Question

the number of water molecules is maximum in....
A) 18 gram of water
B) 18 moles of water
C) 18 molecules of water
D) 1.8 gram of water

Answer 1

Answer: B) 18 moles of water

Explanation:

According to avogadro's law, 1 mole of every substance occupies 22.4 L at STP and contains avogadro's number $6.023\times 10^{23}$ of particles.

A) 18 gram of water

$\text{Number of moles}=\frac{\text{Given mass}}{\text {Molar mass}}=\frac{18g}{18g/mol}=1mole$

1 mole of $H_2O$ contains =$6.023\times 10^{23}$ molecules of water.

B) 18 moles of water

1 mole of $H_2O$ contains =$6.023\times 10^{23}$ molecules of water.

18 moles of $H_2O$ contains =$\frac{6.023\times 10^{23}}{1}\times 18=108.4\times 10^{23}$ molecules of water.

C) 18 molecules of water

D) 1.8 gram of water

$\text{Number of moles}=\frac{\text{Given mass}}{\text {Molar mass}}=\frac{1.8g}{18g/mol}=0.1mole$

1 mole of $H_2O$ contains =$6.023\times 10^{23}$ molecules of water.

0.1 mole of $H_2O$ contains =$\frac{6.023\times 10^{23}}{1}\times 0.1=6.023\times 10^{22}$ molecules of water.

Answer 2

$</p><p>According to avogadro's law, 1 mole of every substance occupies 22.4 L at STP and contains avogadro's number 6.023\times 10^{23}6.023×1023 of particles.</p><p></p><p>A) 18 gram of water</p><p></p><p>\text{Number of moles}=\frac{\text{Given mass}}{\text {Molar mass}}=\frac{18g}{18g/mol}=1moleNumber of moles=Molar massGiven mass=18g/mol18g=1mole</p><p></p><p>1 mole of H_2OH2O contains =6.023\times 10^{23}6.023×1023molecules of water.</p><p></p><p>B) 18 moles of water</p><p></p><p>1 mole of H_2OH2O contains =6.023\times 10^{23}6.023×1023molecules of water.</p><p></p><p>18 moles of H_2OH2O contains =\frac{6.023\times 10^{23}}{1}\times 18=108.4\times 10^{23}16.023×1023×18=108.4×1023 molecules of water.</p><p></p><p>C) 18 molecules of water</p><p></p><p>D) 1.8 gram of water</p><p></p><p>\text{Number of moles}=\frac{\text{Given mass}}{\text {Molar mass}}=\frac{1.8g}{18g/mol}=0.1moleNumber of moles=Molar massGiven mass=18g/mol1.8g=0.1mole</p><p></p><p>1 mole of H_2OH2O contains =6.023\times 10^{23}6.023×1023molecules of water.</p><p></p><p>0.1 mole of H_2OH2O contains =\frac{6.023\times 10^{23}}{1}\times 0.1=6.023\times 10^{22}16.023×1023×0.1=6.023×1022 molecules of water.</p><p></p><p>$

According to avogadro's law, 1 mole of every substance occupies 22.4 L at STP and contains avogadro's number 6.023\times 10^{23}6.023×1023 of particles.

A) 18 gram of water

\text{Number of moles}=\frac{\text{Given mass}}{\text {Molar mass}}=\frac{18g}{18g/mol}=1moleNumber of moles=Molar massGiven mass=18g/mol18g=1mole

1 mole of H_2OH2O contains =6.023\times 10^{23}6.023×1023molecules of water.

B) 18 moles of water

1 mole of H_2OH2O contains =6.023\times 10^{23}6.023×1023molecules of water.

18 moles of H_2OH2O contains =\frac{6.023\times 10^{23}}{1}\times 18=108.4\times 10^{23}16.023×1023×18=108.4×1023 molecules of water.

C) 18 molecules of water

D) 1.8 gram of water

\text{Number of moles}=\frac{\text{Given mass}}{\text {Molar mass}}=\frac{1.8g}{18g/mol}=0.1moleNumber of moles=Molar massGiven mass=18g/mol1.8g=0.1mole

1 mole of H_2OH2O contains =6.023\times 10^{23}6.023×1023molecules of water.

0.1 mole of H_2OH2O contains =\frac{6.023\times 10^{23}}{1}\times 0.1=6.023\times 10^{22}16.023×1023×0.1=6.023×1022 molecules of water.

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