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If the volume of a fixed mass of an ideal gas is halved at a constant temperature, the pressure inside the container would :
Explanation
This phenomenon is explained by Boyle's Law, which states that for a fixed mass of an ideal gas at a constant temperature, the pressure (P) is inversely proportional to its volume (V). Mathematically, this is expressed as:
P ∝ 1/V or PV = k (constant)
If the initial state is P1V1 and the volume is halved (V2 = V1/2), the new pressure P2 can be calculated using the formula:
P1V1 = P2V2
P1V1 = P2(V1/2)
P2 = 2P1
Therefore, when the volume is halved at a constant temperature, the pressure inside the container is doubled. This occurs because the same number of gas molecules are now confined to half the space, resulting in twice as many collisions with the container walls per unit area.
SIMILAR QUESTIONS
In a certain process, the relation between pressure (P) and volume (V), for an ideal gas, is given by PV2 = constant. If the initial temperature is T1 and the final temperature is T2; and the initial volume is V1 and the final volume is V2, then which one of the following is correct?
A very large container consists of an ideal gas. The speed of sound in the gas is x. When the pressure of the gas is doubled while keeping the temperature constant, the speed of sound now becomes y. What is the ratio of x to y?