Le Chatelier's Principle for Del N Greater Than Zero
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Q. Which of the following reactions proceed at low pressure?
- PCl5 ⇌ PCl3 + Cl2
- N2 + O2 ⇌ 2NO
- N2 + 3H2 ⇌ 2NH3
- H2 + I2 ⇌ 2HI
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 ?
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A2(g)+B2(g)⇌X2(g) ;ΔrH=−X kJ ?
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- High temperature and low pressure
- Low temperature and high pressure
- High temperature and high pressure
- Low temperature and low pressure
Q.
For an equilibrium H2O(s)⇌H2O(l), which of the following statements is true?
The pressure changes do not affect the equilibrium
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
Q. For the reaction, PCl5(g)⇌PCl3(g)+Cl2(g) the forward reaction at constant temperature is favoured by
- introducing an inert gas at constant volume
- introducing an inert gas at constant pressure
- increasing the volume of the container
- introducing PCl5 at constant volume
Q. Thermal decomposition of gaseous X2 to gaseous X at 298 K takes place according to the following equation:
X2(g)⇌2X(g)
The standard reaction Gibbs energy, ΔrG0, of this reaction is positive. At the start of the reaction, there is one mole of X2 and no X. As the reaction proceeds, the number of moles of X formed is given by β. Thus, βequilibrium 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−1mol−1)
The equilibrium constant Kp for this reaction at 298 K, in terms of βequilibrium, is:
X2(g)⇌2X(g)
The standard reaction Gibbs energy, ΔrG0, of this reaction is positive. At the start of the reaction, there is one mole of X2 and no X. As the reaction proceeds, the number of moles of X formed is given by β. Thus, βequilibrium 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−1mol−1)
The equilibrium constant Kp for this reaction at 298 K, in terms of βequilibrium, is:
- 8β2equilibrium4−β2equilibrium
- 4β2equilibrium2−βequilibrium
- 4β2equilibrium4−β2equilibrium
- 8β2equilibrium2−βequilibrium
Q. Thermal decomposition of gaseous X2 to gaseous X at 298 K takes place according to the following equation:
X2(g)⇌2X(g)
The standard reaction Gibbs energy, ΔrG0, of this reaction is positive. At the start of the reaction, there is one mole of X2 and no X. As the reaction proceeds, the number of moles of X formed is given by β. Thus, βequilibrium 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−1mol−1).
The INCORRECT statement among the following, for this reaction is:
X2(g)⇌2X(g)
The standard reaction Gibbs energy, ΔrG0, of this reaction is positive. At the start of the reaction, there is one mole of X2 and no X. As the reaction proceeds, the number of moles of X formed is given by β. Thus, βequilibrium 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−1mol−1).
The INCORRECT statement among the following, for this reaction is:
- Decrease in the total pressure will result in formation of more moles of gaseous X
- At the start of the reaction, dissociation of gaseous X2 takes place spontaneously
- Kc<1
- βequilibrium=0.7
Q. Which of the following reactions proceed at low pressure ?
- N2(g)+3H2(g)⇌2NH3(g)
- H2(g)+I2(g)⇌2HI(g)
- N2(g)+O2(g)⇌2NO(g)
- PCl5(g)⇌PCl3(g)+Cl2(g)
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)

2CH3COOH(g)⇌(CH3COOH)2(g)
- −0.263 kJ
- −0613 kJ
- −0.463 kJ
- −0.163 kJ
Q. For a given reaction:
C(s)+O2(g)→Co(g)+H2(g) at 25oC ΔH=131kJ/mol
Given: Kp = 9.36×10−17
Calculate the value of reaction constant at 700oC.
C(s)+O2(g)→Co(g)+H2(g) at 25oC ΔH=131kJ/mol
Given: Kp = 9.36×10−17
Calculate the value of reaction constant at 700oC.
- 0.915
- 0.214
- 0.583
- 0.797
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