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Zorluk: OrtaThe Mole Concept, Avogadro's Constant, and Molar Mass

What is the volume, in dm3\text{dm}^3, occupied by 6.80 g6.80\text{ g} of hydrogen sulfide gas (H2S\text{H}_2\text{S}) measured at standard temperature and pressure (STP)? [H=1.0,S=32.0,Molar volume of gas at STP=22.4 dm3mol−1][\text{H} = 1.0, \text{S} = 32.0, \text{Molar volume of gas at STP} = 22.4\text{ dm}^3\text{mol}^{-1}]

  1. 4.48 dm34.48\text{ dm}^3Cevap
  2. B
    4.80 dm34.80\text{ dm}^3
  3. C
    4.76 dm34.76\text{ dm}^3
  4. D
    2.24 dm32.24\text{ dm}^3

Cevap

The volume occupied by 6.80 g6.80\text{ g} of hydrogen sulfide gas at STP is 4.48 dm34.48\text{ dm}^3.
To find the volume of gas at STP, first determine the molar mass of H2S\text{H}_2\text{S}: (2×1.0)+32.0=34.0 g mol−1(2 \times 1.0) + 32.0 = 34.0\text{ g mol}^{-1}. Next, convert the mass to moles: 6.80 g34.0 g mol−1=0.20 mol\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 dm3mol−122.4\text{ dm}^3\text{mol}^{-1}): 0.20×22.4=4.48 dm30.20 \times 22.4 = 4.48\text{ dm}^3.

Adım Adım Çözüm

1
Calculate the molar mass of hydrogen sulfide (H2S\text{H}_2\text{S})
Molar Mass=(2×1.0)+32.0=34.0 g mol−1\text{Molar Mass} = (2 \times 1.0) + 32.0 = 34.0\text{ g mol}^{-1}
Molar mass is required to convert mass to moles.
2
Calculate the number of moles in 6.80 g6.80\text{ g} of H2S\text{H}_2\text{S}
Moles=6.80 g34.0 g mol−1=0.20 mol\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.
3
Calculate the volume occupied at STP
Volume=0.20 mol×22.4 dm3mol−1=4.48 dm3\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 dm322.4\text{ dm}^3 at STP.

Anahtar Kavram

Molar Volume of Gases at STP
Tahmini Süre:1m 30s
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Konular

The Mole Concept, Avogadro's Constant, and Molar Mass

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