Chemistry
The species present in solution when CO2 is dissolved in water are
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Nov
The species present in solution when CO2 is dissolved in water are The species present in solution when CO2 is dissolved in water are November 17, 2020 Category: Chapter 7 - Equilibrium , Chemistry , JEE Adv and Mains Chemistry 41 Years Solved Video Solutions 1979 - 2019 ,
For the reaction, SO2(g)+1/2O2(g)⇌SO3(g) if KP=KC(RT)x X where, the symbols have usual meaning, then the value of x is (assuming ideality)
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Nov
For the reaction, SO2(g)+1/2O2(g)⇌SO3(g) if KP=KC(RT)x X where, the symbols have usual meaning, then the value of x is (assuming ideality) For the reaction SO2(g)+1/2O2(g)⇌SO3(g) if KP=KC(RT)x X where the symbols have usual meaning then the value of x is (assuming ideality) November 17, 2020 Category: Chapter 7 - Equilibrium , Chemistry , JEE Adv [...]
An aqueous solution contains 0.10 M H2 S and 0.20 M HCl . If the equilibrium constants for the formation of HS− from H2S is 1.0×10^−7 and that of S2− from HS− ions is 1.2×10^−13 then the concentration of S2− ions in aqueous solution is-duplicate-4
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Nov
An aqueous solution contains 0.10 M H2 S and 0.20 M HCl . If the equilibrium constants for the formation of HS− from H2S is 1.0×10^−7 and that of S2− from HS− ions is 1.2×10^−13 then the concentration of S2− ions in aqueous solution is-duplicate-4 Two solids dissociate as follows A(s)↽−−⇀B(g) + C(g);Kp1 = x [...]
The equilibrium constant at 298 K for a reaction A+B↽−−⇀C+D is 100. If the initial concentration of all the four species were 1 M each, then equilibrium concentration of D (in mol L^−1) will be :
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Nov
The equilibrium constant at 298 K for a reaction A+B↽−−⇀C+D is 100. If the initial concentration of all the four species were 1 M each, then equilibrium concentration of D (in mol L^−1) will be : The equilibrium constant at 298 K for a reaction A+B↽−−⇀C+D is 100. If the initial concentration of all the [...]
An aqueous solution contains 0.10 M H2 S and 0.20 M HCl . If the equilibrium constants for the formation of HS− from H2S is 1.0×10^−7 and that of S2− from HS− ions is 1.2×10^−13 then the concentration of S2− ions in aqueous solution is
16
Nov
An aqueous solution contains 0.10 M H2 S and 0.20 M HCl . If the equilibrium constants for the formation of HS− from H2S is 1.0×10^−7 and that of S2− from HS− ions is 1.2×10^−13 then the concentration of S2− ions in aqueous solution is Two solids dissociate as follows A(s)↽−−⇀B(g) + C(g);Kp1 = x [...]
Consider the following reversible chemical reactions : A2(g) + B2(g) ⇌ K12AB(g) ….(1) 6AB(g) ⇌ K23A2(g) + 3B2(g) …(2) The relation between K1 and K2 is :
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Nov
Consider the following reversible chemical reactions : A2(g) + B2(g) ⇌ K12AB(g) ….(1) 6AB(g) ⇌ K23A2(g) + 3B2(g) …(2) The relation between K1 and K2 is : Consider the following reversible chemical reactions : A2(g) + B2(g) ⇌ K12AB(g) ....(1) 6AB(g) ⇌ K23A2(g) + 3B2(g) ...(2) The relation between K1 and K2 is : November [...]
The value of Kp/KC for the following reactions at 300K are, respectively : (At 300K, RT = 24.62 dm^3 atm mol^−1) N2(g)+O2(g)↽−−⇀2NO(g) N2O4(g)↽−−⇀2NO2(g) N2(g)+3H2(g)↽−−⇀2NH3(g)
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Nov
The value of Kp/KC for the following reactions at 300K are, respectively : (At 300K, RT = 24.62 dm^3 atm mol^−1) N2(g)+O2(g)↽−−⇀2NO(g) N2O4(g)↽−−⇀2NO2(g) N2(g)+3H2(g)↽−−⇀2NH3(g) respectively : (At 300K RT = 24.62 dm^3 atm mol^−1) N2(g)+O2(g)↽−−⇀2NO(g) N2O4(g)↽−−⇀2NO2(g) N2(g)+3H2(g)↽−−⇀2NH3(g) The value of Kp/KC for the following reactions at 300K are November 16, 2020 Category: Chapter 7 - [...]
5⋅1g NH4SH is introduced in 3.0 L evacuated flask at 327^∘C. 30% of the solid NH4SH decomposed to NH3 and H2S as gases. The Kp of the reaction at 327^∘C is (R=0⋅082 atm mol^−1K^−1, Molar mass of S = 32 g mol^-1, molar mass of N = 14 g mol^−1)
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Nov
5⋅1g NH4SH is introduced in 3.0 L evacuated flask at 327^∘C. 30% of the solid NH4SH decomposed to NH3 and H2S as gases. The Kp of the reaction at 327^∘C is (R=0⋅082 atm mol^−1K^−1, Molar mass of S = 32 g mol^-1, molar mass of N = 14 g mol^−1) 5⋅1g NH4SH is introduced in [...]
Consider the reaction, N2(g)+3H2(g)↽−−⇀2NH3(g) The equilibrium constant of the above reaction is KP. If pure ammonia is left to dissociate, the partial pressure of ammonia at equilibrium is given by (Assume that PNH3 < < P total at equilibrium)
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Nov
Consider the reaction, N2(g)+3H2(g)↽−−⇀2NH3(g) The equilibrium constant of the above reaction is KP. If pure ammonia is left to dissociate, the partial pressure of ammonia at equilibrium is given by (Assume that PNH3 < < P total at equilibrium) Consider the reaction N2(g)+3H2(g)↽−−⇀2NH3(g) The equilibrium constant of the above reaction is KP. If pure ammonia [...]
Two solids dissociate as follows A(s)↽−−⇀B(g) + C(g);Kp1 = x atm^2 D(s)↽−−⇀C(g) + E(g);Kp2 = y atm^2 The total pressure when both the solids dissociate simultaneously is :-
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Nov
Two solids dissociate as follows A(s)↽−−⇀B(g) + C(g);Kp1 = x atm^2 D(s)↽−−⇀C(g) + E(g);Kp2 = y atm^2 The total pressure when both the solids dissociate simultaneously is :- Two solids dissociate as follows A(s)↽−−⇀B(g) + C(g);Kp1 = x atm^2 D(s)↽−−⇀C(g) + E(g);Kp2 = y atm^2 The total pressure when both the solids dissociate simultaneously is [...]