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Four different experiments were conducted in the following ways
I - 3g of carbon was burnt in 8g of oxygen to give 11g of $C O_{2}$

II - 1.2 g of carbon was burnt in air to give 4.2 g of $C O_{2}$

III - 4.5 g of carbon was burnt in enough air to give 11 g of $C O_{2}$

IV - 4g of carbon was burnt in oxygen to form 30.3 g of $C O_{2}$

Law of constant proportions is illustrated in experiments

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II and III

I and III

IV only

I only

answer is D.

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Detailed Solution

I - 3g of carbon was burnt in 8g of oxygen to give 11g of

C O_{2}

$C + O_{2} \to C O_{2}$

Moles of ‘C’ $= \frac{3}{12} g / m o l = 0.25 m o l e s$

Moles of $O_{2} = \frac{8}{32} = 0.25 m o l e s$

Moles of $C O_{2} = \frac{11}{44} = 0.25 m o l e s$ .

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