JEE Questions for Chemistry Equilibrium Quiz 9 - MCQExams.com

The relation between Kp and Kc for the reaction
Chemistry-Equilibrium-3688.png
  • Kp = Kc
  • Kp = Kc (RT)
  • Kp = Kc / (RT)
  • Kp = Kc / (RT)2
The ratio of Kp /Kc for the reaction:
Chemistry-Equilibrium-3689.png
  • 1
  • RT
  • (RT)1/2
  • (RT)–1/2
For a homogeneous chemical reaction, Kp = kc when
  • Δn = 0
  • Δn = 1
  • Δn = 2
  • Δn = ∞

Chemistry-Equilibrium-3691.png
  • K1 / K2 K3
  • K1 K2 K3
  • K2 K1 K3
  • K1 + K2 + K3
If K1 and K2 are the equilibrium constants of the equilibria (i) and (ii) respectively, what is the relationship between the two constants?
Chemistry-Equilibrium-3692.png

  • Chemistry-Equilibrium-3693.png
  • 2)
    Chemistry-Equilibrium-3694.png

  • Chemistry-Equilibrium-3695.png

  • Chemistry-Equilibrium-3696.png

Chemistry-Equilibrium-3698.png
  • Exothermic
  • Endothermic
  • Exergonic
  • Unpredictable

Chemistry-Equilibrium-3699.png

  • Chemistry-Equilibrium-3700.png
  • 2)
    Chemistry-Equilibrium-3701.png

  • Chemistry-Equilibrium-3702.png

  • Chemistry-Equilibrium-3703.png
Starting with one mole of O2 and two moles of SO2, the equilibrium for the formation of SO3 was established at a certain temperature. If V is the volume of the vessel and 2x is the number of moles of SO3 present, the equilibrium constant will be

  • Chemistry-Equilibrium-3704.png
  • 2)
    Chemistry-Equilibrium-3705.png

  • Chemistry-Equilibrium-3706.png

  • Chemistry-Equilibrium-3707.png

Chemistry-Equilibrium-3709.png

  • Chemistry-Equilibrium-3710.png
  • 2)
    Chemistry-Equilibrium-3711.png

  • Chemistry-Equilibrium-3712.png

  • Chemistry-Equilibrium-3713.png

Chemistry-Equilibrium-3715.png

  • Chemistry-Equilibrium-3716.png
  • 2)
    Chemistry-Equilibrium-3717.png

  • Chemistry-Equilibrium-3718.png

  • Chemistry-Equilibrium-3719.png

Chemistry-Equilibrium-3721.png

  • Chemistry-Equilibrium-3722.png
  • 2)
    Chemistry-Equilibrium-3723.png

  • Chemistry-Equilibrium-3724.png

  • Chemistry-Equilibrium-3725.png

Chemistry-Equilibrium-3726.png
  • [A] = [B]
  • [A] < [B]
  • [B] = [C]
  • [A] > [B]
In which of the following reactions the equilibrium constant will have no units?

  • Chemistry-Equilibrium-3727.png
  • 2)
    Chemistry-Equilibrium-3728.png

  • Chemistry-Equilibrium-3729.png
  • In all the above relations.

Chemistry-Equilibrium-3730.png
  • atm
  • (atm)3
  • (atm)–2
  • (atm)2
Le - Chatelier principle is not applicable when
  • H2 (g) & I2 (g) react to form 2 HI(g)
  • N2 (g) + 3H2 (g) react to form 2NH3(g)
  • PCl5(g) decomposes to form PCl3(g) + Cl2 (g)
  • Fe (s) + S (s) react to form FeS (s)

Chemistry-Equilibrium-3732.png
  • it decreases
  • it increases
  • it remains unaffected
  • it cannot be predicted without the value of Kp
In which of the following reaction, pressure has no effect on equilibrium?

  • Chemistry-Equilibrium-3733.png
  • 2)
    Chemistry-Equilibrium-3734.png

  • Chemistry-Equilibrium-3735.png

  • Chemistry-Equilibrium-3736.png
In which of the following reactions, the equilibrium is shifted to the right by increasing the temperature ?

  • Chemistry-Equilibrium-3737.png
  • 2)
    Chemistry-Equilibrium-3738.png

  • Chemistry-Equilibrium-3739.png

  • Chemistry-Equilibrium-3740.png
Increased temperature favours the forward reaction

  • Chemistry-Equilibrium-3741.png
  • 2)
    Chemistry-Equilibrium-3742.png

  • Chemistry-Equilibrium-3743.png

  • Chemistry-Equilibrium-3744.png
Ostwald’s process for manufacture of nitric acid involves the reaction
Chemistry-Equilibrium-3745.png
  • Increase of pressure
  • Decrease of temperature
  • Increase of Volume
  • Addition of catalyst
Calcium carbonate, CaCo3 ,dissociates in the following manner
Chemistry-Equilibrium-3746.png
  • temperature is increased
  • pressure is increased
  • temperature is decreased
  • pressure is decreased

Chemistry-Equilibrium-3747.png
  • using a catalyst
  • removing some of B2
  • increasing the temperature
  • increasing the pressure

Chemistry-Equilibrium-3748.png
  • temperature is increased
  • pressure is increased
  • temperature is decreased
  • pressure is decreased

Chemistry-Equilibrium-3749.png
  • pH will decrease
  • hydrogen ion concentration will diminish
  • H2CO3 concentration will be altered
  • the forward reaction will be promoted

Chemistry-Equilibrium-3750.png
  • Total pressure
  • Catalyst
  • The amounts of H2 and I2 present
  • Temperature

Chemistry-Equilibrium-3751.png

  • Chemistry-Equilibrium-3752.png
  • 2)
    Chemistry-Equilibrium-3753.png

  • Chemistry-Equilibrium-3754.png

  • Chemistry-Equilibrium-3755.png
A liquid is in equilibrium with its vapour at its boiling point. On the average, the molecules in the two phases have equal
  • Intermolecules forces
  • Potential energy
  • Both kinetic energy and potential energy
  • Kinetic energy

Chemistry-Equilibrium-3756.png

  • Chemistry-Equilibrium-3757.png
  • 2)
    Chemistry-Equilibrium-3758.png

  • Chemistry-Equilibrium-3759.png

  • Chemistry-Equilibrium-3760.png

Chemistry-Equilibrium-3761.png
  • HI is exothermic compound
  • HI is very stable at room temperature
  • HI is relatively less stable than H2 and I2
  • HI is resonance stabilised
k1 and k2 are the velocity constants of forward and backward reactions. The equilibrium constant K of the reaction is:

  • Chemistry-Equilibrium-3762.png
  • 2)
    Chemistry-Equilibrium-3763.png

  • Chemistry-Equilibrium-3764.png

  • Chemistry-Equilibrium-3765.png
A and B are gaseous substances which react reversibly to give two gaseous substances C and D, accompanied by the liberation of heat. When the reaction reaches equilibrium, it is observed that Kp = Kc. The equilibrium cannot be disturbed by
  • Adding A
  • Adding D
  • Raising the temperature
  • Increasing the pressure
Select the reaction for which the equilibrium constant is written as
Chemistry-Equilibrium-3767.png

  • Chemistry-Equilibrium-3768.png
  • 2)
    Chemistry-Equilibrium-3769.png

  • Chemistry-Equilibrium-3770.png

  • Chemistry-Equilibrium-3771.png
In which of the following case, does the reaction go farthest to completion?
  • K = 102
  • K = 10
  • K = 10–2
  • K = 1
For which of the following systems at equilibrium at constant temperature, doubling the volume will cause a shift to the right?

  • Chemistry-Equilibrium-3779.png
  • 2)
    Chemistry-Equilibrium-3780.png

  • Chemistry-Equilibrium-3781.png

  • Chemistry-Equilibrium-3782.png

Chemistry-Equilibrium-3783.png

  • Chemistry-Equilibrium-3784.png
  • 2)
    Chemistry-Equilibrium-3785.png

  • Chemistry-Equilibrium-3786.png

  • Chemistry-Equilibrium-3787.png
Steam reacts with iron at high temperature to give hydrogen gas and Fe3O4(s) . The correct expression for the equilibrium constant is

  • Chemistry-Equilibrium-3789.png
  • 2)
    Chemistry-Equilibrium-3790.png

  • Chemistry-Equilibrium-3791.png

  • Chemistry-Equilibrium-3792.png
The standard state Gibb’s free energy change for the isomerisation reaction cis-2-pentene trans – 2- penten is –3.67 kJ mol–1 at 400 K. If more trans-2-pentene is added to the reaction vessel
  • More cis-2-pentene is formed
  • Equilibrium shifts in the forward direction
  • Equilibrium remains unaltered
  • More trans-2-pentene is produced
In which of the following reaction Kp > Kc

  • Chemistry-Equilibrium-3794.png
  • 2)
    Chemistry-Equilibrium-3795.png

  • Chemistry-Equilibrium-3796.png

  • Chemistry-Equilibrium-3797.png

Chemistry-Equilibrium-3799.png

  • Chemistry-Equilibrium-3800.png
  • 2)
    Chemistry-Equilibrium-3801.png

  • Chemistry-Equilibrium-3802.png

  • Chemistry-Equilibrium-3803.png

Chemistry-Equilibrium-3805.png
  • temperature and pressure
  • pressure only
  • temperature only
  • temperature, pressure and catalyst

Chemistry-Equilibrium-3806.png
  • in atm–2
  • in atm–3
  • in atm–1
  • dimensionless
When two reactants, A and B are mixed to give products C and D, the reaction quotient, Q, at the initial stages of the reaction
  • is zero
  • decreases with time
  • is independent of time
  • increases with time

Chemistry-Equilibrium-3809.png
  • increases
  • decreases
  • remains same
  • cannot be predicted
In the case of gaseous homogeneous reaction, the active mass of the reactant is obtained by the expression

  • Chemistry-Equilibrium-3810.png
  • 2)
    Chemistry-Equilibrium-3811.png

  • Chemistry-Equilibrium-3812.png

  • Chemistry-Equilibrium-3813.png

Chemistry-Equilibrium-3815.png

  • Chemistry-Equilibrium-3816.png
  • 2)
    Chemistry-Equilibrium-3817.png

  • Chemistry-Equilibrium-3818.png

  • Chemistry-Equilibrium-3819.png

Chemistry-Equilibrium-3821.png

  • Chemistry-Equilibrium-3822.png
  • 2)
    Chemistry-Equilibrium-3823.png

  • Chemistry-Equilibrium-3824.png

  • Chemistry-Equilibrium-3825.png
The decompsotion of N2O4 to NO2 is carried out at 280º in chloroform. When equilibrium is reached 0.2 mol of N2O4 and 2 × 10–3 mol of NO2 are present in 2 litre solution. The equilibrium constant for the reaction
Chemistry-Equilibrium-3826.png
  • 1 × 10–3
  • 2 × 10–3
  • 1 × 10–5
  • 2 × 10–5
1.1 mol of A is mixed with 2.2 mol of B and the mixture is kept in a one litre flask till the equilibrium,
Chemistry-Equilibrium-3828.png
  • 0.002
  • 0.004
  • 0.001
  • 0.003
A 1 M solution of glucose reaches dissociation equilibrium according to the equation given below:
Chemistry-Equilibrium-3830.png
  • 1.6 ×10–8 M
  • 3.2 ×10–6 M
  • 3.2 ×10–4 M
  • 1.6 ×10–4 M
1 mol of A and 0.5 mol of B were enclosed in a three litre vessel. The following equilibrium was established under suitable conditions
Chemistry-Equilibrium-3832.png
  • 11.1
  • 1.11
  • 0.01
  • 2.50
0:0:1


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