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The following physics responses are provided by a student and, as such, should be considered in that context. While every effort is made for accuracy, absolute correctness cannot be fully guaranteed.
| Question | |
C | 10 |
I | |
Question Two one-liter containers each contain 10 moles of a gas. The temperature is the same in both containers. Container A holds helium (molecular mass = 4 u), and Container B holds oxygen (molecular mass = 16 u). Which container has the higher pressure and by what factor? | |
Answer Both containers have the same pressure. | |
Notes
| User | Added | Note | e | d |
|---|---|---|---|---|
| KillGorack | 2023-07-04 15:28:35 | To compare the pressures in Container A (helium) and Container B (oxygen), we can use the ideal gas law equation: PV = nRT Since the temperature (T) and volume (V) are the same for both containers, we can compare the pressures (P) directly. The number of moles (n) is also given as 10 moles for both containers. For Container A (helium), the molecular mass (M_A) is 4 u. For Container B (oxygen), the molecular mass (M_B) is 16 u. We can calculate the pressure ratio between the two containers as follows: P_A / P_B = (n_A * R * T) / (n_B * R * T) = (n_A / n_B) * (R * T / R * T) = (n_A / n_B) Since both containers have the same number of moles (n_A = n_B = 10 moles), the pressure ratio simplifies to: P_A / P_B = 10 / 10 = 1 Therefore, the pressure in Container A (helium) is equal to the pressure in Container B (oxygen), with a pressure ratio of 1. They have the same pressure. |
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