Advertisements
Advertisements
प्रश्न
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
Advertisements
उत्तर
The given reaction is:
| 2 ICl(g) | ⇌ | I2(g) | + | Cl2(g) | |
| Initial conc. | 0.78 M | 0 | 0 | ||
| At equilibrium | (0.78 - 2x) M | x M | x M |
Now we can write, `(["I"_2]["Cl"_2])/["ICl"]^2 = "K"_"C"`
`=> (x xx x)/(0.78 - 2x)^2 = 0.14`
`=> x^2/(0.78 - 2x)^2` = 0.14
`=> x/(0.78 - 2x) = 0.374`
`=> x= 0.292 - 0.748 x`
`=> 1.748 x = 0.292`
⇒ x = 0.167
Hence, at equilibrium,
[ICl] = [I2] = 0.167 M[ICl]
= (0.78 - 2 × 0.167)M
= 0.446 M
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 each of the following reactions:
\[\ce{2NOCl (g) ⇌ 2NO (g) + Cl2 (g)}\]
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
\[\ce{I2 (s) + 5F2 ⇌ 2IF5}\]
A reaction between N2 and O2 takes place as follows:
\[\ce{2N2 (g) + O2 (g) ⇌ 2N2O (g)}\]
If a mixture of 0.482 mol of N2 and 0.933 mol of O2 is placed in a 10 L reaction vessel and allowed to form N2O at a temperature for which Kc = 2.0 × 10-37, determine the composition of equilibrium mixture.
At 700 K, the equilibrium constant for the reaction
\[\ce{H_{2(g)} + I_{2(g)} ↔ 2HI_{(g)}}\]
is 54.8. If 0.5 molL–1 of HI(g) is present at equilibrium at 700 K, what are the concentration of H2(g) and I2(g) assuming that we initially started with HI(g) and allowed it to reach equilibrium at 700 K?
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
The reaction, \[\ce{CO(g) + 3H2(g) ↔ CH4(g) + H2O(g)}\] is at equilibrium at 1300 K in a 1L flask. It also contains 0.30 mol of CO, 0.10 mol of H2 and 0.02 mol of H2O and an unknown amount of CH4 in the flask. Determine the concentration of CH4 in the mixture. The equilibrium constant, Kc for the reaction at the given temperature is 3.90.
For the reaction : \[\ce{N2 (g) + 3H2 (g) ⇌ 2NH3 (g)}\]
Equilibrium constant `K_C = ([NH3]^2)/([N_2][H_2]^3)`
Some reactions are written below in Column I and their equilibrium constants in terms of Kc are written in Column II. Match the following reactions with the corresponding equilibrium constant
| Column I (Reaction) | Column II (Equilibrium constant) |
| (i) \[\ce{2N2 (g) + 6H2 (g) ⇌ 4NH3 (g)}\] | (a) `2K_c` |
| (ii) \[\ce{2NH3 (g) ⇌ N2 (g) + 3H2 (g)}\] | (b) `K_c^(1/2)` |
| (iii) \[\ce{1/2 N2 (g) + 3/2 H2 (g) ⇌ NH3 (g)}\] | (c) `1/K_c` |
| (d) `K_c^2` |
The stepwise formation of [Cu(NH3)4]2+ is given below:
\[\ce{Cu^{2+} + NH3 <=>[K1] [Cu(NH3)]^{2+}}\]
\[\ce{[Cu(NH3)]^{2+} + NH3 <=>[K2] [Cu(NH3)2]^{2+}}\]
\[\ce{[Cu(NH3)2]^{2+} + NH3 <=>[K3] [Cu(NH3)3]^{2+}}\]
\[\ce{[Cu(NH3)3]^{2+} + NH3 <=>[K4] [Cu(NH3)4]^{2+}}\]
The value of stability constants K1, K2, K3 and K4 are 104, 1.58 × 102, 5 × 103 and 102 respectively. The overall equilibrium constant for dissociation of [Cu(NH3)4]2+ is x × 10−12. The value of x is ______. (Rounded-off to the nearest integer)
At 1990 K and 1 atm pressure, there are equal numbers of Cl2 molecules and Cl atoms in the reaction mixture. The value of Kp for the reaction Cl2(g) ⇌ 2Cl(g) under the above conditions is x × 10−1. The value of x is ______. (Rounded-off to the nearest integer)
An equilibrium system for the reaction between hydrogen and iodine to give hydrogen iodide at 765 K in a 5 litre volume contains 0.4 mole of hydrogen, 0.4 mole of iodine and 2.4 moles of hydrogen iodide.
\[\ce{H2 + I2 <=> 2HI}\]
The equilibrium constant for the reaction is:
Sulphide ion in alkaline solution reacts with solid sulphur to form polysulphide ions having formula, \[\ce{S^{2-}2}\], \[\ce{S^{2-}3}\], \[\ce{S^{2-}4}\], etc. if K1 = 12 for \[\ce{S + S^{2-} <=> S^{2-}2}\] and K2 = 132 for \[\ce{2S + S^{2-} <=> S^{2-}3}\], K3 = ______ for \[\ce{S + S^{2-}2 <=> S^{2-}3}\].
The decomposition of N2O4 to NO2 was carried out in chloroform at 280°C. At equilibrium, 0.2 mol of N2O4 and 2 × 10−3 mol of NO2 were present in 2 ℓ of the solution. The equilibrium constant for the reaction \[\ce{N2O4 <=> 2NO2}\] is ______.
In which one of the following equilibria, KP ≠ Kc?
