Advertisements
Advertisements
Question
The equilibrium for the dissociation of XY2 is given as,
\[\ce{2 XY2 (g) <=> 2 XY (g) + Y2 (g)}\]
if the degree of dissociation x is so small compared to one. Show that 2 Kp = PX3 where P is the total pressure and Kp is the dissociation equilibrium constant of XY2.
Solution
\[\ce{2 XY2 (g) <=> 2 XY (g) + Y2 (g)}\]
| XY2 | XY | Y2 | |
| Initial no. of. moles | 1 | - | - |
| No. of. moles dissociated | x | - | - |
| No. of. moles at equilibrium | (1 - x) 1 | x | `"x"/2` |
Total no. of moles = `1 - x + x + x/2 = 1 + x/2 ≅ 1`
[∵ Given that x << 1; 1 - x ≅ 1 and 1 + `x/2` ≅ 1]
`"K"_"p" = (["P"_"xy"]^2["P"_("Y"_2)])/["P"_("XY"_2)]^2`
`= ((x/1 xx "P")^2((x//2)/1 xx "P"))/(1/1 xx "P")^2`
`"K"_"P" = (x^2"P"^2 xx "P")/(2"P"^2)`; 2Kp = x3P
APPEARS IN
RELATED QUESTIONS
K1 and K2 are the equilibrium constants for the reactions respectively.
\[\ce{N2(g) + O2(g) <=>[K1] 2NO(g)}\]
\[\ce{NO(g) + O2(g) <=>[K2] 2NO2(g)}\]
What is the equilibrium constant for the reaction \[\ce{NO2(g) <=> 1/2 N2(g) + O2(g)}\]
`"K"_"C"/"K"_"P"` for the reaction,
\[\ce{N2(g) + 3H2(g) <=> 2NH3(g)}\] is
In which of the following equilibrium, Kp and Kc are not equal?
The equilibrium constants of the following reactions are:
\[\ce{N2 + 3H2 <=> 2NH3}\]; K1
\[\ce{N2 + O2 <=> 2NO}\]; K2
\[\ce{H2 + 1/2O2 <=> H2O}\]; K3
The equilibrium constant (K) for the reaction;
\[\ce{2NH3 + 5/2 O2 <=> 2NO + 3H2O}\], will be
For a given reaction at a particular temperature, the equilibrium constant has a constant value. Is the value of Q also constant? Explain.
For the reaction, \[\ce{A2(g) + B2(g) <=> 2AB(g); \Delta H}\] is -ve.
the following molecular scenes represent differenr reaction mixture. (A-green, B-blue)
| Closed ← |
 |
 |
 |
| System | At equilibrium | (x) | (y) |
- Calculate the equilibrium constant Kp and (Kc).
- For the reaction mixture represented by scene (x), (y) the reaction proceed in which directions?
- What is the effect of an increase in pressure for the mixture at equilibrium?
Write the balanced chemical equation for an equilibrium reaction for which the equilibrium constant is given by expression.
`"K"_"C" = (["NH"_3]^4["O"_2]^5)/(["NO"]^4["H"_2"O"]^6)`
Derive the relation between Kp and Kc.
For the reaction
\[\ce{SrCO3(s) <=> SrO(s) + CO2(g)}\]
the value of equilibrium constant Kp = 2.2 × 10-4 at 1002 K. Calculate Kc for the reaction.
To study the decomposition of hydrogen iodide, a student fills an evacuated 3 litre flask with 0.3 mol of HI gas and allows the reaction to proceed at 500°C. At equilibrium he found the concentration of HI which is equal to 0.05 M. Calculate Kc and Kp.
