Le Chatelier's Principle for Del N Greater Than Zero

Q. Le Chatelier's principle is not applicable for which of the following reaction?

1. $H_2\left(g\right)+I_2\left(g\right)\rightleftharpoons 2HI\left(g\right)$
2. $Fe\left(s\right)+S\left(s\right)\rightleftharpoons FeS\left(s\right)$
3. $N_2\left(g\right)+3H_2\left(g\right)\rightleftharpoons 2N{H}_3\left(g\right)$
4. $N_2\left(g\right)+O_2\left(g\right)\rightleftharpoons 2NO\left(g\right)$

Q. When $NaN{O}_3$ is heated in a closed vessel, oxygen is liberated and $NaN{O}_2$ is left behind.
The reaction is :
$2NaN{O}_3\left(s\right)\rightleftharpoons 2NaN{O}_2\left(s\right)+O_2\left(g\right)$
Which of the following is true at equilibrium?

1. Addition of $NaN{O}_3$ favors backward reaction
2. Addition of $NaN{O}_2$ favors forward reaction
3. Increasing pressure favors reverse reaction.
4. All of the above.

Q. Which of the following factors will not disturb the equilibrium state of the reaction? $H_2\left(g\right)+I_2\left(g\right)\rightleftharpoons 2HI\left(g\right){\Delta }_{r}H=+3000\text{cal}$

1. Change in temperature
2. Addition of catalyst
3. Addition of $H_2$
4. All of the above.

Q. For a given reaction:
$C\left(s\right)+O_2\left(g\right)\to Co\left(g\right)+H_2\left(g\right)$ at ${25}^{o}C$ $\Delta H=131kJ/mol$
Given: $K_p$ = $9.36\times {10}^{-17}$
Calculate the value of reaction constant at ${700}^{o}C$.

1. $0.915$
2. $0.214$
3. $0.583$
4. $0.797$

Q. Which of the following reactions will be favored in the forward direction when the pressure in a system is increased?
$I.CaC{O}_3\left(s\right)\rightleftharpoons CaO\left(s\right)+CO\left(g\right)$
$II.Mg\left(s\right)+2H_{2}O\left(g\right)\rightleftharpoons Mg\left(OH{)}_2\right(aq)+H_2(g)$
$III.2N_2{O}_5\left(g\right)\rightleftharpoons O_2\left(g\right)+4N{O}_2\left(g\right)$

1. II only
2. I only
3. I and II only
4. I, II, and III

Q. For the given reaction :
$2A\left(g\right)+B\left(g\right)\rightleftharpoons C\left(g\right),△H=-ve$
Which of the following conditions favour the formation of products?

1. Low Pressure
   
2. High Pressure
   
3. Low Temperature
   
4. High Temperature

Q. For the given reaction :
$2A\left(g\right)+B\left(g\right)\rightleftharpoons C\left(g\right),△H=-ve$
Which of the following conditions favour the formation of products?

1. Low Pressure
   
2. High Pressure
   
3. Low Temperature
   
4. High Temperature

Q. Given reaction:
$N_2\left(g\right)+3H_2\left(g\right)\rightleftharpoons 2N{H}_3\left(g\right)$
What would happen if there is a decrease in volume of container in which reaction occurs?

1. Less $N{H}_3$ would form
2. More $N_2$ would form
3. More $N{H}_3$ would form
4. More $H_2$ would form

Q. Consider the following reaction taking place in a container,
$2A\left(g\right)\rightleftharpoons 3B\left(g\right)$
On doubling the volume of the container, the equilibrium amount of the product would:

1. increase
2. decrease
3. remain same
4. Data is insufficient

Q. Which of the following reactions will be favoured at low pressure?

1. $N_2\left(g\right)+3H_2\left(g\right)\rightleftharpoons 2N{H}_3\left(g\right)$
2. $H_2\left(g\right)+I_2\left(g\right)\rightleftharpoons 2HI\left(g\right)$
3. $PC{l}_5\left(g\right)\rightleftharpoons PC{l}_3\left(g\right)+C{l}_2\left(g\right)$
4. $N_2\left(g\right)+O_2\left(g\right)\rightleftharpoons 2NO\left(g\right)$

Q. A system at equilibrium is described by the equation at a fixed temperature T.
$S{O}_{2}C{l}_2\left(g\right)\rightleftharpoons S{O}_2\left(g\right)+C{l}_2\left(g\right)$
What effect will an increases in the total pressure is caused by a decrease in volume have on the equilibrium?

1. Concentration of $S{O}_{2}C{l}_2\left(g\right)$ increases
2. Concentration of $S{O}_2\left(g\right)$ increases
3. Concentration of $C{l}_2\left(g\right)$ increases
4. Concentration of all gases increases

Q. Which of the following factor shifts the reaction,
$PC{l}_3\left(g\right)+C{l}_2\left(g\right)\rightleftharpoons PC{l}_5\left(g\right);\Delta H=-ve$ towards the reactant side?

1. Addition of $PC{l}_5$
2. Increasing the pressure
3. Decreasing the temperature
4. Addition of a catalyst

Q. Which of the following reaction will not be affected by increasing the pressure?

1. $PC{l}_3\left(g\right)\rightleftharpoons PC{l}_3\left(g\right)+C{l}_2\left(g\right)$
2. $N_2\left(g\right)+O_2\left(g\right)\rightleftharpoons 2NO\left(g\right)$
3. $CaC{O}_3\left(s\right)\rightleftharpoons CaO\left(s\right)+C{O}_2\left(g\right)$
4. $CO\left(g\right)+H_{2}O\left(g\right)\rightleftharpoons C{O}_2\left(g\right)+H_2\left(g\right)$

Q. Predict the effect upon the following reaction equilibria of increased pressure.
$\left(1\right)H_{2}O\left(g\right)\rightleftharpoons H_2\left(g\right)+\frac{1}{2}{O}_2\left(g\right)\left(2\right)CaC{O}_3\left(s\right)\rightleftharpoons CaO\left(s\right)+C{O}_2\left(g\right)\left(3\right)C\left(s\right)+H_{2}O\left(g\right)\rightleftharpoons H_2\left(g\right)+CO\left(g\right)$

1. Left, Left, Left
2. Right, Right, Right
3. Left, Right, Left
4. Right, Left, Right

Q. The following reaction attains equilibrium at high temperature.
$N_2\left(g\right)+2H_{2}O\left(g\right)+\text{heat}\rightleftharpoons 2NO\left(g\right)+2H_2\left(g\right)$
The yield of $NO$ is affected by

1. Increasing the nitrogen concentration
2. Decreasing the hydrogen concentration
3. Compressing the reaction mixture
4. None of these

Q.

For an equilibrium $H_{2}O\left(s\right)\rightleftharpoons H_{2}O\left(l\right)$, which of the following statements is true?

1. The pressure changes do not affect the equilibrium

2. More of ice melts if pressure on the system is increased

3. More of liquid freezes if pressure on the system is increased

4. The pressure changes may increase or decrease the degree of advancement of the reaction depending upon the temperature of the system

Q. Consider a reaction :
A(g) + B(g) $\rightleftharpoons$ C(g)
The backward reaction is favoured by :

1. Decrease in pressure
2. Increase in pressure
3. Increase in concentration of $\left[B\right]$
4. None of the above

Q. The solubility product of $AgBr\left(s\right)$ is $5\times {10}^{-13}$ at $298K$. If the standard reduction potential of the half cell $E_{B{r}^{-}|AgBr|Ag}^0$ is $0.07V$.
Find the value of the $E_{A{g}^{+}/Ag}^0$

Q. The exothermic formation of $CI{F}_3$ is represented by the equation:
$C{l}_2\left(g\right)+3F_2\left(g\right)\rightleftharpoons 2CI{F}_3\left(g\right);△H=-329kJ$
Which of the following will increase the quantity of $CI{F}_3$ in an equilibrium mixture of $C{l}_2,F_{2}andCI{F}_3$?

1. By addition of $F_2$
2. Increasing the volume of the container
3. By removal of $C{l}_2$
4. Increasing the temperature

Q. Predict the effect upon the following reaction equilibria of increased pressure.
$\left(1\right)H_{2}O\left(g\right)\rightleftharpoons H_2\left(g\right)+\frac{1}{2}{O}_2\left(g\right)\left(2\right)CaC{O}_3\left(s\right)\rightleftharpoons CaO\left(s\right)+C{O}_2\left(g\right)\left(3\right)C\left(s\right)+H_{2}O\left(g\right)\rightleftharpoons H_2\left(g\right)+CO\left(g\right)$

1. Left, Left, Left
2. Right, Right, Right
3. Left, Right, Left
4. Right, Left, Right

Q. When hydrochloric acid is added to cobalt nitrate solution at room temperature, the following reaction takes place and the reaction mixture becomes blue. On cooling the mixture, it becomes pink. On the basis of this information mark the correct answer.
$\underset{\left(pink\right)}{{\left[Co\right(H_{2}O{)}_5]}^{3+}}\left(aq\right)+4C{l}^{-}\left(aq\right)\rightleftharpoons \underset{\left(blue\right)}{[CoC{l}_4{]}^{2-}}\left(aq\right)+6H_{2}O\left(l\right)$

1. $\Delta H>0$ for the reaction
2. $\Delta H<0$ for the reaction
3. $\Delta H=0$ for the reaction
4. The sign of $\Delta H$ cannot be predicted on the basis of this information

Q. Reaction in which, the yield of product(s) increases with an increase in pressure is:

1. $H_2\left(g\right)+I_2\left(g\right)\rightleftharpoons 2HI\left(g\right)$
2. $H_{2}O\left(g\right)+CO\left(g\right)\rightleftharpoons C{O}_2\left(g\right)+H_2\left(g\right)$
3. $H_{2}O\left(g\right)+C\left(s\right)\rightleftharpoons CO\left(g\right)+H_2\left(g\right)$
4. $CO\left(g\right)+3H_2\left(g\right)\rightleftharpoons C{H}_4\left(g\right)+H_{2}O\left(g\right)$

Q. Equilibrium constant, $K_C$ for the reaction
$N_2\left(g\right)+3H_2\left(g\right)\leftrightharpoons 2N{H}_3\left(g\right)$ at 500 K is 0.061 $L^{2}mo{l}^{-2}$.
At a particular time, the analysis shows that composition of the reaction mixure is $3.0mol{L}^{-1}$ $N_2,2.0$ $molL$${}^{-1}{H}_2$ and $0.5mol{L}^{-1}$ $N{H}_3$. What will be the direction of equilibrium?

1. at equilibrium
2. not at equilibrium, backward shift
3. not at equilibrium, forward shift
4. can not be predicted

Q. Equilibrium constant, $K_C$ for the reaction
$N_2\left(g\right)+3H_2\left(g\right)\leftrightharpoons 2N{H}_3\left(g\right)$ at 500 K is 0.061 $L^{2}mo{l}^{-2}$.
At a particular time, the analysis shows that composition of the reaction mixure is $3.0mol{L}^{-1}$ $N_2,2.0$ $molL$${}^{-1}{H}_2$ and $0.5mol{L}^{-1}$ $N{H}_3$. What will be the direction of equilibrium?

1. at equilibrium
2. not at equilibrium, backward shift
3. not at equilibrium, forward shift
4. can not be predicted

Q. The volume of the reaction vessel containing an equilibrium mixture in the reaction is increased, when equilibrium is re-established:
$S{O}_{2}C{l}_2\left(g\right)\rightleftharpoons S{O}_2\left(g\right)+C{l}_2\left(g\right)$

1. The amount of $S{O}_2$ will have decreased
2. The amount of $S{O}_{2}C{l}_2$ will have increased
3. The amount of $C{l}_2$ will have increased
4. The amount of $C{l}_2$ will have remained unchanged

Q. When hydrochloric acid is added to cobalt nitrate solution at room temperature, the following reaction takes place and the reaction mixture becomes blue. On cooling the mixture, it becomes pink. On the basis of this information mark the correct answer.
$\underset{\left(pink\right)}{{\left[Co\right(H_{2}O{)}_5]}^{3+}}\left(aq\right)+4C{l}^{-}\left(aq\right)\rightleftharpoons \underset{\left(blue\right)}{[CoC{l}_4{]}^{2-}}\left(aq\right)+6H_{2}O\left(l\right)$

1. $\Delta H>0$ for the reaction
2. $\Delta H<0$ for the reaction
3. $\Delta H=0$ for the reaction
4. The sign of $\Delta H$ cannot be predicted on the basis of this information

Q. Given reaction:
$N_2\left(g\right)+3H_2\left(g\right)\rightleftharpoons 2N{H}_3\left(g\right)$
What would happen if there is a decrease in volume of container in which reaction occurs?

1. Less $N{H}_3$ would form
2. More $N_2$ would form
3. More $N{H}_3$ would form
4. More $H_2$ would form

Q. Reaction :
$Ba{O}_2\left(s\right)\rightleftharpoons BaO\left(s\right)+O_2\left(g\right)\Delta H=+ve$
In equilibrium condition, pressure of $O_2$ depends on :

1. Mass of $Ba{O}_2$
2. Mass of $BaO$
3. Increasing temperature at equilibrium.
4. (a) and (b) above.

Q. Thermal decomposition of gaseous $X_2$ to gaseous X at 298 K takes place according to the following equation:
$X_2\left(g\right)\rightleftharpoons 2X\left(g\right)$
The standard reaction Gibbs energy, ${\Delta }_r{G}^0,$ of this reaction is positive. At the start of the reaction, there is one mole of $X_2$ and no X. As the reaction proceeds, the number of moles of X formed is given by $\beta$. Thus, ${\beta }_{equilibrium}$ is the number of moles of X formed at equilibrium. The reaction is carried out at a constant total pressure of 2 bar. Consider the gases to behave ideally. (Given: R = 0.083 L bar $K^{-1}mo{l}^{-1}$).

The INCORRECT statement among the following, for this reaction is:

1. Decrease in the total pressure will result in formation of more moles of gaseous X
2. At the start of the reaction, dissociation of gaseous $X_2$ takes place spontaneously
3. ${\beta }_{equilibrium}=0.7$
4. $K_c<1$

Q. A certain reaction has value of $K_p=0.0260$ at ${25}^{o}C$ and ${\Delta }_{rxn}{H}^o=32.4kJmo{l}^{-1}$. Calculate the value of $K_p$ at ${57}^{o}C$.
antilog 0.55 = 3.55

1. 0.1431
2. 0.0924
3. 0.2431
4. 0.0431