From the following thermochemical equations,S+O2→SO2; ΔH=−398.5KJSO2+12O2→SO3; ΔH=−98.7KJSO3+H2O→H2SO4; ΔH=−130.5KJH2+12O2→H2; ΔH=−227.3KJ If the magnitude of enthalpy of formation of sulphuric acid at 298 k is -95 x, x = ____

Reaction for formation of sulphuric acid H2+S+2O2→H2SO4As per Hess law; ΔH of formation of H2SO4=−398.5−98.7−130.5−227.3 =−855.KJ =−855=95xx=−85595=−9

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From the following thermochemical equations,
$\begin{array}{l} S + O_{2} \to S O_{2}; Δ H = - 398.5 K J \\ S O_{2} + \frac{1}{2} O_{2} \to S O_{3}; Δ H = - 98.7 K J \\ S O_{3} + H_{2} O \to H_{2} S O_{4}; Δ H = - 130.5 K J \\ H_{2} + \frac{1}{2} O_{2} \to H_{2}; Δ H = - 227.3 K J \end{array}$
If the magnitude of enthalpy of formation of sulphuric acid at 298 k is -95 x, x = ____

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answer is 9.

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Detailed Solution

Reaction for formation of sulphuric acid
$H_{2} + S + 2 O_{2} \to H_{2} S O_{4}$
As per Hess law; $Δ H$ of formation of $H_{2} S O_{4}$

$= - 398.5 - 98.7 - 130.5 - 227.3 = - 855. K J \begin{array}{l} = - 855 = 95 x \\ x = \frac{- 855}{95} = - 9 \end{array}$

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