(a) Which poisonous gas is evolved when white phosphorus is heated with $c o n c . N a O H$ solution? Write the chemical equation involved.
(b) Which noble gas has the lowest boiling point?
(c) Fluorine is a stronger oxidizing agent than chlorine. Why?
(d) What happens when $H_{3} P O_{3}$ is heated?
(e) Complete the equation :
$P b S + O_{3} \to$

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Solution

(a) Phosphine

$P_{4} (s) + 3 N a O H (a q) + 3 H_{2} O (l) \to 3 N a H_{2} P O_{2} (a q) Sodium hypophosphite + P H_{3} (g) Phosphine ↑$

(b) Helium

(c) The electrode potential of $F_{2}$ and $C l_{2}$ are:
$F_{2} + 2 e^{-} \to 2 F^{-}; E^{\circ} = + 2.87 V$
$C l_{2} + 2 e^{-} \to 2 C l^{-}; E^{\circ} = 1.36 V$
Since $E^{\circ}$ for $F_{2} / F^{-}$ is higher than that of $C l_{2} / C l^{-}$ , therefore, $F_{2}$ is more easily reduced than $C l_{2}$ . As a result, $F_{2}$ is stronger oxidising agent than $C l_{2}$ .

(d) It undergoes disproportionation to form $P H_{3}$ and $H_{3} P O_{4}$ .
$4 H_{3} P O_{3} Δ - \to P H_{3} Phosphine + 3 H_{3} P O_{4} Orthophosphoric acid$
$(e) P b S + 4 O_{3} \to P b S O_{4} + 4 O_{2}$

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Similar questions

c o n c . N a O H

H_{3} P O_{3}

P b S + O_{3} \to

(a) Account for the following:

(i) Interhalogens are more reactive than pure halogens.

(ii) $N_{2}$ is less reactive at room temperature.

(iii) Reducing character increases from $N H_{3} t o B i H_{3}$ .

(b) Draw the structures of the following:

(i) $H_{4} P_{2} O_{7}$ (Pyrophosphoric acid)

(ii) $X e F_{4}$

(a) Which poisonous gas is evolved when white phosphorus is heated with conc. NaOH solution? Write the chemical equation involved.

(b) Which noble gas has the lowest boiling point?

(d) What happens when $H_{3} P O_{3}$ is heated?

(e) Complete the equation:

$P b S + O_{3} \to$

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