Q. If $S + O_{2} \to S O_{2}; Δ H = - 298.2 k J m o l^{- 1}$
$S O_{2} + 1/2 O_{2} \to S O_{3}; Δ H = - 98.7 k J m o l^{- 1}$
$S O_{3} + H_{2} O \to H_{2} S O_{4}; Δ H = - 130.2 k J m o l^{- 1}$
$H_{2} + 1/2 O_{2} \to H_{2} O; Δ H = - 287.3 k J m o l^{- 1}$
Then the enthalpy of formation of $H_{2} S O_{4}$ at $298 K$ is-

908 159 NTA AbhyasNTA Abhyas 2020 Report Error

A

$- 814.4 K J$

B

$- 650.3 K J$

C

$- 320.5 K J$

D

$- 433.5 K J$

Solution:

$Δ H = Δ H_{1} + Δ H_{2} + Δ H_{3} + Δ H_{4}$