If H 2- O 2- H 2 O - So- while proving law of conservation of mass Why we take O 2 as 1 - 2 O 2 -

We take single molecule of oxygen to balance the number of oxygen atom on the both sides of the equation ...

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Stoichiometry

If H 2+ O 2= ...

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If H₂+ O₂= H₂O . So, while proving the law of conservation of mass Why we take O₂as 1/2 O₂?

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H_{2} S + \frac{3}{2} O_{2} \to H_{2} O + S O_{2},

Δ H = - 136.7 K c a l

H_{2} + \frac{1}{2} O_{2} \to H_{2} O, Δ H = - 68.4 K c a l

S + O_{2} \to S O_{2}, Δ H = - 71 K c a l

Δ H_{f} o f H_{2} S

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 = - 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}; 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} \to S O_{2}

Δ H = - 298.2

S O_{2} + \frac{1}{2} O_{2} \to S O_{3}

Δ H = - 98.7

S O_{3} + H_{2} O \to H_{2} S O_{4}

Δ H = - 130.2

H_{2} + \frac{1}{2} O_{2} \to H_{2} O

Δ H = - 287.3

H_{2} S O_{4}

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