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Heat of Reaction

Given:[[ H 2 ...

Question

Given:
$⎡ ⎢ ⎢ ⎢ ⎢ ⎢ ⎣ \begin{matrix} H_{2} (g) + \frac{1}{2} O_{2} (g) = H_{2} O (g); Δ H = - 241.8 k J C_{2} H_{2} (g) + \frac{5}{2} O_{2} (g) = 2 C O_{2} (g) + H_{2} O (g); Δ H = - 1300 k J \end{matrix} ⎤ ⎥ ⎥ ⎥ ⎥ ⎥ ⎦$
Equal volumes of $C_{2} H_{2}$ and $H_{2}$ are combusted under identical conditions. The ratio of heats evolved in the two cases is

A

5.37/1

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B

1/5.37

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C

1/1

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D

none of these

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Solution

The correct option is A 5.37/1
According to Avogadro's law: Equal volumes of all gases, at the same temperature and pressure, have the same number of molecules/moles.

Lets consider equal volumes are combusted in such a manner that 1 mole of each is combusted.
$Δ H$ for 1 mole of the reactant is given in the question.
$∴$ Using the given data,
$\frac{△ H_{c o m b} (C_{2} H_{2})}{△ H_{c o m b} (H_{2})} = \frac{- 1300}{- 241.8}$ = $\frac{5.376}{1}$

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Similar questions

Q. Equal volumes of

C_{2} H_{2}

H_{2}

are combusted under identical conditions. The ratio of heat evolved for

C_{2} H_{2}

H_{2}

H_{2} (g) + 1 / 2 O_{2} (g) \to H_{2} O (g),

Δ H = - 241.8

C_{2} H_{2} (g) + 5 / 2 O_{2} (g) \to 2 C O_{2} (g) + H_{2} O (g)

Δ H = - 1300

⎡ ⎢ ⎢ ⎢ ⎢ ⎢ ⎣ \begin{matrix} H_{2} (g) + \frac{1}{2} O_{2} (g) = H_{2} O (g); Δ H = - 241.8 k J C_{2} H_{2} (g) + \frac{5}{2} O_{2} (g) = 2 C O_{2} (g) + H_{2} O (g); Δ H = - 1300 k J \end{matrix} ⎤ ⎥ ⎥ ⎥ ⎥ ⎥ ⎦

Equal volumes of

C_{2} H_{2}

H_{2}

are combusted under identical conditions. The ratio of heats evolved in the two cases is

H_{2 (g)} + \frac{1}{2} O_{2 (g)} \to H_{2} O_{(g)}

Δ H = 241.8 k J

C O_{(g)} + \frac{1}{2} O_{2 (g)} \to C O_{2 (g)}

Δ H = 283 k J

The heat evolved during the combustion of

112

litre of water gas (mixture of equal volume of

H_{2}

C O

Q. The heat evolved during the combustion of 112 litre of water gas at STP (mixture of equal volume of

H_{2}

H_{2} (g) + 1 / 2 O_{2} (g) = H_{2} O (g); Δ H = - 241.8 k J

C O (g) + 1 / 2 O_{2} (g) = C O_{2} (g); Δ H = - 283 k J

Q. Find out the heat evolved in combustion if

112

litres(at STP) od water gas (mixture of equal volue of

H_{2} (g)

C O (g)

H_{2} (g) + 1 / 2 O_{2} (g) \to H_{2} O (g)

Δ H = - 241.8 k J

C O (g) + 1 / 2 O_{2} (g) \to C O_{2} (g)

Δ H = - 283 k J

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Heat of Reaction

Standard XII Chemistry

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