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Standard XII

Chemistry

Oxides of Sulphur

When 0.5 g of...

Question

When 0.5 g of sulfur is burnt to ${S O}_{2}$ 4.6 kJ heat is liberated. What is the enthalpy of formation of sulfur dioxide?
( $S = 32$ and $O = 16$ )

+294.4 kJ

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+147.2 kJ

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-147.2 kJ

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-294.4 kJ

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Solution

The correct option is D -294.4 kJ
$S + O_{2} ⟶ S O_{2}$
The enthalpy of formation is calculated for 1 mole of formation of $S O_{2}$ .
One mole of $S O_{2}$ forms when one mole of $S$ (32 grams) reacts.
For 0.5 g $⟶ Δ H$ =-4.6 kJ
$Δ H$ is negative because it is exothermic, heat is released.
For 32 g $⟶ Δ H = x$
$⟹ x = \frac{32 \times (- 4.6)}{0.5} k J = - 294.4 k J$
$∴$ Enthalpy of formation of $S O_{2}$ is -294.4 kJ.

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When 0.5 g of sulfur is burnt to SO2 4.6 kJ heat is liberated. What is the enthalpy of formation of sulfur dioxide? (S=32 and O=16)

When 0.5 g of sulfur is burnt to ${S O}_{2}$ 4.6 kJ heat is liberated. What is the enthalpy of formation of sulfur dioxide?
( $S = 32$ and $O = 16$ )