HARD
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At 700 K, the equilibrium constant Kp for the reaction 2SO3(g)2SO2(g)+O2(g) is 1.80×10-3 kPa, (R=8.314 Jk-1 mol1). The numerical value in moles per litre of Kc for this reaction at the same temperature will be

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Important Questions on Equilibrium

EASY
Consider the following reversible chemical reactions:

A2g+B2gk12ABg .....(1)  

6ABgk23A2g+3B2g .....(2)

The relation between K1 and K2 is:
HARD
4.0 moles of argon and 5.0 moles of PCl5 are introduced into an evacuated flask of 100 litre capacity at 610 K. The system is allowed to equilibrate. At equilibrium, the total pressure of mixture was found to be 6.0 atm. The Kp for the reaction is [Given : R=0.082 L atm K-1 mol-1 ]
HARD
What are the values of KpKc for the following reactions at 300K respectively?

(At 300K,RT=24.62dm3atmmol-1 )

N2 g+O2 g2NO g;  KpKc=x1

N2O4 g2NO2 g;  KpKc=x2

N2 g+3H2 g2NH3 g; KpKc=x3
EASY
If the value of an equilibrium constant for a particular reaction is 1.6×1012, then at equilibrium the system will contain:
MEDIUM
At 60°C, dinitrogen tetroxide is fifty percent dissociated. Find its standard free energy change at this temperature and one atmosphere. [ Given: log1.33=0.1239 ]
EASY
If the equilibrium constant for N2g+O2(g)2NO(g) is K, the equilibrium constant for 12N2g+12O2(g)NO(g) will be:
MEDIUM
In a chemical reaction, A+2BK2C+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 chemical reaction is:
MEDIUM
Consider the equilibria i and ii with equilibrium constants K1 and K2 , respectively

SO2g+12O2gSO3g .... (i)

2SO3g2SO2g+O2g .... (ii)

K1 and K2 are related as
HARD
For the reaction AgBg+Cg, A is 33% dissociated at a total pressure P. The correct relation between P and Kp is
MEDIUM

For the reaction

H2g+CO2gCOg+H2Og, if the initial concentration of H2=CO2 = 1M and x moles/L of H2 is consumed at equilibrium, the correct expression of KP is.

HARD
Consider the equilibrium X2+Y2P . Find the stoichiometric coefficient of the P using the data given in the following table:
 
X2/mol L-1 Y2/mol L-1 P/mol L-1
1.14×10-2 0.12×10-2 2.52×10-2
0.92×10-2 0.22×10-2 3.08×10-2
EASY
For NH4HSsNH3g+H2 Sg  the
observed pressure for the reaction mixture in equilibrium is 1.12 atm at 106°C. What is the value of Kp for the reaction?
MEDIUM
For the reaction, AnB the concentration of A decreases from 0.06 to 0.03 mol L-1 and that of B rises from 0 to 0.06 mol L-1 at equilibrium. The values of n and the equilibrium constant for the reaction, respectively, are
HARD
5.1 g NH4SH is introduced in 3.0 L evacuated flask at 327oC . 30% of the solid NH4SH is  decomposed to NH3 and H2S as gases. The KP of the reaction at 327oC is

R=0.082 L atm mol-1K-1, Molar mass of S=32 g mol-1, Molar mass of N=14 g mol-1
MEDIUM
The equilibrium constants of the following are:

N2+3H22 NH3K1N2+O22 NOK2H2+12O2H2O K3

The equilibrium constant (K) of the reaction:

2NH3+52O2K2NO+3H2O, will be:
EASY
For the reaction SO 2 g + 1 2 O 2 g SO 3 g , if K P = K C RT x where the symbols have usual meaning then the value of x is:
(assuming ideality)
MEDIUM
The equilibrium constant Kc of two reactions H2+I22HI and N2+3H22NH3 are 50 and 1000, respectively. The equilibrium constant of the reaction N2+6HI2NH3+3I2 is closest to:
HARD

For a reaction at equilibrium

 AgBg+12Cg

 the relation between dissociation constant K, degree of dissociation α and equilibrium pressure p is given by :

MEDIUM
A sample of HI(g) is placed in a flask at a pressure of 0.2 atm. At equilibrium, partial pressure of HI(g) is 0.04 atm. What is Kp for the given equilibrium ? 2HI(g)H2( g)+I2(g)
HARD
A 20 litre container at 400 K contains CO2g at pressure 0.4 atm and an excess of SrO (neglect the volume of solid SrO ). The volume of the container is now decreased by moving the movable piston fitted in the container. The maximum volume of the container, when the pressure of CO2 attains its maximum value, will be:

Given that:SrCO3sSrOs+CO2g, Kp=1.6 atm