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Mole Concept and Avogadro's Number

A bulb contai...

Question

A bulb contains $1.6$ g of $O_{2}$ . It contains

A

0.05

mol of

O_{2}

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B

3.011 \times 10^{22}

molecules of

O_{2}

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C

1.12

L of

O_{2}

at STP

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D

1.12

L of

O_{2}

at SATP

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Solution

The correct options are
A $0.05$ mol of $O_{2}$
B $1.12$ L of $O_{2}$ at STP
C $3.011 \times 10^{22}$ molecules of $O_{2}$
D $1.12$ L of $O_{2}$ at SATP
$N u m b e r o f m o l e s = \frac{W e i g h t o f s u b s t a n c e}{M o l e c u l a r w e i g h t o f s u b s t a n c e}$ .
$N u m b e r o f m o l e c u l e s = N u m b e r o f m o l e s \times 6.023 \times 10^{23}$ .
$V o l u m e o f s u b s t a n c e a t S A T P a n d S T P = N u m b e r o f m o l e s \times 22.4 = 1.12 L$ .
a. Moles of $O_{2} = \frac{1.6}{32} = 0.05$
b. Molecules of $O_{2} = 0.05 \times 6.023 \times 10^{23} = 3.011 \times 10^{22}$
c. Volume of $O_{2}$ at STP $= 0.05 \times 22.4 = 1.12 L$
d. $V_{O_{2}}$ at SATP $= 0.05 \times 24.4 = 1.22 L$
Hence options A,B,C & D are correct.

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