Which of the following statements is (are) correct ?
The value of equilibrium constant of a reversible reaction at a given temperature :
Which of the following statement is (are) correct ?
If is found that the equilibrium constant increases by factor of four when the temperature is increased from 25°C to 40°C. The value of ΔH° is
As we know
Ammonium carbamate dissociates as follows :
NH2COONH4(s) 2NH3(g) + CO2(g)
The value of KP for this reaction is found to be equal to 2.92 × 10-5 atm3. If one mole of ammonium carbamate is heated in a sealed container, the total pressur develped in the container is
The equilibrium constant for the following reactions at 1400 K are given.
2H2O(g) 2H2(g) + O2(g) ; K1=2.1×10-13
2CO2(g)2CO(g)+O2(g);K2 = 1.4 × 10-12
Then, the equilibrium constant K for the reaction
H2(g) + CO2(g) CO(g) + H2O(g) is
Under what conditions of temperature and pressure, the formation of atomic hydrogen from molecular hydrogen will be favoured most ?
For the reaction PCl5(g) PCl3(g) + Cl2(g), the forward reaction at constant temperature is favoured by
Introduction of inet gas at constant Pressure will increase Pressure of gases of equilibrium
⇒ equilibrium shifted forward
When NaNO3(s) is heated in a closed vessel, oxygen is liberated and NaNO2(s) is left behind. At equilibrium.
High temperature
∴ forward reaction favoured 1000 pressure
High pressure → Reverse reaction
Phase diagram of CO2 is shown as following
Based on above find the correct statement (s)
The equilibrium between, gaseous isomers A, B and C can be represented as
Reaction Equilibrium constant
A(g) B (g) : K1 = ?
B(g) C(g) : K2 = 0.4
C(g) A(g) : K3 = 0.6
If one mole of A is taken in a closed vessel of volume 1 litre, then
For the gas phase exothermic reaction.
A2 + B2 C2, carried out in a closed vessel, the equilibrium moles of A2 can be increased by
According to Le Chatelier’s Principle A, B and C are correct.
Hence A, B and C
Consider the equilibrium
HgO(s) + 4I- (aq) + H2O(l) Hg I42- (aq) + 2OH- (aq), which changes will decrease the equilibrium concentration of HgI42-
As given :
In the laboratory the equilibrium constant for a particular reaction can be measured at different temperatures. Plotting the data yields the graph shown. Which of the following statements is false?
(Note : The notation 4.40 e- 4 is equivalent to 4.40 × 10-4)
slope of the line equal to ΔHº/R
Decrease in the pressure for the following equilibria : H2O (s) H2O(l) result in the :
∴ formation of more H2O (s) and increase in melting point of H2O (s)
Statement-1 : Water boils at high temperature in pressure cooker.
Statement-2 : Increase in pressure leads to an increase in boiling point.
Statement-1 is true, statement-2 is true and statement-2 is correct explanation for statement-1
Statement-1 : A decrease in pressure leads to an increase in freezing point of water.
Statement-2 : For ice on melting volume decreases.
Statement-1 is true, statement-2 is true and statement-2 is correct explanation for statement-1
Statement-1 : The solubility of gases always increases with increase in pressure.
Statement-2 : High pressure favours the change where volume of gas decreases.
Statement-1 is true, statement-2 is true and statement-2 is correct explanation for statement-1
Statement-1 : Total number of moles in a closed system at new equilibrium is less than the old equilibrium if some amount of a substance is removed from a system.
A(g) B(g) equilibrium.
Statement-2 : The number of moles of the substance which is removed, is partially compensated as the system reached to new equilibrium.
Statement-1 is true, statement-2 is true and statement-2 is NOT the correct explanation for statement-1
Statement-1 : An exothermic reaction, non-spontaneous at high temperature, may become spontaneous at low temperature.
Statement-2 : Entropy of an exothermic reaction always decrease with decrease in temperature.
Statement-I is false, statement-2 is true.
Statement-1 : Ammonia at a pressure of 10 atm and CO2 at a pressure of 20 atm are intoduced into an evacuated chamber. If Kp for the reaction.
NH2COONH4(s) 2NH3(g) + CO2(g) is 2020 atm3, the total pressure after a long time is less than 30 atm.
Statement-2 : Equilibrium can be attained from both directions.
Statement-1 is true, statement-2 is false.
In a 7.0 L evacuated chamber, 0.50 mol H2 and 0.50 mol I2 react at 427°C
H2(g) + I2 (g) 2HI(g). At the given temperature, Kc = 49 for the reaction.
What is the value of Kp ?
In a 7.0 L evacuated chamber, 0.50 mol H2 and 0.50 mol I2 react at 427°C
H2(g) + I2 (g) 2HI(g). At the given temperature, Kc = 49 for the reaction.
What is the total pressure (atm) in the chamber
In a 7.0 L evacuated chamber, 0.50 mol H2 and 0.50 mol I2 react at 427°C
H2(g) + I2 (g) 2HI(g). At the given temperature, Kc = 49 for the reaction.
How many moles of the iodine remain unreacted at equilibrium ?
from above question
In a 7.0 L evacuated chamber, 0.50 mol H2 and 0.50 mol I2 react at 427°C
H2(g) + I2 (g) 2HI(g). At the given temperature, Kc = 49 for the reaction.
What is the partial pressure (atm) of HI in the equilibrium mixture ?
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