When one mole of monoatomic ideal gas at T K undergoes adiabatic change under a constant external pressure of 1 atm and changes volume from 1 litre to 2 litre, the final temperature (in Kelvin) would beA.B.C.TD.
Question
When one mole of monoatomic ideal gas at T K undergoes adiabatic change under a constant external pressure of 1 atm and changes volume from 1 litre to 2 litre, the final temperature (in Kelvin) would beA.B.C.TD.
Solution
The question seems to be incomplete. Could you please provide the options (A, B, C, D) for the final temperature? Also, for an adiabatic process, we need to know the specific heat capacity ratio (γ) of the gas. This is typically around 1.4 for monoatomic ideal gases, but it would be helpful if you could confirm this.
Assuming γ = 1.4, we can use the formula for an adiabatic process:
T1 * V1^(γ-1) = T2 * V2^(γ-1)
Where: T1 = initial temperature V1 = initial volume T2 = final temperature V2 = final volume γ = heat capacity ratio
Given in the problem: T1 = T K V1 = 1 litre V2 = 2 litre
We can substitute these values into the formula and solve for T2:
T * (1 litre)^(1.4-1) = T2 * (2 litre)^(1.4-1)
Solving this equation will give us the final temperature T2 in Kelvin.
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