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JEE Advanced · Physics · 13. Thermodynamics

One mole of an ideal monatomic gas undergoes an adiabatic expansion in which its volume becomes eight times its initial value. If the initial temperature of the gas is 100K and the universal gas constant R=8.0 J mol-1 K-1, then how much is the decrease in its internal energy (in J) ?

  1. A 1000
  2. B 1500
  3. C 900
  4. D 500
Verified Solution

Answer & Solution

Correct Answer

(C) 900

Step-by-step Solution

Detailed explanation

\(V_i=V\)
\(V_f=8 V\)
For adiabatic process \(\{\gamma=5 / 3\) for monoatomic gas \(\}\)
\(\begin{array}{l}T_1 \cdot V_1^{\gamma-1}=T_2 \cdot V_2^{\gamma-1} \\100(V)^{\frac{2}{3}}=T_2(8 V)^{\frac{2}{3}} \\T_2=25 K\end{array}\)
Loss in internal energy
\(\Delta U=n C_v \Delta T=1\left(\frac{f R}{2}\right)[100-25]=12\) \(\times~ 75=900 J\)
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