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Standard XII

Chemistry

Equilibrium Constant and Standard Free Energy Change

The standard ...

Question

The standard heats of formation of NO $_{2}$ (g) and N $_{2}$ O $_{4}$ (g) are 33.5 and 8.4 KJ mol $^{- 1}$ respectively.
The heat of dimerisation of NO $_{2}$ in KJ is:

41.9

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-25.1

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-52.2

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-58.6

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Solution

The correct option is A -58.6
$2 N O_{2} \to N_{2} O_{4}$
$Δ H$ = $Δ H_{P r o d u c t s} - Δ H_{r e a c t a n t s}$ = $8.4 - 2 \times 33.5$
= $8.4 - 67$

$=$ - 58.6 KJ mol $^{- 1}$

Option D is correct.

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Similar questions

The standard heats of formation in K.cal mol $^{- 1}$ of NO $_{2 (g)}$ and N $_{2}$ O $_{4 (g)}$ are 8.0 and 2.0 respectively. The heat of dimerisation of $N O_{2}$ in K.cal is $2 N O_{2 (g)} \to N_{2} O_{4 (g)}$

Q. The standard enthalpy of formation of

N_{2} O

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respectively. The enthalpy change of the reaction,

2 N_{2} O (g) + O_{2} (g) \to 4 N O (g)

is equal to:

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C C l_{4} (l), H_{2} O (g), C O_{2} (g) a n d H C l (g)

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The molar heat of formation of $N H_{4} N O_{3} (s)$ is $- 367.5 K J$ and those of $N_{2} O (g)$ and $H_{2} O (l)$ are $+ 81.46 K J$ and $- 285.78 K J$ respectively at $25^{o} C$ and 1 atmospheric pressure. The $△$ U for the reaction
$N H_{4} N O_{3} (s) \to N_{2} O (g) + 2 H_{2} O (l)$

Q. For the reaction:

4 N H_{3} (g) + 3 O_{2} (g) \to 2 N_{2} (g) + 6 H_{2} O (l)

298 K

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The standard heats of formation of NO2 (g) and N2O4 (g) are 33.5 and 8.4 KJ mol−1 respectively.The heat of dimerisation of NO2 in KJ is:

The correct option is A -58.62NO2→N2O4ΔH =ΔHProducts−ΔHreactants= 8.4−2×33.5= 8.4−67= - 58.6 KJ mol−1Option D is correct.

The standard heats of formation of NO $_{2}$ (g) and N $_{2}$ O $_{4}$ (g) are 33.5 and 8.4 KJ mol $^{- 1}$ respectively.
The heat of dimerisation of NO $_{2}$ in KJ is:

The correct option is A -58.6
$2 N O_{2} \to N_{2} O_{4}$
$Δ H$ = $Δ H_{P r o d u c t s} - Δ H_{r e a c t a n t s}$ = $8.4 - 2 \times 33.5$
= $8.4 - 67$

$=$ - 58.6 KJ mol $^{- 1}$

Option D is correct.