10. At constant volume (-0.01m') the pressure of 1g of Hydrogen is increased from 1.0X10' Pa to 2.0 X 10³ Pa. Using Ideal gas equation find out the initial and final temperatures. Use first law of thermodynamics to calculate the heat required during the above process. (Assume the molecular weight of Hydrogen-2; Hydrogen is a diatomic gas)
10. At constant volume (-0.01m') the pressure of 1g of Hydrogen is increased from 1.0X10' Pa to 2.0 X 10³ Pa. Using Ideal gas equation find out the initial and final temperatures. Use first law of thermodynamics to calculate the heat required during the above process. (Assume the molecular weight of Hydrogen-2; Hydrogen is a diatomic gas)
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Transcribed Image Text:10. At constant volume (-0.01m') the pressure of 1g of Hydrogen is increased from 1.0X10 Pa
to 2.0 X 10³ Pa. Using Ideal gas equation find out the initial and final temperatures.
Use first law of thermodynamics to calculate the heat required during the above process..
(Assume the molecular weight of Hydrogen-2; Hydrogen is a diatomic gas)
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