An ideal gas is enclosed in a container at absolute temperature T. The absolute temperature is now reduced to 0.5T, whilst the volume is kept constant. Why the following statement is correct?
(1) The average separation of the molecules remains unchanged.
Physics - Matter
2011-01-24 5:40 am
回答 (2)
2011-01-24 6:01 am
✔ 最佳答案
Because the question states that the volume is kept CONSTANT, thus the density of the gas remains CONSTANT since the container is supposed to be closed, i.e. the mass of gas kept in it is also constant.With the density of the gas remaining constant, the average separation of the molecules also remains unchanged.
參考: 原創答案
2011-01-24 6:17 am
The crucial point is the number of molecules is the same before and after the temperature change. This is the conservation of mass.
Suppose there are N molecules in a volume V, say. Hence, each molecule occupies, on average, a volume of V/N
The average separation between molecules = cube-root[V/N]
Since it is given that V is kept constant, as long as N also remains constant (and this is the case), the average separation thus remains unchanged.
Suppose there are N molecules in a volume V, say. Hence, each molecule occupies, on average, a volume of V/N
The average separation between molecules = cube-root[V/N]
Since it is given that V is kept constant, as long as N also remains constant (and this is the case), the average separation thus remains unchanged.
收錄日期: 2021-04-29 17:38:17
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