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An open vessel at 27^(@)C is heated until three-fifths of the air in it has been expelled. Assuming the volume of the vessle remains constant, find the temperature to which the vessle has to be heated. |
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Answer» Solution :Suppose the volume of the vessel at `27^(@)C` is V containing N moles of the gas. LET the vessel be heated to T K when 2n/5 moles remain (as three-fifth has been EXPELLED). Since `(2n)/(5)` moles at T K OCCUPY a volume V, `therefore` n moles at T K should occupy `= (5V)/(2)`. Thus for n moles of the gas, `p_(1) = p ""p_(2) = p(p_(1) = p_(2) = p " as the vessel is open")` `V_(1) = V ""V_(2) = (5V)/(2)` `T_(1) = 300 K ""T_(2) = T K` `(pV)/(300) = (p xx (5V//2))/(T)` `T = 750 K = 477^(@)C`. |
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