Advertisements
Advertisements
प्रश्न
Write the expression for the equilibrium constant, Kc for the following reactions:
\[\ce{CH3COOC2H5(aq) + H2O(l) ⇌CH3COOH (aq) + C2H5OH (aq)}\]
Advertisements
उत्तर
`"K"_"c" = (["CH"_3"COOH"_(("aq"))]["C"_2"H"_5"OH"_(("aq"))])/(["CH"_3"COOC"_2"H"_(5("aq"))]["H"_2"O"_((l))])`
`= (["CH"_3"COOH"_(("aq"))]["C"_2"H"_2"OH"_(("aq"))])/["CH"_3"COOC"_2"H"_(5("aq"))]`
APPEARS IN
संबंधित प्रश्न
What is Kc for the following equilibrium when the equilibrium concentration of each substance is: [SO2] = 0.60 M, [O2] = 0.82 M and [SO3] = 1.90 M?
\[\ce{2SO2(g) + O2(g) ⇌ 2SO3(g)}\]
Write the expression for the equilibrium constant, Kc for following reactions:
\[\ce{Fe^{3+}(aq) + 3OH^-(aq) ⇌ Fe(OH)3(s)}\]
Write the expression for the equilibrium constant, Kc for the following reactions
\[\ce{I2 (s) + 5F2 ⇌ 2IF5}\]
Nitric oxide reacts with Br2 and gives nitrosyl bromide as per reaction given below:
\[\ce{2NO(g) + Br2 (g) ⇌ 2NOBr (g)}\]
When 0.087 mol of NO and 0.0437 mol of Br2 are mixed in a closed container at the constant temperature, 0.0518 mol of NOBr is obtained at equilibrium. Calculate the equilibrium amount of NO and Br2.
What is the equilibrium concentration of each of the substances in the equilibrium when the initial concentration of ICl was 0.78 M?
\[\ce{2 ICl(g) ⇌ I2(g) + Cl2(g)}\]; KC = 0.14
Kp = 0.04 atm at 899 K for the equilibrium shown below. What is the equilibrium concentration of C2H6 when it is placed in a flask at 4.0 atm pressure and allowed to come to equilibrium?
\[\ce{C2H6 (g) ⇌ C2H4 (g) + H2 (g)}\]
Calculate a) ΔG°and b) the equilibrium constant for the formation of NO2 from NO and O2 at 298 K
\[\ce{NO(g) + 1/2 O_2 (g) <=> NO_2(g)}\]
where ΔfG⊝ (NO2) = 52.0 kJ/mol
ΔfG⊝ (NO) = 87.0 kJ/mol
ΔfG⊝ (O2) = 0 kJ/mol
Predict which of the following reaction will have the appreciable concentration of reactants and products:
- \[\ce{Cl2 (g) ⇌ 2Cl (g)}\] Kc = 5 ×10–39
- \[\ce{Cl2 (g) + 2NO (g) ⇌ 2NOCl (g)}\] Kc = 3.7 × 108
- \[\ce{Cl2 (g) + 2NO2 (g) ⇌ 2NO2Cl (g)}\] Kc = 1.8
The value of Kc for the reaction 3O2 (g) ↔ 2O3 (g) is 2.0 ×10–50 at 25°C. If the equilibrium concentration of O2 in the air at 25°C is 1.6 ×10–2, what is the concentration of O3?
For the reaction \[\ce{H2 (g) + I2 (g) ⇌ 2HI (g)}\], the standard free energy is ∆GΘ > 0. The equilibrium constant (K ) would be ______.
At 500 K, equilibrium constant, \[\ce{K_c}\], for the following reaction is 5.
\[\ce{1/2 H2 (g) + 1/2 I2 (g) ⇌ HI (g)}\]
What would be the equilibrium constant \[\ce{K_c}\] for the reaction
\[\ce{2HI (g) ⇌ H2 (g) + I2 (g)}\]
Match standard free energy of the reaction with the corresponding equilibrium constant.
| Column I | Column II |
| (i) ∆GΘ > 0 | (a) K > 1 |
| (ii) ∆GΘ > 0 | (b) K = 1 |
| (iii) ∆GΘ = 0 | (c) K = 0 |
| (d) K < 1 |
For the reaction,
\[\ce{N2 + O2(g) ⇌ 2NO(g)}\]
the equilibrium constant is K1. The equilibrium constant is K2 for the reaction
\[\ce{2NO(g) + O2(g) ⇌ 2NO2(g)}\]
What is "K" for the reaction:
\[\ce{NO2(g) ⇌ 1/2 N2(g) + O2(g)}\]?
For the reaction \[\ce{A(g) <=> B(g)}\] at 495 K, ΔG° = −9.478 kJ mol−1
If we start the reaction in a closed container at 495 K with 22 millimoles of A, the amount of B in the equilibrium mixture is ______ millimoles. (Round off to the Nearest Integer).
[R = 8.314 J mol−1 K−1; ln 10 = 2.303]
For which of the following Kp is less than Kc?
The equilibrium constant for the reaction is ______ × 1026.
\[\ce{Fe + CuSO4 <=> FeSO4 + Cu}\] at 25°C.
Given `"E"_("Fe"//"Fe"^(2+))^0` = 0.44 V
`"E"_("Cu"//"Cu"^(2+))^0` = - 0.337 V
In which of the following equilibria, Kp and Kc are not equal?
