Vant Hoff's Equation and Effect of Temperature on Equilibrium Constant
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The favourable conditions for the forward reaction are:
- Increasing temperature as well as pressure
- Lowering the temperature and increasing the pressure
- Lowering of temperature as well as pressure
- Lowering the pressure and increasing the temperature
For the reaction 2NO(g)⇌N2(g)+O2(g), ΔH=−180 kJ mol−1. Which of the following facts does not hold well?
The volume changes at constant temperature do not affect the equilibrium constant
The dissociation of NO is favored less at high temperature
The pressure changes at constant temperature do not affect the equilibrium constant
The dissociation of NO is favored more at high temperature
2SO2(g) + O2(g) ⇋ 2SO3(g) △ H = −45 kCal
- High pressure will be favorable for production of
- High temperature will favor forward reaction.
- Decreasing
concentration will reduce the rate of backward reaction.
- Doubling the volume of container while keeping temperature same, will shift the equilibrium in reverse direction.
The oxidation of SO2 by O2 to SO3 is an exothermic reaction. The yield of SO3 will be maximum if
Temperature is increased and pressure is kept constant
Temperature is reduced and pressure is increased
Both temperature and pressure are increased
Both temperature and pressure are reduced
- The pressure inside the container will not change
- The temperature will not change
- the temperature will decrease
- The temperature will increase
In the reaction N2(g) + 3H2(g) ⇌ 2NH3(g), the value of the equilibrium
constant depends on
-
The temperature
Volume of the reaction vessel
Total pressure of the system
The initial concentration of nitrogen and hydrogen
For an equilibrium reaction A (g) + B (g) ⇌ C (g) + D (g), ΔH = -ve. An increase in temperature would cause
No change in the value of
A decrease in the value of
A change in
which cannot be qualitatively predicted
An increase in the value of
\(N_2 ~+ ~O_2 ~\rightleftharpoons~ 2NO ~+~ (-Q cals)\)
In the above reaction which is the essential condition for the higher production of NO
High temperature
High pressure
Low temperature
Low pressure
H = +ve.
H = -ve.
H whose sign cannot be predicted
H = Zero
For an equilibrium reaction A (g) + B (g)⇌ C (g) + D (g), ΔH = +ve. An increase in temperature would cause
An increase in the value of
No change in the value of
A change in
which cannot be qualitatively predicted
A decrease in the value of