In: Chemistry
The equilibrium constant, Kc, for the following reaction
is 6.50×10-3 at
298K.
2NOBr(g)<====>
2NO(g) +
Br2(g)
If an equilibrium mixture of the three gases in a
16.4 L container at 298K contains
0.383 mol of NOBr(g) and
0.230 mol of NO, the equilibrium
concentration of Br2 is____M
The equilibrium constant, Kc , for the following
reaction is 7.00×10-5 at
673 K.
NH4I(s)
<====>NH3(g) +
HI(g)
If an equilibrium mixture of the three compounds in a
5.04 L container at 673 K
contains 2.25 mol of
NH4I(s) and 0.339 mol
of NH3, the number of moles of
HI present is _____M
Consider the following reaction:
2NOBr(g)
<=======>2NO(g) +
Br2(g)
If 0.325 moles of NOBr(g),
0.405 moles of NO, and
0.613 moles of Br2 are
at equilibrium in a 15.0 L container at
531 K, the value of the equilibrium constant,
Kc, is ____m
1.
The given reaction is
For a generic reaction , the equilibrium constant Kc is expressed as
Where the concentrations are equilibrium values.
Hence, for our reaction, the expression of Kc can be written as
It is given that volume of the container = 16.4 L
We can calculate the equilibrium concentration of given species from their number of moles as follows:
Hence, putting in the values in equilibrium expression, we can calculate the equilibrium concentration of Br2.
Hence, the equilibrium concentration of Br2 is 0.0180 M approximately. (Rounded to three significant figures).
2.
The given equilibrium is
The equilibrium constant Kc of the reaction can be written as
Note that NH4I is a solid and its concentration is taken as unity. Hence, it does not appear in the equilibrium constant expression.
Volume of the container = 5.04 L
Hence, we can calculate the concentration of NH3 at equilibrium as follows:
Hence, we can calculate the concentration of HI as follows:
Hence, the number of moles of HI can be calculated as
Hence, the number of moles of HI present is ( Rounded to three significant figures).
3.
The given reaction is
The equilibrium expression can be written as
Volume of the container = 15.0 L
Hence, we can calculate the concentrations at equilibrium from the number of moles as follows;
Now, we can calculate the equilibrium constant Kc as follows:
Hence, the value of equilibrium constant Kc is . (Rounded to three significant figures).