Which of the following has the maximum mass?

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(D) To find the maximum mass,calculate the mass for each option:$(A)$ $0.1 \ g$ atom of $C$ means $0.1 \ mole$ of $C$ atoms. Mass $= 0.1 	imes 12 = 1

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$1120 \ mL$ of $CO_2$ at $1 \ atm, 273 \ K$

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(D) To find the maximum mass,calculate the mass for each option:$(A)$ $0.1 \ g$ atom of $C$ means $0.1 \ mole$ of $C$ atoms. Mass $= 0.1 	imes 12 = 1.2 \ g$.$(B)$ $0.1 \ mole$ of $NH_3$. Molar mass of $NH_3 = 14 + 3 = 17 \ g/mol$. Mass $= 0.1 	imes 17 = 1.7 \ g$.$(C)$ $6.02 	imes 10^{22}$ molecules of $H_2$. Number of moles $= \frac{6.02 	imes 10^{22}}{6.02 	imes 10^{23}} = 0.1 \ mole$. Mass $= 0.1 	imes 2 = 0.2 \ g$.$(D)$ $1120 \ mL$ of $CO_2$ at $STP$ $(1 \ atm, 273 \ K)$. Number of moles $= \frac{1120}{22400} = 0.05 \ mole$. Mass $= 0.05 	imes 44 = 2.2 \ g$.Comparing the values: $1.2 \ g, 1.7 \ g, 0.2 \ g, 2.2 \ g$. The maximum mass is $2.2 \ g$.

List-$I$	List-$II$
$(a)$ $2 \text{ moles of ethene}$	$(i)$ $11.2 \text{ L volume at STP}$
$(b)$ $\text{Molar mass is equal to } 66 \text{ g}$	$(ii)$ $56 \text{ g}$
$(c)$ $1 \text{ g of } H_2$	$(iii)$ $12.04 \times 10^{23} \text{ molecules}$
$(d)$ $2 \text{ moles of water vapours}$	$(iv)$ $1.5 \text{ mole of } CO_2$

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