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Mass of 525mL of a gaseous compound at 28 degree Celsius and 0.970 bar pressure was found to be 0.900g. Calculate its molar mass. ( R=0.083 )?
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Mass of 525mL of a gaseous compound at 28 degree Celsius and 0.970 bar...
To calculate the molar mass of the gaseous compound, we can use the Ideal Gas Law, which is represented by the formula:
PV = nRT
Where:
- P = Pressure
- V = Volume
- n = Number of moles
- R = Ideal gas constant
- T = Temperature in Kelvin
First, we need to convert the given conditions into suitable units.
1. Convert Temperature to Kelvin
- Given temperature = 28°C
- Temperature in Kelvin (K) = 28 + 273.15 = 301.15 K
2. Use the Ideal Gas Law to find the number of moles (n)
- Given:
- P = 0.970 bar = 0.970 × 10^5 Pa (since 1 bar = 10^5 Pa)
- V = 525 mL = 0.525 L (since 1 L = 1000 mL)
- R = 0.083 L·bar/(K·mol)
- Rearranging the Ideal Gas Law:
n = PV / RT
n = (0.970 bar) × (0.525 L) / (0.083 L·bar/(K·mol) × 301.15 K)
3. Calculate n
- n = (0.970 × 0.525) / (0.083 × 301.15)
- n ≈ 0.0202 moles
4. Calculate Molar Mass (M)
- Molar Mass (M) = mass / n
- Given mass = 0.900 g
- M = 0.900 g / 0.0202 moles ≈ 44.55 g/mol
5. Conclusion
The molar mass of the gaseous compound is approximately 44.55 g/mol.
PV = nRT
Where:
- P = Pressure
- V = Volume
- n = Number of moles
- R = Ideal gas constant
- T = Temperature in Kelvin
First, we need to convert the given conditions into suitable units.
1. Convert Temperature to Kelvin
- Given temperature = 28°C
- Temperature in Kelvin (K) = 28 + 273.15 = 301.15 K
2. Use the Ideal Gas Law to find the number of moles (n)
- Given:
- P = 0.970 bar = 0.970 × 10^5 Pa (since 1 bar = 10^5 Pa)
- V = 525 mL = 0.525 L (since 1 L = 1000 mL)
- R = 0.083 L·bar/(K·mol)
- Rearranging the Ideal Gas Law:
n = PV / RT
n = (0.970 bar) × (0.525 L) / (0.083 L·bar/(K·mol) × 301.15 K)
3. Calculate n
- n = (0.970 × 0.525) / (0.083 × 301.15)
- n ≈ 0.0202 moles
4. Calculate Molar Mass (M)
- Molar Mass (M) = mass / n
- Given mass = 0.900 g
- M = 0.900 g / 0.0202 moles ≈ 44.55 g/mol
5. Conclusion
The molar mass of the gaseous compound is approximately 44.55 g/mol.
Community Answer
Mass of 525mL of a gaseous compound at 28 degree Celsius and 0.970 bar...
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Mass of 525mL of a gaseous compound at 28 degree Celsius and 0.970 bar pressure was found to be 0.900g. Calculate its molar mass. ( R=0.083 )?
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Mass of 525mL of a gaseous compound at 28 degree Celsius and 0.970 bar pressure was found to be 0.900g. Calculate its molar mass. ( R=0.083 )? for Class 11 2024 is part of Class 11 preparation. The Question and answers have been prepared according to the Class 11 exam syllabus. Information about Mass of 525mL of a gaseous compound at 28 degree Celsius and 0.970 bar pressure was found to be 0.900g. Calculate its molar mass. ( R=0.083 )? covers all topics & solutions for Class 11 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for Mass of 525mL of a gaseous compound at 28 degree Celsius and 0.970 bar pressure was found to be 0.900g. Calculate its molar mass. ( R=0.083 )?.
Mass of 525mL of a gaseous compound at 28 degree Celsius and 0.970 bar pressure was found to be 0.900g. Calculate its molar mass. ( R=0.083 )? for Class 11 2024 is part of Class 11 preparation. The Question and answers have been prepared according to the Class 11 exam syllabus. Information about Mass of 525mL of a gaseous compound at 28 degree Celsius and 0.970 bar pressure was found to be 0.900g. Calculate its molar mass. ( R=0.083 )? covers all topics & solutions for Class 11 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for Mass of 525mL of a gaseous compound at 28 degree Celsius and 0.970 bar pressure was found to be 0.900g. Calculate its molar mass. ( R=0.083 )?.
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