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Heat of Reaction

Consider the ...

Question

Consider the reaction at $300 K$ , $H_{2} (g) + C l_{2} (g) \to 2 H C l (g), Δ H^{\circ} = - 185 k J$
If $3$ mole of $H_{2}$ completely reacts with $3$ mole of $C l_{2}$ to form $H C l$ , What is $Δ U^{\circ}$ for this reaction?

A

0

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B

- 185 k J

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C

555 k J

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D

None of these

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Solution

The correct option is A $- 185 k J$
$\begin{matrix} H_{3}^{+} C l_{2} \to 2 H C L, Δ H^{\circ} = - 18 k J 1 m o l 1 m o l 2 m o l 3 m o l 3 m o l 6 m o l Δ n g = 0 Δ H^{\circ} = Δ U^{6} \Rightarrow Δ U^{6} = Δ H^{\circ} = - 185 K J . H e n c e, t h e o p t i o n B i s t h e c o r r e c t a n s w e r . \end{matrix}$

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Similar questions

Q. Consider the reaction at

300 K

H_{2} (g) + {C l}_{2} (g) \to 2 H C l (g)

Δ H^{o} = - 185 k J / m o l

3

H_{2}

completely react with

3

{C l}_{2}

H C l

Δ U^{o}

for this process?

Q. Consider the reaction at 300 K,

H_{2} (g) + C l_{2} (g) \to 2 H C l (g); Δ H = - 185 k J / m o l

Δ U

H_{2}

completely reacts with 3 mole of

C l_{2}

H C l

Q. Consider the reaction at

300

H_{2} (g) + C l_{2} (g) \to 2 H C l (g);

Δ H^{o} = - 185

2

H_{2}

completely react with

2

C l_{2}

to form HCl. What is

Δ U^{o}

for the reaction?

H_{2} (g) + C l_{2} (g) ⟶ 2 H C l (g) + 185 k J

. This reaction is exothermic. Reason: Heat is being evolved.

H_{2} (g) + C l_{2} (g) = 2 H C l (g)

;

Δ H

= - 22.06

kcal. For this reaction,

Δ U

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