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5.6 litre of an unknown gas at NTP requires 12.5 calorie to raise its temperature by $10^{\large\circ}C$ at constant volume. Calculate the $C_v$ of the gas.

$(a)\;3\;calorie\qquad(b)\;5\;calorie\qquad(c)\;7\;calorie\qquad(d)\;9\;calorie$

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1 Answer

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Given
Volume = 5.6 litre
R = 0.0821
T = 273K
We have $n = \large\frac{PV}{RT}$
$=\large\frac{1\times5.6}{0.0821\times273}$
= 0.25
Also $q = mS\bigtriangleup T$
$12.5 = 0.25\times C_v\times10$
$C_v = 5\;calorie$
Hence answer is (b)
answered Feb 16, 2014 by sharmaaparna1
 

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