How many FeSO₄.7H₂SO₄ will be oxidised by an acidified solution containing 9.48g

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How many FeSO₄.7H₂SO₄ will be oxidised by an acidified solution containing 9.48 g KMnO₄

Options

(a) 83.4 g
(b) 16.7 g
(c) 1.67 g
(d) 8.3 g

Correct Answer:

83.4 g

Explanation:

Balanced reaction: 2KMnO₄ + 10FeSO₄.7H₂O + 8H₂SO₄ → 5F₂(SO₄)₃ + K₂SO₄ + 2MnSO₄ + 78H₂O. 2 * 158 g KMnO₄ oxidises = 10 * 278 g FeSO₄.7H₂O. 9.48 g KMnO₄ oxidises = 10 * 278 * 9.48 / 2 * 158 = 83.4 g.

Related Questions:

1. The following composition is known as “Bordeaux mixture”.
2. M⁺³ ion loses 3e⁻. Its oxidation number will be
3. Which of the following compounds shows evidence of the strongest hydrogen bond
4. Which one of the following reagents will be able to distinguish between 1-butyne
5. Metallic crystalline solids have

Topics: D and F Block Elements (91)
Subject: Chemistry (2512)

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