(a)i. State two conditions used in the Haber process
ii. Explain briefly the effect of increasing the pressure on the rate of reaction in the Haber process.
(b)i. A mixture of nitrogen(IV) oxide and oxygen is bubbled into warm water to produce
trioxonitrate(V) oxide, write a balanced chemical equation for the reaction.
ii. Using a balanced chemical equation only, explain what would happen if nitrogen(IV) oxide is bubbled into warm water.
iii.
Compare the gases evolved when trioxonitrate(V) acid decomposes under each of the following properties:
i. pH
ii. Solubility in water
iii. Reaction with carbon(II) oxide
(c)i. Name two oxides of sulphur
ii. Write a balanced equation for the reaction between each of the named oxides(Sulphur(IV) oxide, Sulphur (VI) oxide) and water
(d)i. Name one calcium compound
a, Used to dry ammonia gas
b. Used in the manufacture of cement
c. That causes hardness in water
d. Name one calcium compound
(a)i. Temperature: 350-5000C/high temperature
Pressure: 150-1000 atm/high pressure
Catalyst: (Finely divided) Iron
ii. Rate of the reaction increases as particles are closer together/more particles per unit volume. There are more collisions per seconds/collisions are more often
(b)i. 4NO2 + O2 + 2H2O -----> 4HNO3
ii. 2NO2 + 2H2O -----> HNO3 + HNO2
A misture of two acids will be produced
iii. 4HNO3(aq) → 4NO2 + O2 + 2H2O
i. - Oxygen is neutral while NO2 is acidic
ii. - NO2 is soluble while O2 is sparingly soluble in water
iii. - O2 reacts with CO to form CO2 while NO2 reacts with CO to form a mixture of N2 and CO2
(c)i. Sulphur(IV) oxide
Sulphur (VI) oxide
ii. SO2(g) + H2O(l) ---->H2SO3(aq)
SO3(g) + H2O(l) ---->H2SO4(aq)
(d)i. - calcium oxide
- quick lime
b. - Limestone
- Quick lime
- Calcium trioxocarbonat(IV)
- Calcium oxide
c. - Calcium chloride
- Calcium tetraoxosulphate (VI)
- Calcium hydrogen trioxocarbonate (IV)
d. Calcium tetraoxosulphate (VI) (dihydrate)
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