Le Chatelier's Principle for Del N Equals to 0

Q.

For an endothermic reaction where $\Delta H$ represents the enthalpy of the reaction in $kJmo{l}^{-1}$, the minimum value for the energy of activation will be.

1. Equal to

2. Less than

3. Zero

4. More than

Q.

Which equation represents an example of Friedel-Crafts reaction

1. 

2. 

3. 

4. 

Q. 100 3.2 moles of HI(g) were heated in a sealed bulb at 444degree Celsius till the equilibrium is reached. Its degree of dissociation is 20% calculate the no of moles of hydrogen, iodide, hydrogen iodide Present at the equilibrium point and determine the value of equilibrium constant for the reaction. Considering the volume of the container 1L

Q. What volume of ammonia gas at NTP will be required to passed into 30ml of H_2SO_{4 }to bring down the acid normality to 0.2N

Q.

For which of the following reactions does the equilibrium constant

depend on the units of concentration

1. NO(g) 0.5N₂(g) + 0.5O₂(g)

2. Zn(s) + Cu²⁺(aq) Cu(s) + Zn²⁺(aq)

3. C₂H₅OH(l) + CH₃COOH(l) CH₃COOC₂H₅(l) + H₂O(l)

4. COCl₂(g) CO(g) + Cl₂(g)

Q. 9 Equilibrium concentrations of HI, I2 and H2 is 0.7, 0.1 and 0.1M respectively. The equilibrium constant for the reaction

Q. 36.At a certain temperature and 2 ATM pressure equilibrium constant KP is 25 for the reaction of SO2(g) +No2(g)---------- SO3(g) + NO(g).initially we take 2 moles of each of the four gases and 2 moles of inert gas what would be the equilibrium partial pressure of an NO2

Q. Which among the following is least soluble?

1. LiF

2. RbF

3. NaF

4. KF

Q.

The reaction A + B $\rightleftharpoons$​ C + D + heat has reached equilibrium. The reaction may

be made to proceed forward by

1. Adding more C

2. Adding more D

3. Decreasing the temperature

4. Increasing the temperature

Q.

For the reaction $N_2\left(g\right)+3H_2\left(g\right)\rightleftharpoons 2N{H}_3\left(g\right),\Delta H=-ve$. The formation of $N{H}_3\left(g\right)$ is favored a

1. Low pressure and low temperature

2. High pressure and high temperature

3. High pressure and low temperature

4. Low pressure and high temperature

Q. Vapour density=Density of gas at STP/Density of hydrogen gas at STP. Here what is STP??

Q.

The equilibrium constant for the given reaction $H_2+I_2\rightleftharpoons 2HI$ is correctly

given by expression

1. K = ([H₂] [I₂]) / [HI]

2. K = ([H₂] [I₂]) / [2HI]

3. K = ([H₂] [I₂]) / [HI]²

4. K = [HI]²/ ([H₂] [I₂])

Q.

The equilibrium, $S{O}_{2}C{l}_2\left(g\right)\rightleftharpoons S{O}_2\left(g\right)+C{l}_2\left(g\right)$ is attained at ${25}^{\circ }C$ in a closed container and an inert gas, helium, is introduced. Which of the following statements are correct?

1. More chlorine is formed

2. Concentration of is reduced

3. More is formed

4. Concentrations of and are not changed

Q. 6. At 817^° C Ko for the reaction b/w CO2 and excess of hot graphite is 10 atm. a) What are the equilibrium concentration of the gases at 817^° C and 5 atm total pressure? b) At what total pressure does the gas contains 5% CO2 by volume?

Q.

Q.

Pure ammonia is placed in a vessel at temperature where its dissociation constant ( ) is appreciable. At equilibrium

1. α does not change with pressure

2. K_P does not change significantly with pressure

3. Concentration of NH₃ does not change with pressure

4. Concentration of H₂ is less than that of N₂

Q. at temperature T K, Pcl5 is 50% dissociated at an equilibrium pressure of 4atm.at what pressure it would dissociate to the extent of 80% at the same temperature?

Q.

The equilibrium constant for the reaction :

$A\left(g\right)+B\left(g\right)\rightleftharpoons C\left(g\right)+D\left(g\right)$ is 1 \times ${10}^{-2}$ at 298K and it is 2 at 373K. The chemical process resulting the formation of C and D is

1. Unpredicatable

2. Exothermic

3. Endothermic

4. There is no relation between K and DH

Q.

What is the $pH$ of $0.5M$ aqueous solution of $NaCN$? Given $p{K}_b$ of $C{N}^{-}$ = $4.70$

1. 5.6

2. 3.4

3. 8.8

4. 11.5

Q. 52.2A+B=C+2D, 4 moles of A are mixed with 2 moles of B and the mixture is kept in one litre flask till the equilibrium is reached. At equilibrium 2 moles of D are formed. Calculate the value of kc

Q.

When two reactants, A and B are mixed to give products C and D such that
A + B $\leftrightharpoons$ C + D

the reaction quotient, Q = $\frac{\left[C\right]\left[D\right]}{\left[A\right]\left[B\right]}$ at the final stages of the reaction

1. is zero

2. increases with time

3. decreases with time

4. is independent of time

Q.

For the reaction $CO\left(g\right)+H_{2}O\left(g\right)\rightleftharpoons C{O}_2\left(g\right)+H_2\left(g\right)$ at a given temperature, the equilibrium amount of $C{O}_2\left(g\right)$ can be increased by

1. Increasing the amount of CO (g)

2. Decreasing the volume of the container

3. Adding an inert gas

4. Adding a suitable catalyst

Q. When 80 ml of ozonised oxygen was heated until no further change was observed and then cooled to have the same initial temperature and pressure, the volume measured was 95 ml. What would be the voume, if 40 ml of the mixture of O2 and O3 was exposed to oil of turpentine?

Q.

For the gas phase reaction $C_2{H}_4+H_2\rightleftharpoons C_2{H}_6,$ DH = -32.7kcal carried out in a vessel, the equilibrium concentration of $C_2{H}_4$ can be increased by -

1. increasing the temperature

2. Decreasing temperature

3. Increasing pressure

4. Increasing concentration of

Q.

\(N_2 ~+ ~O_2 ~\rightleftharpoons~ 2NO ~+~ (-Qcals)\)

In the above reaction which is the essential condition for the higher production of $NO$

1. High pressure

2. High temperature

3. Low temperature

4. Low pressure

Q.

For the reaction $2N{H}_3\left(g\right)\rightleftharpoons N_2\left(g\right)+3H_2\left(g\right),\Delta H=93.6kJmo{l}^{-1}$. Which of the following facts does not hold well?

1. The pressure changes at constant temperature do not affect the equilibrium constant

2. The volume changes at constant temperature do not affect the equilibrium constant

3. The dissociation of is less favored at high temperature

4. The dissociation of is more favored at high temperature

Q. For the gas phase reaction,
$C_2{H}_4\left(g\right)+H_2\left(g\right)\rightleftharpoons C_2{H}_6\left(g\right);△H^o=-136.8kJmo{l}^{-1}$
carried out in a vessel, the equilibrium concentration of $C_2{H}_4$ can be increased by:

1. Increasing the temperature
2. Decreasing the pressure
3. Removing some $H_2$
4. Adding some $C_2{H}_6$

Q. Complete the following reactions:

Q.

The following equilibria are given: $N_2$ +3$H_2$ $\leftrightharpoons$ $2N{H}_3$ $K_1$ ; $N_2$ + $O_2$ $\leftrightharpoons$ 2NO $K_2$ ;
$H_2$ + $\frac{1}{2}$ $O_2$ $\leftrightharpoons$ $H_{2}O{K}_3$ ;

The Equilibrium constant for the reaction $2N{H}_3$ + $\frac{5}{2}$ $O_2$ $\leftrightharpoons$ 2NO + 3$H_2$ O in terms of $K_1{K}_2$ and $K_3$ is:

1. 

2. 

3. 

4. 

Q. For which of the following reactions, $\Delta H<\Delta E$?

1. $N_2\left(g\right)+3H_2\left(g\right)⟶2{NH}_3\left(g\right)$
2. ${Ag}_{2}O\left(g\right)⟶2Ag\left(s\right)+\frac{1}{2}{O}_2\left(g\right)$
3. $CO\left(g\right)+\frac{1}{2}{O}_2\left(g\right)⟶C{O}_2\left(g\right)$
4. $C\left(s\right)+O_2\left(g\right)⟶C{O}_2\left(g\right)$