Chapter 7 – Equilibrium
At 700 K equilibrium constant for the reaction; H2(g) + I2(g) ⇌ 2HI(g) is 54.8. If 0.5 mol litre^ −1 of HI(g) is present at equilibrium at 700 K, what are the concentrations of H2(g) and I2(g) assuming that we initially started with HI(g) and allowed it to reach equilibrium at 700 K.
22
Nov
At 700 K equilibrium constant for the reaction; H2(g) + I2(g) ⇌ 2HI(g) is 54.8. If 0.5 mol litre^ −1 of HI(g) is present at equilibrium at 700 K, what are the concentrations of H2(g) and I2(g) assuming that we initially started with HI(g) and allowed it to reach equilibrium at 700 K. At 700 [...]
One mole of H2O and one mole of CO are taken in a 10litre vessel and heated to 725 K. At equilibrium, 40percent of water (by mass) reacts with CO according to the equation, H2O(g)+CO(g)⇔H2(g)+CO2(g) Calculate the equilibrium constant for the reaction.
22
Nov
One mole of H2O and one mole of CO are taken in a 10litre vessel and heated to 725 K. At equilibrium, 40percent of water (by mass) reacts with CO according to the equation, H2O(g)+CO(g)⇔H2(g)+CO2(g) Calculate the equilibrium constant for the reaction. 40percent of water (by mass) reacts with CO according to the equation H2O(g)+CO(g)⇔H2(g)+CO2(g) [...]
The equilibrium constant expression for a gas reaction is, KC = [NO]^4 [H2O]^6/ [NH3 ]^4 [O2 ]^5 The balanced chemical equation corresponding to this expression is.
22
Nov
The equilibrium constant expression for a gas reaction is, KC = [NO]^4 [H2O]^6/ [NH3 ]^4 [O2 ]^5 The balanced chemical equation corresponding to this expression is. KC = [NO]^4 [H2O]^6/ [NH3 ]^4 [O2 ]^5 The balanced chemical equation corresponding to this expression is. The equilibrium constant expression for a gas reaction is November [...]
A mixture of 1.57 mol of N2,1.92 mol of H2 and 8.13 mol of NH3 is introduced in a 20L reaction vessel at 500K.At this temperature the equilibrium constant, Kc for the reaction N2 (g)+3H2(g)⇌2NH3(g) is 1.7×10^2. Is the reaction mixture at equilibrium? If not what is the direction of net reaction?
22
Nov
A mixture of 1.57 mol of N2,1.92 mol of H2 and 8.13 mol of NH3 is introduced in a 20L reaction vessel at 500K.At this temperature the equilibrium constant, Kc for the reaction N2 (g)+3H2(g)⇌2NH3(g) is 1.7×10^2. Is the reaction mixture at equilibrium? If not what is the direction of net reaction? 1.92 [...]
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1.92 mol of H2 and 8.13 mol of NH3 is introduced in a 20L reaction vessel at 500K.At this temperature the equilibrium constant ,
A mixture of 1.57 mol of N2 ,
Kc for the reaction N2 (g)+3H2(g)⇌2NH3(g) is 1.7×10^2. Is the reaction mixture at equilibrium? If not what is the direction of net reaction? ,
A sample of HI(g) is placed in flask at a pressure of 0.2 atm. At equilibrium the partial pressure of HI(g) is 0.04 atm. What is KP for the given equilibrium?
22
Nov
A sample of HI(g) is placed in flask at a pressure of 0.2 atm. At equilibrium the partial pressure of HI(g) is 0.04 atm. What is KP for the given equilibrium? A sample of HI(g) is placed in flask at a pressure of 0.2 atm. At equilibrium the partial pressure of HI(g) is 0.04 atm. [...]
At 450K, KP = 2.0×10^10 bar for the given reaction at equilibrium. 2SO2(g) + O2(g)⇌2SO3 (g) What is Kc , at this temperature?
22
Nov
At 450K, KP = 2.0×10^10 bar for the given reaction at equilibrium. 2SO2(g) + O2(g)⇌2SO3 (g) What is Kc , at this temperature? At 450K at this temperature? KP = 2.0×10^10 bar for the given reaction at equilibrium. 2SO2(g) + O2(g)⇌2SO3 (g) What is Kc November 22, 2020 Category: Chapter 7 - Equilibrium [...]
Nitric oxide reacts with bromine and gives nitrosyl-bromide as per reaction given below: 2NO(g)+Br2(g)⇔2NOBr(g). When 0.087mole of NO and 0.0437mole of Br2 are mixed in a closed container at constant temperature, 0.0518mole of NOBr is obtained at equilibrium. Calculate equilibrium amount of nitric oxide and bromine.
22
Nov
Nitric oxide reacts with bromine and gives nitrosyl-bromide as per reaction given below: 2NO(g)+Br2(g)⇔2NOBr(g). When 0.087mole of NO and 0.0437mole of Br2 are mixed in a closed container at constant temperature, 0.0518mole of NOBr is obtained at equilibrium. Calculate equilibrium amount of nitric oxide and bromine. For the following equilibrium for the reverse reaction? KC [...]
Reaction between nitrogen and oxygen takes place as following: 2N2(g)+O2⇔2N2O(g) If a mixture of 0.482 mole N2 and 0.933 mole of O2 is placed in a reaction vessel of volume 10 litre and allowed to form N2O at a temperature for which Kc=2.0 × 10^−37 litre mol^−1. Determine the composition of equilibrium mixture.
22
Nov
Reaction between nitrogen and oxygen takes place as following: 2N2(g)+O2⇔2N2O(g) If a mixture of 0.482 mole N2 and 0.933 mole of O2 is placed in a reaction vessel of volume 10 litre and allowed to form N2O at a temperature for which Kc=2.0 × 10^−37 litre mol^−1. Determine the composition of equilibrium mixture. For the [...]
Explain why pure liquids and solids can be ignored while writing the equilibrium constant expression.
22
Nov
Explain why pure liquids and solids can be ignored while writing the equilibrium constant expression. Explain why pure liquids and solids can be ignored while writing the equilibrium constant expression. November 22, 2020 Category: Chapter 7 - Equilibrium , Chemistry , NCERT Exemplar Class 11 ,
Find out the value of Kc for each of the following equilibria from the value of Kp (a)2NOCl(g)⇔2NO(g)+Cl2(g),Kp=1⋅8×10−2 at 500 K (b) CaCO3(s)⇔CaO(s) ⇔ CaO(s) + CO2(g), Kp=167at1073K.
22
Nov
Find out the value of Kc for each of the following equilibria from the value of Kp (a)2NOCl(g)⇔2NO(g)+Cl2(g),Kp=1⋅8×10−2 at 500 K (b) CaCO3(s)⇔CaO(s) ⇔ CaO(s) + CO2(g), Kp=167at1073K. Find out the value of Kc for each of the following equilibria from the value of Kp (a)2NOCl(g)⇔2NO(g)+Cl2(g) Kp=1⋅8×10−2 at 500 K (b) CaCO3(s)⇔CaO(s) ⇔ CaO(s) + [...]