Isothermal and Adiabatic Processes Numerical on Molar Specific Heat Class-11 Physics

Isothermal and Adiabatic Processes Numerical on Molar Specific Heat Class-11 Nootan ISC Physics Solutions Ch-20. Step by step solutions of Kumar and Mittal Physics of Nageen Prakashan as council latest prescribe guideline for upcoming exam. Visit official Website CISCE  for detail information about ISC Board Class-11 Physics.

Isothermal and Adiabatic Processes Numerical on Molar Specific Heat Class-11

(Nootan ISC Physics Solutions Ch-20)

Board	ISC
Class	11
Subject	Physics
Book	Nootan
Chapter-20	Isothermal and Adiabatic Processes
Topics	Numerical on Molar Specific Heat
Academic Session	2024-2025

Isothermal and Adiabatic Processes Numerical on Molar Specific Heat

page-780

Que-14: 0.5 mole CO2 is heated from 25°C to 125°C at constant pressure. If Cp = 8.0 Cal / mol-°C and Cv = 6.0 Cal / mol-°C for CO2, then calculate (i) amount of heat given to the gas, (ii) increase in the internal energy of the gas.

Ans: Cp – Cv = R

=> μ Cp ΔT – μ Cv ΔT = R ΔT

=> ΔQ – ΔU = R ΔT

=> ΔQ = 0.5 x 8 x 100 = 400 Cal

ΔU = μ Cv ΔT = 0.5 (Cp – R) ΔT

=> 0.5  x (8 – 2) x 100 = 300 Cal

Que-15: 0.1 mole nitrogen is heated from 27°C to 327°C at constant pressure. Determine the heat given to the gas, increase in internal energy of the gas and work done by the gas. For nitrogen Cp = 7 and C, = 5 Cal / mol-°C

Ans: ΔQ = μ Cp ΔT

=> 0.1 x 7 x 300 = 210 Cal

ΔU = μ Cv ΔT

=> 0.1 (7 – 2) x 300 = 150 Cal

ΔW = μ R ΔT

=> 0.1 x 2 x 300 = 60 Cal

Que-16: Calculate the amount of heat required to raise the temperature of two moles of an ideal monoatomic gas from 0°C to 100°C if no work is done. You are given that the molar specific heat of the above gas at constant pressure is 2.5 R, where R is the universal gas constant (R = 8.3 J / mol-K).

Ans: ΔQ = μ Cv ΔT

=> 2 x (Cp – R) ΔT

=> 2 x (2.5 R – R) x ΔT

=> 2 x 1.5 R x ΔT

=> 2 x 1.5 x 8.31 x 100

=> 2490 J

-— : end of Isothermal and Adiabatic Processes Numerical on Molar Specific Heat ISC Physics Solutions  :–

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