Thermodynamics ...

Which of the following statements is incorrect?

In a cylinder, $$2.0 \ moles$$ of an ideal monatomic gas initially at $$1.0 \times 10^6 \ Pa$$ and $$300 K$$ expands until its volume doubles. The work done if the expansion is isobaric is

Electric work done on the nitrogen gas is

Two moles of an ideal gas at temperature $$T_o = 300 K$$ was cooled isochorically so that the pressure was reduced to half. Then, in an isobaric process, the gas expanded till its temperature got back to the initial value. The total amount of heat absorbed by the gas in the process is:

In an adiabatic process, the pressure is increased by$$\frac{2}{3}$$%. If $$\gamma =\frac{3}{2}$$, then the volume decreases by nearly:

As a result of isobaric heating by $$\Delta T = 72 K$$, one mole of certain ideal gas obtains an amount of heat $$Q = 1.60 kJ$$. The value of $$\gamma$$ is

An ideal gas initially at $$30 K$$ undergoes an isobaric expansion at $$2.50 \  kPa$$. If the volume increases from $$1.00 m^3$$ to $$3.00 m^3$$ and $$12.5 \ kJ$$ is transferred to the gas by heat,what are its final temperature?

In the following pressure-volume diagram, the isochoric, isothermal and isobaric parts, respectively, are

Figure shows four PV diagrams. Which of these curves represent isothermal and adiabatic processes respectively?

A gas is at $$1\:atm$$ pressure with a volume $$800\:cm^3$$. When $$100\:J$$ of heat is supplied to the gas, it expands to $$1\:L$$ at constant pressure. The change in its internal energy is