Question:
At T (K), a closed vessel containing 2 g of an ideal gas (A) (molar mass = $ M_A $) exerted a pressure of 1 atm. When 16 g of another ideal gas (B) (molar mass = $ M_B $) was introduced into this vessel, the pressure increased to 2 atm. What is the correct relationship between $ M_A $ and $ M_B $?
At T (K), a closed vessel containing 2 g of an ideal gas (A) (molar mass = $ M_A $) exerted a pressure of 1 atm. When 16 g of another ideal gas (B) (molar mass = $ M_B $) was introduced into this vessel, the pressure increased to 2 atm. What is the correct relationship between $ M_A $ and $ M_B $?
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Use the ideal gas law to relate the pressure and mass of gases. For a fixed volume, the pressure is proportional to the amount of substance.
Updated On: May 9, 2025
- \( 2M_A = M_B \)
- \( 4M_A = M_B \)
- \( 8M_A = M_B \)
- \( M_A = M_B \)
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The Correct Option is C
Solution and Explanation
Using the ideal gas law, the pressure is directly proportional to the amount of gas. Since the pressure doubled when 16 g of gas B was added, the relationship between the masses of A and B must satisfy \( 8M_A = M_B \).
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