Under the same conditions of temperature and pressure, which of the following gases would occupy the largest volume?
A 0-20g of hydrogen
B 0-44g of carbon dioxide
C 0-60g of neon
D 0-80g of argon - Scottish Highers Chemistry - Question 13 - 2018
Question 13
Under the same conditions of temperature and pressure, which of the following gases would occupy the largest volume?
A 0-20g of hydrogen
B 0-44g of carbon dioxide
C... show full transcript
Worked Solution & Example Answer:Under the same conditions of temperature and pressure, which of the following gases would occupy the largest volume?
A 0-20g of hydrogen
B 0-44g of carbon dioxide
C 0-60g of neon
D 0-80g of argon - Scottish Highers Chemistry - Question 13 - 2018
Step 1
0-20g of hydrogen
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Answer
Hydrogen is a light gas and has a molar mass of approximately 2 g/mol. Therefore, 20 g of hydrogen would equal about 10 moles of hydrogen, which occupies a volume of approximately 2240 liters at standard temperature and pressure (STP).
Step 2
0-44g of carbon dioxide
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Answer
Carbon dioxide has a molar mass of about 44 g/mol. With 44 g, we have 1 mole of CO2, which occupies approximately 22.4 liters at STP.
Step 3
0-60g of neon
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Answer
Neon has a molar mass of around 20 g/mol. Therefore, 60 g of neon corresponds to about 3 moles, occupying approximately 67.2 liters at STP.
Step 4
0-80g of argon
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Argon has a molar mass of approximately 40 g/mol. Thus, 80 g of argon would be equivalent to 2 moles, occupying approximately 44.8 liters at STP.
Step 5
Conclusion
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Answer
Among all the gases, 0-20g of hydrogen will occupy the largest volume due to its low molar mass and high number of moles. Hence, the answer is A.
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