Le Chatelier's Principle for Del N Greater Than Zero

Q.

What happens to equilibrium when the volume is increased?

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

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

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

4. The pressure changes do not affect the equilibrium

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. 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. 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. Which one of the following conditions will favour maximum formation of the product in the reaction,
$A_2\left(g\right)+B_2\left(g\right)\rightleftharpoons X_2\left(g\right){\Delta }_{r}H=-XkJ$

1. High temperature and high pressure
2. High temperature and low pressure
3. Low temperature and high pressure
4. Low temperature and hlow pressure

Q. Four alkali metals $A,B,C$ and $D$ are having respectively standard reduction potentials as $3.05,1.66,0.40$ and $0.80$ V. Which one will be the most reducing agent?

1. A
2. B
3. C
4. D

Q. Which of the following reactions will get affected by increasing the pressure? Also, mention whether change will cause the reaction to go into forward or backward direction.
(i) ${COCl}_2\left(g\right)\rightleftharpoons CO\left(g\right)+{Cl}_2\left(g\right)$
(ii) ${CH}_4\left(g\right)+2S_2\left(g\right)\rightleftharpoons {CS}_2\left(g\right)+2H_{2}S\left(g\right)$
(iii) ${CO}_2\left(g\right)+C\left(s\right)\rightleftharpoons 2CO\left(g\right)$
(iv) $2H_2\left(g\right)+CO\left(g\right)\rightleftharpoons {CH}_{3}OH\left(g\right)$
(v) ${CaCO}_3\left(s\right)\rightleftharpoons CaO\left(s\right)+{CO}_2\left(g\right)$
(vi) $4{NH}_3\left(g\right)+5O_2\left(g\right)\rightleftharpoons 4NO\left(g\right)+6H_{2}O\left(g\right)$

Q. Consider the reaction : $2S{O}_2\left(g\right)+O_2\left(g\right)\rightleftharpoons 2S{O}_3\left(g\right);△H^o=-198kJ$
The favourable conditions for the forward reaction are:

1. Increasing temperature as well as pressure
2. Lowering the temperature and increasing the pressure
3. Any value of temperature and pressure
4. Lowering of temperature as well as pressure

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. 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 in any system at equilibrium state pressure, temperature or concentration is changed then the equilibrium will shift in such a direction which neutralizes the effect of change.
This is known as:

1. First Law of Thermodynamics
2. Le-Chatelier's principle
3. Ostwald's Rule
4. None of the above

Q. For the reaction: $C{l}_2\left(g\right)+3F_2\left(g\right)\rightleftharpoons 2Cl{F}_3\left(g\right);\Delta H=-329\text{kJ}$, dissociation of $Cl{F}_3\left(g\right)$ will be favoured by:

1. Increasing the temperature
2. Decreasing the volume of the container
3. Addition of $F_2$ gas
4. Addition of inert gas at constant pressure

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. An increase in the concentration of the reactants of a reaction leads to change in :

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1. collision frequency
2. threshold energy
3. heat of reaction
4. activation energy

Q. Acetic acid $C{H}_{3}COOH$ can form a dimer $(C{H}_{3}COOH{)}_2$ in the gas phase. The dimer is held together by two H-bonds with a total strenght of 66.5 kJ per mol of dimer
If at ${25}^{o}C,$ the equilibrium constant for the dimerization is $1.3\times {10}^3.$ Calculate $△S^o$ for the reaction:
$2C{H}_{3}COOH\left(g\right)\rightleftharpoons \left(C{H}_{3}COOH{)}_2\right(g)$

1. $-0.263kJ$
2. $-0.463kJ$
3. $-0.163kJ$
4. $-0613kJ$

Q. The following reaction is made to reach equilibrium. 3H2 + N2 gives 2NH3 What will be the effect of equilibrium if the volume of the vessel is decreased?

Q.

How does equilibrium gets effected when pressure is decreased ??