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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 $(iv)$.

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$2$. The element used by Rutherford during his $\alpha$-scattering experiment.	$1$. $A$ white lustrous metal used for making ornaments and which tends to get tarnished black in the presence of moist air.
$3$. An element which forms rust on exposure to moist air.	$4$. Both brass and bronze are alloys of this element.
$5$. $A$ very reactive non-metal stored under water.	$6$. The metal which exists in the liquid state at room temperature.
$7$. Zinc metal when treated with dilute hydrochloric acid produces a gas of this element which when tested with a burning splinter produces a pop sound.	$8$. An element with the symbol $Pb$.

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

Similar Questions

$A$ $0.24 \, g$ sample of a compound of oxygen and boron was found by analysis to contain $0.096 \, g$ of boron and $0.144 \, g$ of oxygen. Calculate the percentage composition of the compound by weight.

State the postulate of Dalton's atomic theory which led to the law of conservation of mass. Calculate the molecular mass of water.

Calculate the mass of:
$(a)$ $1$ atom of carbon
$(b)$ $0.02$ mole of sodium
$(c)$ $1$ molecule of water.

Verify by calculating that:
$(a)$ $5$ moles of $CO_2$ has a higher mass than $5$ moles of $H_2O$.
$(b)$ $120 \, g$ of calcium and $120 \, g$ of magnesium elements have a mole ratio of $3:5$.

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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