}^{2}}$

$\frac{{\left[{\mathrm{NH}}_{3}\right]}^{2}}{\left[{\mathrm{N}}_{2}\right]{\left[{\mathrm{H}}_{2}\right]}^{3}}$

What is the equilibrium constant expression K_{C} of the reaction: 2 ICl (s) $\rightleftarrows $ I_{2 }(s) + Cl_{2 }(g)?

[Cl_{2}]

$\frac{\left[{\mathrm{I}}_{2}\right]}{{\left[\mathrm{ICl}\right]}^{2}}$

$\frac{\left[{\mathrm{Cl}}_{2}\right]\left[{\mathrm{I}}_{2}\right]}{2\left[\mathrm{ICl}\right]}$

$\frac{\left[{\mathrm{Cl}}_{2}\right]\left[{\mathrm{I}}_{2}\right]}{{\left[\mathrm{ICl}\right]}^{2}}$

How can we increase the total amount of produced Cl_{2} during the reaction: 2 ICl (s) $\rightleftarrows $ I_{2 }(s) + Cl_{2 }(g)?

By adding more ICl

By increasing the pressure

By removing the Cl_{2} as it is formed

By decreasing the volume of the container

What happens when the reaction quotient Q_{C} is less than the equilibrium constant K?

The reaction will move to the left

The reaction will move to the right

It depends on whether the reaction is endothermic or exothermic

It depends on the reaction conditions