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Calculate the molar mass of a gaseous oxide of sulfur and deduce its molecular formular if 0.250dm³ of this oxide at STP has a mass of 0.706 g.​

Sagot :

Nono946
To calculate the molar mass of the gaseous oxide of sulfur, we can use the ideal gas law:

PV = nRT

Where:
- P is the pressure (STP: standard pressure = 1 atm)
- V is the volume (0.250 dm³)
- n is the number of moles
- R is the ideal gas constant (0.0821 L.atm/mol.K)
- T is the temperature (STP: standard temperature = 273 K)

First, we need to calculate the number of moles of the gas using the given volume and the ideal gas law:

n = (PV) / (RT)

n = ((1 atm)(0.250 dm³)) / ((0.0821 L.atm/mol.K)(273 K))

n ≈ (0.250) / (22.414)

n ≈ 0.01116 moles

Next, we use the definition of molar mass (M):

M = (m) / (n)

Where:
- m is the mass of the gas (0.706 g)
- n is the number of moles we calculated earlier

M = (0.706 g) / (0.01116 moles)

M ≈ 63.26 g/mol

Now, we know the molar mass of the gaseous oxide of sulfur is approximately 63.26 g/mol.

To deduce its molecular formula, we need to know the individual masses of sulfur and oxygen in the compound. Without that information, we can't determine the molecular formula uniquely. However, one common gaseous oxide of sulfur is sulfur dioxide (SO₂), which has a molar mass close to the calculated value. So, the molecular formula might be SO₂.
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