For a solid with a small expansion coefficient,
1. Cp - CV = R
2. Cp = CV
3. Cp is slightly greater than CV
4. Cp is slightly less than CV
The value of Cp – CV is 1.00 R for a gas sample in state A and is 1.08 R in state B. Let pA , pB denote the pressures and TA and TB denote the temperatures of the states A and B respectively. Most likely
1. pA < pB and TA > TB
2. pA > pB and TA < TB
3. pA = PB and TA < TB
4. pA > pB and TA = TB
The figure shows a process on a gas in which pressure and volume both change. The molar heat capacity for this process is C.
1. C = 0
2. C = CV
3. C > CV
4. C < CV
The molar heat capacity for the process shown in the following figure is:
1. C = Cp
2. C = Cv
3. C > CV
4. C =0
In an isothermal process on an ideal gas, the pressure increases by 0.5%. The volume decreases by about
1. 0.25%
2. 0.5%
3. 0.7%
4. 1%.
In an adiabatic process on a gas with y = 1.4, the pressure is increased by 0.5%. The volume decreases by about
1. 0.36%
2. 0.5%
3. 0.7%
4. 1%.
Two samples A and B are initially kept in the same state. The sample A is expanded through an adiabatic process and the sample B through an isothermal process. The final volumes of the samples are the same. The final pressures in A and B are pA and pB respectively.
1. PA > PB
2. PA = PB
3. PA < PB
4. The relation between pA and pB cannot be deduced.
Let Ta and Tb be the final temperatures of the samples A and B respectively in the previous question.
1. Ta < Tb
2. Ta = Tb
3. Ta > Tb
4. The relation between Ta and Tb cannot be deduced.
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