What is the volume, in \text{dm}^3, occupied by 6.80\text{ g} of hydrogen sulfide gas (\te… — JAMB UTME

What is the volume, in $\text{dm}^3$ , occupied by $6.80\text{ g}$ of hydrogen sulfide gas ( $\text{H}_2\text{S}$ ) measured at standard temperature and pressure (STP)? $[\text{H} = 1.0, \text{S} = 32.0, \text{Molar volume of gas at STP} = 22.4\text{ dm}^3\text{mol}^{-1}]$

$4.48\text{ dm}^3$ Answer
B
$4.80\text{ dm}^3$
C
$4.76\text{ dm}^3$
D
$2.24\text{ dm}^3$

Answer

The volume occupied by

6.80\text{ g}

of hydrogen sulfide gas at STP is

4.48\text{ dm}^3

To find the volume of gas at STP, first determine the molar mass of

\text{H}_2\text{S}

(2 \times 1.0) + 32.0 = 34.0\text{ g mol}^{-1}

. Next, convert the mass to moles:

\frac{6.80\text{ g}}{34.0\text{ g mol}^{-1}} = 0.20\text{ mol}

. Finally, multiply the moles by the molar volume at STP (

22.4\text{ dm}^3\text{mol}^{-1}

0.20 \times 22.4 = 4.48\text{ dm}^3

Step-by-Step Solution

Calculate the molar mass of hydrogen sulfide (

\text{H}_2\text{S}

)

\text{Molar Mass} = (2 \times 1.0) + 32.0 = 34.0\text{ g mol}^{-1}

Molar mass is required to convert mass to moles.

Calculate the number of moles in

6.80\text{ g}

\text{H}_2\text{S}

\text{Moles} = \frac{6.80\text{ g}}{34.0\text{ g mol}^{-1}} = 0.20\text{ mol}

Dividing given mass by molar mass yields amount of substance in moles.

Calculate the volume occupied at STP

\text{Volume} = 0.20\text{ mol} \times 22.4\text{ dm}^3\text{mol}^{-1} = 4.48\text{ dm}^3

1 mole of any ideal gas occupies

22.4\text{ dm}^3

at STP.

Key Concept

Molar Volume of Gases at STP

Estimated Time:1m 30s

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