If a mole is defined to be 3 - 1024 instead of Avogadro-s Number- 6 - 1023 - what would be the mass of one mole of Argon atoms- -Atomic mass of Ar on conventional scale is 40 -

The correct option is B 200 g6 × 10^23 atoms of Ar = 40 g 3 × 10^24 atoms of Ar = 40/6 × 10^23× 3 × 10^24 = 200 g ...

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Standard XII

Physics

Measuring Mass

If a mole is ...

Question

If a mole is defined to be $3 \times 10^{24}$ (instead of Avogadro’s Number, $6 \times 10^{23}$ ), what would be the mass of one mole of Argon atoms? [Atomic mass of Ar on the conventional scale is 40]

40 g

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200 g

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20 g

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None of these

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Solution

The correct option is B 200 g
$6 \times 10^{23}$ atoms of $A r = 40 g$

$3 \times 10^{24}$ atoms of $A r = \frac{40}{6 \times 10^{23}} \times 3 \times 10^{24}$

Then, the mass of one mole of Argon atoms $= 200 g$

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If a mole is defined to be 3×1024 (instead of Avogadro’s Number, 6×1023), what would be the mass of one mole of Argon atoms? [Atomic mass of Ar on the conventional scale is 40]

The correct option is B 200 g6×1023 atoms of Ar=40 g 3×1024 atoms of Ar=406×1023×3×1024 Then, the mass of one mole of Argon atoms=200 g

If a mole is defined to be $3 \times 10^{24}$ (instead of Avogadro’s Number, $6 \times 10^{23}$ ), what would be the mass of one mole of Argon atoms? [Atomic mass of Ar on the conventional scale is 40]

The correct option is B 200 g
$6 \times 10^{23}$ atoms of $A r = 40 g$

$3 \times 10^{24}$ atoms of $A r = \frac{40}{6 \times 10^{23}} \times 3 \times 10^{24}$

Then, the mass of one mole of Argon atoms $= 200 g$