Potassium metal is commercially prepared by the reduction of molten KCl with metallic sodium at $850^{\circ}$ C. This method is based upon the following principal.

Sodium is more reactive than potassium at this temperature.

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Potassium, being volatile, distills off thus shifting the reaction forward.

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Sodium prefers to bind to chloride ions in preferance to potassium ions.

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Potassium and sodium form an alloy at this temperature.

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Solution

The correct option is C Sodium prefers to bind to chloride ions in preferance to potassium ions.
As sodium prefers to bind to chloride ions in preferance to potassium ions due to higher affinity energy with chlorine gas.

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Potassium metal is commercially prepared by the reduction of molten KCl with metallic sodium is $850^{0}$ C (1123K). This method is based upon the following principle

Q. Assertion :Sodium reacts with oxygen to form

N a_{2} O_{2}

but postassium reacts with oxygen to form

K O_{2}

. Reason: Potassium is more reactive metal than sodium.

Q. Give reasons for the following:
(i) Sodium is more reactive than aluminium.
(ii) Mercury is not the only metallic liquid at around 30 C.
(iii) Metals always combine by electrovalency.
(iv) Metal ions are always positively charged.
(v) Metal ions always get discharged at the cathode during electrolysis.
(vi) Metals generally do not form hydrides.
(vii) Metals are always monoatomic.
(viii) Sodium and potassium cannot be kept exposed to air.
(ix) Sodium and potassium should not be treated with acids.
(x) Hydrogen is not a metal but it has been assigned a place in the reactivity series of metals.

The aqueous solution of one of the following salts will turn red litmus to blue. This salt is :

(a) potassium sulphate

(b) sodium sulphate

(d) potassium carbonate

Q. State as to why:
(a) a solution of

N a_{2} C O_{3}

is alkaline ?
(b) alkali metals are prepared by electrolysis of their fused chlorides ?
(c) sodium is found to be more useful than potassium ?

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Potassium metal is commercially prepared by the reduction of molten KCl with metallic sodium at 850∘ C. This method is based upon the following principal.

The correct option is C Sodium prefers to bind to chloride ions in preferance to potassium ions.As sodium prefers to bind to chloride ions in preferance to potassium ions due to higher affinity energy with chlorine gas.

Potassium metal is commercially prepared by the reduction of molten KCl with metallic sodium at $850^{\circ}$ C. This method is based upon the following principal.

The correct option is C Sodium prefers to bind to chloride ions in preferance to potassium ions.
As sodium prefers to bind to chloride ions in preferance to potassium ions due to higher affinity energy with chlorine gas.