Le Chatelier's Principle for Del N Greater Than Zero
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Q.
What happens to equilibrium when the volume is increased?
Q.
For an equilibrium H2O(s)⇌H2O(l), which of the following statements is true?
More of ice melts if pressure on the system is increased
More of liquid freezes if pressure on the system is increased
The pressure changes may increase or decrease the degree of advancement of the reaction depending upon the temperature of the system
The pressure changes do not affect the equilibrium
Q. Which of the following reaction will not be affected by increasing the pressure?
- PCl3(g)⇌PCl3(g)+Cl2(g)
- N2(g)+O2(g)⇌2NO(g)
- CaCO3(s)⇌CaO(s)+CO2(g)
- CO(g)+H2O(g)⇌CO2(g)+H2(g)
Q. The volume of the reaction vessel containing an equilibrium mixture in the reaction is increased, when equilibrium is re-established:
SO2Cl2(g)⇌SO2(g)+Cl2(g)
SO2Cl2(g)⇌SO2(g)+Cl2(g)
- The amount of SO2 will have decreased
- The amount of SO2Cl2 will have increased
- The amount of Cl2 will have increased
- The amount of Cl2 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. CaCO3 (s)⇌CaO (s)+CO (g)
II. Mg (s)+2H2O (g)⇌Mg(OH)2 (aq)+H2 (g)
III. 2N2O5 (g)⇌O2 (g)+4NO2 (g)
I. CaCO3 (s)⇌CaO (s)+CO (g)
II. Mg (s)+2H2O (g)⇌Mg(OH)2 (aq)+H2 (g)
III. 2N2O5 (g)⇌O2 (g)+4NO2 (g)
- II only
- I only
- I and II only
- I, II, and III
Q. Which one of the following conditions will favour maximum formation of the product in the reaction,
A2 (g)+B2 (g)⇌X2 (g) ΔrH=−X kJ
A2 (g)+B2 (g)⇌X2 (g) ΔrH=−X kJ
- High temperature and high pressure
- High temperature and low pressure
- Low temperature and high pressure
- 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?
- A
- B
- C
- 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) COCl2(g)⇌CO(g)+Cl2(g)
(ii) CH4(g)+2S2(g)⇌CS2(g)+2H2S(g)
(iii) CO2(g)+C(s)⇌2CO(g)
(iv) 2H2(g)+CO(g)⇌CH3OH(g)
(v) CaCO3(s)⇌CaO(s)+CO2(g)
(vi) 4NH3(g)+5O2(g)⇌4NO(g)+6H2O(g)
(i) COCl2(g)⇌CO(g)+Cl2(g)
(ii) CH4(g)+2S2(g)⇌CS2(g)+2H2S(g)
(iii) CO2(g)+C(s)⇌2CO(g)
(iv) 2H2(g)+CO(g)⇌CH3OH(g)
(v) CaCO3(s)⇌CaO(s)+CO2(g)
(vi) 4NH3(g)+5O2(g)⇌4NO(g)+6H2O(g)
Q. Consider the reaction : 2SO2(g)+O2(g)⇌2SO3(g);△Ho=−198 kJ
The favourable conditions for the forward reaction are:
The favourable conditions for the forward reaction are:
- Increasing temperature as well as pressure
- Lowering the temperature and increasing the pressure
- Any value of temperature and pressure
- Lowering of temperature as well as pressure
Q. The exothermic formation of CIF3 is represented by the equation:
Cl2(g)+3F2(g)⇌2CIF3(g);△H=−329 kJ
Which of the following will increase the quantity of CIF3 in an equilibrium mixture of Cl2, F2 and CIF3?
Cl2(g)+3F2(g)⇌2CIF3(g);△H=−329 kJ
Which of the following will increase the quantity of CIF3 in an equilibrium mixture of Cl2, F2 and CIF3?
- By addition of F2
- Increasing the volume of the container
- By removal of Cl2
- Increasing the temperature
Q. Le Chatelier's principle is not applicable for which of the following reaction?
- H2 (g)+I2 (g)⇌2HI (g)
- Fe (s)+S (s)⇌FeS (s)
- N2 (g)+3H2 (g)⇌2NH3 (g)
- N2 (g)+O2 (g)⇌2NO (g)
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:
This is known as:
- First Law of Thermodynamics
- Le-Chatelier's principle
- Ostwald's Rule
- None of the above
Q. For the reaction: Cl2(g)+3F2(g)⇌2ClF3(g); ΔH=−329 kJ, dissociation of ClF3(g) will be favoured by:
- Increasing the temperature
- Decreasing the volume of the container
- Addition of F2 gas
- Addition of inert gas at constant pressure
Q. Reaction :
BaO2 (s)⇌BaO (s)+O2 (g) ΔH=+ve
In equilibrium condition, pressure of O2 depends on :
BaO2 (s)⇌BaO (s)+O2 (g) ΔH=+ve
In equilibrium condition, pressure of O2 depends on :
- Mass of BaO2
- Mass of BaO
- Increasing temperature at equilibrium.
- (a) and (b) above.
Q. An increase in the concentration of the reactants of a reaction leads to change in :
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- collision frequency
- threshold energy
- heat of reaction
- activation energy
Q. Acetic acid CH3COOH can form a dimer (CH3COOH)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 25oC, the equilibrium constant for the dimerization is 1.3×103. Calculate △So for the reaction:
2CH3COOH(g)⇌(CH3COOH)2(g)
If at 25oC, the equilibrium constant for the dimerization is 1.3×103. Calculate △So for the reaction:
2CH3COOH(g)⇌(CH3COOH)2(g)
- −0.263 kJ
- −0.463 kJ
- −0.163 kJ
- −0613 kJ
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 ??