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(B) The molar mass of water $(H_2O)$ is calculated as: $(2 	imes 1) + 16 = 18 \, g/mol$.To find the number of moles in $360 \, g$ of water,we use the

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$(ii)$ and $(iv)$

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(B) The molar mass of water $(H_2O)$ is calculated as: $(2 	imes 1) + 16 = 18 \, g/mol$.To find the number of moles in $360 \, g$ of water,we use the formula: $	ext{Number of moles} = \frac{	ext{Given mass}}{	ext{Molar mass}} = \frac{360 \, g}{18 \, g/mol} = 20 \, 	ext{moles}$.Thus,statement $(ii)$ is correct.To find the number of molecules,we multiply the number of moles by Avogadro's constant $(N_A = 6.022 	imes 10^{23} \, 	ext{molecules/mol})$:$	ext{Number of molecules} = 20 	imes 6.022 	imes 10^{23} = 1.2044 	imes 10^{25} \, 	ext{molecules}$.Thus,statement $(iv)$ is also correct.Therefore,the correct representation is $(ii)$ and $(iv)$.

Which of the following correctly represents $360 \, g$ of water?
$(i)$ $2$ moles of $H_2O$
$(ii)$ $20$ moles of water
$(iii)$ $6.022 \times 10^{23}$ molecules of water
$(iv)$ $1.2044 \times 10^{25}$ molecules of water

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Which of the following correctly represents $360 \, g$ of water?$(i)$ $2$ moles of $H_2O$$(ii)$ $20$ moles of water$(iii)$ $6.022 \times 10^{23}$ molecules of water$(iv)$ $1.2044 \times 10^{25}$ molecules of water