Thermodynamics ...

When bulb of initial resistance $$R_{0}$$ is switch on its resistance increase due to heat production. Assuming initial temperature of bulb is $$0^{o}C$$. and temperature coefficient of bulb is $$\alpha$$. After what time its temperature will become $$T$$. (Heat capacity of bulb is $$'c'$$)

If $$C _ { V }$$ for an ideal gas is given by $$C _ { V } = 3 + 2 T, $$ where $$T$$ is the absolute temperature of the gas, then the equation of the adiabatic process for this gas is

Two moles of an ideal monoatomic gas occupies a volume V at $$27^0C$$. The gas expands adiabatically to a volume 2 V. Calculate (a) the final temperature of the gas and (b) change in its internal energy.

$$n$$ moles of a gas expands from volume $${V_1}\;to\;{V_2}$$ at constant temperature $$T$$. The work done by the gas is

Icc of water at $$ 100^o C $$ is given 540 cal of heat and the steam formed accupies 167 Icc at the atmospheric pressure. Then workdone against atmospheric pressure in this process is nearly.

The P - V diagram of a system undergoing a thermodynamic process is shown in figure. Work done by the system in going from $$A \rightarrow B \rightarrow C$$ is 30 J and 40 J heat is given to the system. The change in internal energy of the gas if the gas is directly taken from A to C  is 

The following sets of values for $$C_{v}$$ and $$C_{p}$$ of gas has been reported by different students. The units are $$cal/gm-mole-K$$. Which of these sets is most reliable 

A gas is compressed at a constant pressure of $$50 N/{ m }^{ 2 }$$ from a volume $$10{ m }^{ 3 }$$ to a volume of $$6 { m }^{ 3 }$$. $$100 J$$ of heat is added to the gas then its internal energy

A monoatomic gas is suddenly compressed to 1/8 th of its initial volume adiabactically. The ratio of its final pressure to initial pressure is (y=5/3)

P-V graph for a cyclic process is as shown. V-T graph for the process is [AB is isothermal and CA is an adiabatic process]