Occurrence Of Metals

Step 1: Understanding Salt Preparation:
Soluble salts can be made by reacting an acid with a metal, base, or carbonate. However, the "Metal + Acid" method only works for metals more reactive than hydrogen.

Step 2: Checking Copper's Reactivity:
As established in question (vii), Copper is below hydrogen in the reactivity series. This means it cannot displace hydrogen from dilute acids like (HCl) or (H_2SO_4).

Step 3: Evaluating Alternatives:
Copper salts can be prepared by reacting Copper oxide (a base) or Copper carbonate with dilute acids, as these are neutralization/decomposition reactions that do not require hydrogen displacement.

Step 4: Final Answer:
Method 3 (Action of dilute acid on metals) cannot be used for copper.

Reactant A: Concentrated Sulphuric Acid (H_2SO_4) at 170°C. It acts as a dehydrating agent to convert ethanol into ethene.

Reactant B: Acetic Acid (CH_3COOH). Ethanol is oxidized to acetic acid, which then reacts with more ethanol (in the presence of an acid catalyst) to form Ethyl acetate (esterification).

Reactant C: Oxygen (O_2) or an Oxidizing agent. This facilitates the conversion of Ethanol to B (Acetic acid) or the combustion of Ethanol/Ethene to CO_2 and water.

(a) Lead (II) carbonate: (Prepared via double decomposition/precipitation) [ Pb(NO_3)_2 + Na_2CO_3 PbCO_3downarrow + 2NaNO_3 ]

(b) Copper (II) chloride: (Prepared via action of acid on a carbonate) [ CuCO_3 + 2HCl CuCl_2 + H_2O + CO_2uparrow ] (c) Iron (II) chloride: (Prepared via direct synthesis/combination) [ Fe + 2HCl FeCl_2 + H_2uparrow ] Note: Iron reacting with dry Chlorine would produce Iron (III) chloride, so dilute HCl is used for the (II) state.

(a) Reason for temperature < 200°C:
Maintaining the temperature below 200°C is important for several reasons:
1. It prevents the formation of a hard crust of sodium sulphate (Na2SO4), which is difficult to remove from the glass retort.
2. It prevents the thermal decomposition of the product, nitric acid (HNO3).
3. It saves fuel and prevents the glass apparatus from cracking.

(b) Use of concentrated sulphuric acid:
Concentrated sulphuric acid is used because it is a non-volatile acid. It can displace the more volatile nitric acid from its salt (sodium nitrate) when heated.

(a) Name the process:
The industrial manufacture of ammonia is known as the Haber Process.

(b) Which catalyst is used in the above process?
The catalyst used is Finely divided Iron (Fe).
Note: Molybdenum is often used as a promoter to enhance the efficiency of this catalyst.

(c) In the above diagrammatic setup, how is ammonia gas separated from the unreacted gases to obtain liquid ammonia?
Ammonia gas is separated by the process of liquefaction. Because ammonia has a higher boiling point and is more easily liquefied under pressure than nitrogen or hydrogen, it is condensed into a liquid in a cooling chamber while the unreacted gases are pumped back into the catalytic chamber.

(d) Which two properties of ammonia gas can be demonstrated by the Fountain Experiment?
The two properties demonstrated are: beginenumerate High solubility of ammonia gas in water. Basic (alkaline) nature of the gas. endenumerate