Le Chatelier's Principle for Del N Equals to 0

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. Adding an inert gas

2. Adding a suitable catalyst

3. Decreasing the volume of the container

4. Increasing the amount of CO (g)

Q. For the gaseous reaction, $pA+qB\rightleftharpoons qC+pD$, which of the following relationship is true?

1. 
2. 
3. 
4. 

Q. The effect of increasing the pressure on the equilibrium for the given reaction is
2A + 3B $\rightleftharpoons$ 3C + 2D

1. Forward reaction is favoured
2. Backward reaction is favoured
3. No effect
4. It will stop the reaction

Q.

Regarding the rate of a reversible reaction, the correct explanation of the effect

of catalyst is

1. It provides a new reaction path of low activation energy

2. It decreases the velocity of backward reaction

3. It increases the kinetic energy of reacting molecules

4. It displaces the equilibrium state on right side

Q.

The effect of increasing the pressure on the equilibrium

$2A\left(g\right)+3B\left(g\right)\rightleftharpoons 3A\left(g\right)+2B\left(g\right)$ is

1. Backward reaction is favoured
2. None of the above
3. Forward reaction is favoured
4. No effect

Q. The yield of product in the reaction,
$A_2\left(g\right)+2B\left(g\right)\rightleftharpoons C\left(g\right)+QkJ$
would be higher at:

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

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. The equilibrium reaction that is not influenced by volume change at constant temperature is:

1. $2NO\left(g\right)+O_2\left(g\right)\rightleftharpoons 2N{O}_2\left(g\right)$
2. $H_2\left(g\right)+I_2\left(g\right)\rightleftharpoons 2HI\left(g\right)$
3. $N_2\left(g\right)+3H_2\left(g\right)\rightleftharpoons 2N{H}_3\left(g\right)$
4. $N_2{O}_4\left(g\right)\rightleftharpoons 2N{O}_2\left(g\right)$

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) $COC{l}_2\left(g\right)\leftrightarrow CO\left(g\right)+C{l}_2\left(g\right)$
(ii) $C{H}_4\left(g\right)+2S_2\left(g\right)\leftrightarrow C{S}_2\left(g\right)+2H_{2}S\left(g\right)$
(iii) $C{O}_2\left(g\right)+C\left(s\right)\leftrightarrow 2CO\left(g\right)$
(iv) $2H_2\left(g\right)+CO\left(g\right)\leftrightarrow C{H}_{3}OH\left(g\right)$
(v) $CaC{O}_3\left(s\right)\leftrightarrow CaO\left(s\right)+C{O}_2\left(g\right)$
(vi) $4N{H}_3\left(g\right)+5O_2\left(g\right)\leftrightarrow 4NO\left(g\right)+6H_{2}O\left(g\right)$

Q. According to le-Chatelier 's principle, adding heat to a solid and liquid in equilibrium will cause the :

1. Amount of solid to decrease
2. Amount of liquid to decrease
3. Temperature to rise
4. Temperature to fall