Heating Ideal gas

Classical Mechanics Level 2

The above picture shows a monoatomic ideal gas in a cylinder being heated under the constant pressure of 1 × 1 0 5 1\times 10^5 Pa. At the initial state before heating, the temperature and volume of the ideal gas were 300 300 K and 1 × 1 0 − 3 m 3 1\times 10^{-3} \text{ m}^3 , respectively. After heating, its volume has become 3 × 1 0 − 3 m 3 . 3 \times 10^{-3} \text{ m}^3. Which of the following statements is correct?

a) The temperature of the ideal gas after heating is 600 600 K.

b) The work done by the ideal gas is 200 200 J.

c) The heat absorbed by the ideal gas is 500 500 J.

b) and c) c) only a) and b) a) only

Lakshan Dumpa by Lakshan Dumpa , 24, India

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1 solution

Arijit Banerjee
Apr 15, 2014

option B is possible becoz we knw Work done = Pressure * Change in volume = 10^5 * 2 * 10^-3 = 200J . Then option A is not possible becoz if we apply this frmula . .. initial Volume / initial temperature = Final Vol /final temp ... we get final temp as 900K ... I didn't calculate the heat absorbed ... there r only two options containing B so the one with A is getting eliminated so answer is B and C... :D I cudn calculate heat absorbed sorry!

2 Helpful 0 Interesting 0 Brilliant 0 Confused

Heat absorbed at constant pressure is equal to nCp(T2-T1). with Cp = R (Y/Y-1). for monoatomic ideal gas Y = 1 + (2/3) . Using the above formula we get the heat absorbed to be 500J. The truthfulness of Option B is explained above

Srivatsav Viswanadha - 7 years, 1 month ago

Same here.... I don't know how to calculate heat absorbed

aditya mahadik - 7 years ago

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