Chemistry Chapter 7 Mock Test

15 moles of H₂ and 5.2 moles of l₂ are mixed and allowed to attain equilibrium at 500°c The concentration of HI is found to be 10 moles at equilibrium. Find the equilibrium constant for the formation of HI.

Statement 1: Unit of \(K_{c} =L^{2} mol^{-2}\) for the reaction \(N_{2}(g)+3H_{2}(g) \leftrightharpoons 2NH_{3}(g)\).

Statement 2: Equilibrium constant \(K_{c} = \frac{[NH_{3}^{2}]}{[N_{2}][H_{2}]^{3}}\) for the reaction \(N_{2}(g) + 3H_{2}(g) \leftrightharpoons 2NH_{3}(g).\)

The value of K_p will be equal to K_c in which of the following equation?

Find the equilibrium constant for the following gaseous reaction \(H_{2}+I_{2} \leftrightharpoons 2HI.\)

2 moles of PCl₅ were heated in a closed vessel of 2 litre capacity. At equilibrium, 40% of PCl₅ is dissociated into PCl₃ and Cl₂. What is the value of equilibrium constant?

Statement 1 : Colour of the mixture turns to pink from deep blue for a reaction, \(Co(H_{2}O)_{6(aq)}^{2+}+4Cl_{(aq)}^{-} \leftrightharpoons CoCl_{4(aq)}^{2-}+6H_{2}O_{(l)}\)after cooling a freezing mixture.

Statement 2 : Reaction is endothermic so on cooling, the reaction moves to backward direction.

What is the correct explanation of the effect of catalyst on the velocity in a reversible reaction?

What does the K becomes if concentration of reactants is increased by ‘x’?

Equilibrium is attained by the reaction when the free energy change accompanying it is

HI was heated in a closed tube at 440°c till equilibrium is obtained. At this temperature 22% of HI was dissociated. What will be the equilibrium constant for this dissociation?

Reactant ‘A’ decomposes 10% in 1 hour, 20% in 2 hour and 30% in 3 hour in a reaction. What is the unit of rate constant of this reaction?

For which of the following reactions K_p is greater than K_c?

K_p is less than K_c in which of the following equilibria?

56 g of nitrogen and 8 g hydrogen gas are heated in a closed vessel. At equilibrium 34 g of ammonia are present. What are the equilibrium no. of moles of nitrogen, hydrogen and ammonia respectively?

In which of the following reaction, yield of product will increase with increase in pressure?

If for \(H_{2(g)} + \frac{1}{2}S_{2(s)} \leftrightharpoons H_{2}S_{(g)} and H_{2(g)} + Br_{2(g)} \leftrightharpoons 2HBr_{(g)}.\)The reaction\(Br_{2(g)} + H_{2}S_{(g)} \leftrightharpoons 2HBr_{(g)}+ \frac{1}{2}S_{2(s)}\) would have equilibrium constant ________ where \(K_{1} and K_{2}\) are the equilibrium constants respectively.

For reaction \(PCl_{5}(g) \leftrightharpoons PCl_{3}(g) + Cl_{2}(g),\)

5 moles of SO₂ and 5 moles of O₂ are allowed to react to form SO₃ in a closed vessel. At the equilibrium stage 60% of SO₂ is used up. Find the total number of moles of SO₂, O₂ and SO₃ in the vessel now.

Statement 1: Catalyst affects the final state of the Equlibrium.

Statement 2: It enables the system to attain a new equilibrium state by complexing with the reagents.

In Haber process 30 litres of dihydrogen and 30 litres of dinitrogen were taken for reaction which yielded only 50% of the expected product. The composition of gaseous mixture under the aforesaid condition in the end will be:

The information that can be obtained on the basis of Le-chatelier’s principle is:

Increasing the temperature of an equilibrium system

One mole of \(SO_{3}\) was placed in a litre reaction vessel at a certain temperature. The following equilibrium was established \(2SO_{3} \leftrightharpoons 2SO_{2}+O_{2}\). At equilibrium 0.6 moles of \(SO_{2}\) were formed. What will be the equilibrium constant of the reaction?

What is the equilibrium constant K for the system \( 2A(g) + B(g) \leftrightharpoons 3C(g)?\)

Statement 1: Addition of a small amount of sodium acetate to a dilute solution of acetic acid does not affect the pH value.

Statement 2: Buffer solutions have a definite pH value.

     Statement 1: The pH of 10 M HCI aqueous solution is less than 1.

     Statement 2: The pH is -ve logarithm of H⁺ concentration.

Statement 1 : For the reverse reaction, equilibrium constant is the inverse of the equilibrium constant for the reaction in the forward direction.

Statement 2 : Equilibrium constant depends upon the way in which the reaction is written.

The equilibrium constant changes with _____ for the reaction\(H_2(g)+ l_2(g) \leftrightharpoons 2HI(g) \)

For the reaction \(C(s) + CO_{2}(g) \leftrightharpoons 2CO(g)\), the partial pressure of \(CO_{2}\) and CO are 2.0 and 4.0 atm respectively at equilibrium. What is the \(K_{p}\) for the reaction?

Under conditions of constant _________ \(\Delta G = 0\) for a system in equilibrium.

Statement 1 : Effect of temperature of K_c or K_p depends on enthalpy

Statement 2 : Increase in temperature shifts the equilibrium in exothermic direction while decrease in the temperature shifts the equilibrium position in endothermic direction.

The equilibrium reactions in which the equilibrium would shift to the right if total pressure is increased is:

The standard state Gibbs free energy change for the given isomerization reaction \(cis-2-pentene \leftrightharpoons trans -2 -pentene\) is -3.67 kJ/mol at 400 K. What happens if more trans-2-pentene is added to the reaction vessel?

Following gaseous reaction is undergoing in a vessel \(C_{2}H_{4}+H_{2} \leftrightharpoons C_{2}H_{6}: \Delta H=-32.7 Kcal\), Which of the following will increase the equilibrium concentration of \(C_{2}H_{6}\)?

in the chemical reaction \(N_{2}+3H_{2} \rightarrow 2NH_{3}\) the product increases by ________ .

Consider the reaction \(A_{2(g)} + B_{2(g)} \leftrightharpoons 2AB_{(g)} ; \Delta H= + ve\)

Gaseous reaction \(A + B \leftrightharpoons 2C + D ; + Q\) is most favoured at which of the following?

Sodium sulphate dissolves in water with evolution of heat. Consider a saturated solution of sodium sulphate. According to Le-Chatelier principle, if the temperature is raised, then

If the equilibrium concentration of A is doubled in the equilibrium \(AB \leftrightharpoons A + B\). the equilibrium concentration of B would become:

The equilibrium constant of the reaction \(H_{2}(g)+I_{2}(g) \leftrightharpoons 2HI\) is 64. What will be the value of the equilibrium constant if volume of the container is reduced to one fourth of its original volume?

All reactions that possess chemical disintegration is_____ .

The following equation gives the exothermic formation of \(ClF_{3}\).

\(Cl_{2(g)}+3F_{2(g)} \leftrightharpoons 2ClF_{3(g)} ; \Delta H= – 329 kj\)

Which of the following will increase the quantity of \(ClF_{3}\) in an equilibrium mixture of \(Cl_{2}, F_{2}\) and \(ClF_{3}?\)