? $\to B a S O_{4} (a q) + H_{2} O (l)$
What are the reactants used to carry out this reaction?

S O_{4} (g) + B a (O H)_{2}

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S O_{3} (g) + B a (O H)_{2}

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S O_{3} (g) + B a O H

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The reaction does not occur.

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Solution

The correct option is A $S O_{3} (g) + B a (O H)_{2}$
The non-metal oxides can be neutralized with a base to form a salt and water.
$S O_{3} (g) + B a (O H)_{2} (a q) \to B a S O_{4} (a q) + H_{2} O (l)$

Suggest Corrections

Similar questions

Δ H^{o}

N a_{2} O (s) + S O_{3} (g) \to N a_{2} S O_{4} (g)

N a (s) + H_{2} O (l) \to N a O H (s) + \frac{1}{2} H_{2} (g); Δ H^{o} = - 146 k J

N a_{2} S O_{4} (s) + H_{2} O (l) \to 2 N a O H (s) + S O_{3} (g); Δ H^{o} = + 418 k J

2 N a O (s) + 2 H_{2} (g) \to 4 N a (s) + 2 H_{2} O (l); Δ H^{o} = + 259 k J

{S O}_{2} (g) + \frac{1}{2} O_{2} (g) ⇋ {S O}_{3} (g); Δ H^{o} = - v e

S O_{3} (g) + H_{2} O (l) \to H_{2} S O_{4} (a q)

Δ

H_{2} {S O}_{4} (a q) + {B a (O H)}_{2} \to

S (s) + O_{2} (g) \to {S O}_{2} (g) Δ H^{\circ} = - 297 k J

2 {S O}_{2} (g) + O_{2} (g) \to 2 {S O}_{3} (g) Δ H^{\circ} = - 198 k J

{S O}_{3} (g)

S (s) + {3 / 2 O}_{2} (g) \to {S O}_{3} (g)

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