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Aluminium Chloride

Which of the ...

Question

Which of the following chemical reaction correctly shows Aqua-regia dissolving in gold?

A

A u + 2 [C l] ⟶ A u C l_{2} H C l ⟶ H_{2} [A u C l_{4}]

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B

A g + 3 [C l] ⟶ A g C l_{3} H C l ⟶ H [A g C l_{4}]

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C

A u + 3 [C l] ⟶ A u C l_{3} H C l ⟶ H [A u C l_{4}]

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D

A g + 2 [C l] ⟶ A g C l_{2} H C l ⟶ H_{2} [A g C l_{4}]

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Solution

The correct option is C $A u + 3 [C l] ⟶ A u C l_{3} H C l ⟶ H [A u C l_{4}]$
Aqua regia is a mixture of nitric acid and hydrochloric acid, optimally in a molar ratio of 1:3. Aqua regia is a yellow-orange fuming liquid. It can dissolve the noble metals gold and platinum.
$A u + 3 [C l] ⟶ A u C l_{3} H C l ⟶ H [A u C l_{4}]$

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Similar questions

Q. In which of the following reactions, chlorine acts as an oxidising agent?
(i)

C H_{3} C H_{2} O H + {C l}_{2} ⟶ C H_{3} C H O + H C l

C H_{3} C H O + {C l}_{2} ⟶ C {C l}_{3} C H O + H C l

C H_{4} + {C l}_{2} ⟶ C H_{3} C l + H C l

Balance the following below equation.

A u + {N O}_{3}^{-} + C l^{-} + H^{+} \to {A u C l}_{4}^{-} + N O_{2} + H_{2} O

Q. Consider the reaction :

C l_{2} (a q) + H_{2} S (a q) \to S (s) + 2 H^{+} (a q) + 2 C l^{-} (a q)

The rate equation for this reaction is

= k [C l_{2}] [H_{2} S]

Which of these mechanisms

i s / a r e

consistent with this rate equation?
(A)

C l_{2} + H_{2} S \to H^{+} + C l^{-} + C l^{+} + H S^{-}

C l^{+} + H S^{-} \to H^{+} + C l^{-} + S

H_{2} S \Leftrightarrow H^{+} + H S^{-}

(fast equilibrium)

C l_{2} + H S^{-} \to 2 C l^{-} + H^{+} + S

Q. Heat evolved in the reaction

H_{2} + {C l}_{2} \to 2 H C l

182 k J

( Bond energies

H - H = 430 k J / m o l e, C l - C l - 242 k J / m o l e

H - C l

bond energy is:

Q. Consider the reaction:

{C l}_{2} (a q .) + H_{2} S (a q .) ⟶ S (s) + 2 H^{+} (a q .) + 2 {C l}^{-} (a q .)

The rate equation for this reaction is:
Rate

= k [{C l}_{2}] [H_{2} S]

Which of these mechanisms is/are consistent with this rate equation?

A

{C l}_{2} + H_{2} S ⟶ H^{+} + {C l}^{-} + {C l}^{+} + H S^{-}

{C l}^{+} + H S^{-} ⟶ H^{+} + {C l}^{-} + S

B

H_{2} S ⇌ H^{+} + H S^{-}

(fast equilibrium)

{C l}_{2} + H S^{-} ⟶ 2 {C l}^{-} + H^{+} + S

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