Equilibrium Chemistry Worksheet Page 2
ADVERTISEMENT
1
2
3
4
5
62.
Convert K, based on concentration, to K
, based on partial pressures.
P
The term Δn means the number of moles of gas in the products minus the
number of moles of gas in the reactants. If Δn = 0, K = K
.
P
Δn =
Δn
K
= K(RT)
=
P
3.
Calculate the partial pressures of N
, H
and NH
assuming a 10.0 L
2
2
3
o
volume, at 250
C.
a)
First calculate the moles of each gas present at equilibrium.
mol N
=
2
mol H
=
2
mol NH
=
3
b)
Now find the total pressure, using the ideal gas law.
P
= _______
tot
c)
Find the partial pressures of each of the gases using their mol
fractions:
P
= (mol N
/mol total) x P
= _____
N2
2
tot
P
= (mol H
/mol total) x P
= _____
H2
2
tot
P
= (mol NH
/mol total) x P
= _____
NH3
3
tot
4.
Calculate K
using these values. Is it the same as your previous answer,
P
calculated from K in question 2?
p
K
= P
=
P
prod
r
P
react
ADVERTISEMENT
0 votes
Related Articles
Related forms
Related Categories
Parent category: Education