If S- O 2 - SO 2 - H-298-2kJ S0 2 -1- 20 2 - SO 3 - H-98-7kJ SO 3 - H 2 O- H 2 SO 4 - H-130-2kJ H 2 -1- 20 2 - H 2 O- H-287kJThen the enthalpy of formation of H 2 SO 4 at 298 K is-

The correct option is A 814.4 kJ S + O_2 ⇌ SO_2 Δ H_1 = 298.2 kJ ... (I) SO_2 + 12 O_2 ⇌ SO_3 Δ H_2 = 98.7 kJ ... (II) SO_3 + H_ ...

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Heat of Formation

If S+ O 2 →...

Question

If $S + O_{2} \to {S O}_{2}; △ H = - 298.2 k J$
${S 0}_{2} + 1 / 20_{2} \to {S O}_{3}; △ H = - 98.7 k J$
$S O_{3} + H_{2} O \to H_{2} {S O}_{4}; △ H = - 130.2 k J$
$H_{2} + 1 / 20_{2} \to H_{2} O; △ H = - 287 k J$
Then the enthalpy of formation of $H_{2} {S O}_{4}$ at 298 K is?

-814.4 kJ

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-650.3 kJ

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-320.5 kJ

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-433.5 kJ

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Solution

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Similar questions

S + O_{2} \to {S O}_{2}; Δ H = - 298.2 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 = - 130.2 k J

H_{2} + \frac{1}{2} O_{2} \to H_{2} O; Δ H = - 227.3 k J

H_{2} {S O}_{4}

S + O_{2} \to {S O}_{2}; △ H = - 398.2 k J : {S O}_{2} + \frac{1}{2} O_{2} \to {S O}_{3}; △ H = - 98.7 k J

{S O}_{3} + H_{2} O \to H_{2} {S O}_{4}; △ H = - 130.2 k J : H_{2} + \frac{1}{2} O_{2} \to H_{2} O, △ H = - 227.3 k J

S + O_{2} \to S O_{2}; Δ H = - 298.2 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 = - 130.2 k J

H_{2} + \frac{1}{2} O_{2} \to H_{2} O; Δ H = - 227.3 k J

H_{2} S O_{4}

298

S + O_{2} ⟶ S O_{2}; Δ H = - 298.2 k J

S O_{2} + 1 / 2 O_{2} ⟶ S O_{3}; Δ H = - 98.7 k J

S O_{3} + H_{2} O ⟶ H_{2} S O_{4}; Δ H = - 130.2 k J

H_{2} + 1 / 2 O_{2} ⟶ H_{2} O; Δ H = - 287.3 k J

H_{2} S O_{4} a t 298 K

S + O_{2} \to S O_{2}; Δ H = - 398.2 k J; S O_{2} + \frac{1}{2} O_{2} \to S O_{3}; Δ H = - 98.7 k J

S O_{2} + H_{2} O \to H_{2} S O_{4}; Δ H = - 130.2 k J; H_{2} + \frac{1}{2} O_{2} \to H_{2} O; Δ H = - 227.3 k J

298

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