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Photochemical Reaction

The balanced ...

Question

The balanced chemical equation for the thermal decomposition of ferrous sulphate crystals is :

6 F e S O_{4} (s) H e a t - -- \to 3 F e_{2} O_{3} (s) + S O_{2} (g) + 4 S O_{3} (g)

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3 F e S O_{4} (s) H e a t - -- \to F e_{3} O_{4} (s) + S O_{2} (g) + S O_{3} (g)

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2 F e S O_{4} (s) H e a t - -- \to F e_{2} O_{3} (s) + S O_{2} (g) + S O_{3} (g)

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F e S O_{4} (s) H e a t - -- \to F e_{2} O_{3} (s) + S O_{2} (g) + S O_{3} (g)

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Solution

The correct option is B $2 F e S O_{4} (s) H e a t - -- \to F e_{2} O_{3} (s) + S O_{2} (g) + S O_{3} (g)$
$2 F e S O_{4} (s) H e a t - -- \to F e_{2} O_{3} (s) + S O_{2} (g) + S O_{3} (g)$

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Similar questions

F e S O_{4} (s) h e a t - - \to F e_{2} O_{3} (s) + S O_{2} (g) + S O_{3} (g)

. . . S O_{2} (g) + . . . . O_{2} (g) \to . . . S O_{3} (g)

According to the above unbalanced equation, how many moles of $S O_{2} (g)$ will react completely with 1 mole of $O_{2} (g)$ ?

S_{(s)} + O_{2 (g)} \to S O_{2 (g)}; Δ H = - 298.2 k J

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

S O_{3 (g)} + H_{2} O_{(l)} \to H_{2} S O_{4 (l)}; Δ H = - 130.2 k J

H_{2 (g)} + \frac{1}{2} O_{2 (g)} \to H_{2} O_{(l)}; Δ H = - 287.3 k J

H_{2} S O_{4}

S O_{2} (g) + \frac{1}{2} O_{2} (g) ⇌ {S O}_{3} (g)

K_{c}

1.7 \times 10^{12}

300 K

300 K

2 S O_{2} (g) + O_{2} (g) ⇌ 2 {S O}_{3} (g)

{S O}_{3} (g) ⇌ S O_{2} (g) + \frac{1}{2} O_{2} (g)

S (s) + \frac{3}{2} O_{2} (g) \to S O_{3} (g) + 2 x k c a l

S O_{2} (g) + \frac{1}{2} O_{2} (g) \to S O_{3} (g) + y k c a l

S O_{2}

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