Initially 1.4 moles of NH
(g) is introduced into a sealed 2.0 dm
reaction vessel. The ammonia decomposes when the temperature is increased to 600K and reaches equilibrium as follows:
When the equilibrium mixture is analysed, the concentration of NH
(g) is 0.3 mol
dm
Calculate the concentration of N
(g) and H
(g) in the equilibrium mixture.
Calculate the equilibrium constant for the reaction at 900 K.
Therefore,
Moles used up = 1.4 - 0.6 = 0.8 moles
Remember to use the mole ratio of reactants to products to do this. In this case, the ratio of NH
:N
:H
= 2:1:3. Therefore, if 0.8 moles of ammonia are used up in the reaction, then 0.4 moles of nitrogen are produced and 1.2 moles of hydrogen are produced.
Hydrogen and iodine gas react according to the following equation:
When 0.496 mol
and 0.181 mol
are heated at
C in a 1 dm
container, the equilibrium mixture is found to contain 0.00749 mol
. Calculate the equilibrium constant for the reaction at
C.
Moles of iodine used = 0.181 - 0.00749 = 0.1735 mol
The mole ratio of hydrogen:iodine = 1:1, therefore 0.1735 moles of hydrogen must also be used up in the reaction.
The mole ratio of H
:I
:HI = 1:1:2, therefore the number of moles of HI produced is 0.1735
2 = 0.347 mol.
So far, the table can be filled in as follows:
H
(g)
I
2HI
Start of reaction
0.496
0.181
0
Used up
0.1735
0.1735
0
Produced
0
0
0.347
Equilibrium
0.3225
0.0075
0.347
Therefore the equilibrium concentrations are as follows:
Write the equilibrium constant expression, K
for the following reactions:
The following reaction takes place:
K
for the reaction is 7.5
10
mol.dm
. At equilibrium, the concentration of FeCl
is 0.95
10
mol.dm
and the concentration of free iron (Fe
) is 0.2 mol.dm
. Calculate the concentration of chloride ions at equilibrium.
Ethanoic acid (CH
COOH) reacts with ethanol (CH
CH
OH) to produce ethyl ethanoate and water. The reaction is:
At the beginning of the reaction, there are 0.5 mols of ethanoic acid and 0.5 mols of ethanol. At equilibrium, 0.3 mols of ethanoic acid was left unreacted. The volume of the reaction container is 2 dm
. Calculate the value of K
.
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