If an average person jogs, he produces $14.5 \times10^3$ cal/min. This is removed by the evaporation of sweat. The amount of sweat evaporated per minute (assuming $1$ kg requires $580 \times10^3$ cal for evaporation) is:

$1~\text g$ of water of volume $1~\text{cm}^3$ at $100^\circ \text{C}$ is converted into steam at the same temperature under normal atmospheric pressure $\approx 1\times10^{5}~\text{Pa}.$ The volume of  steam formed equals $1671~\text{cm}^3.$ If the specific latent heat of vaporization of water is $2256~\text{J/g},$ the change in internal energy is:
1. $2423~\text J$ 
2. $2089~\text J$ 
3. $167~\text J$ 
4. $2256~\text J$ 

The first law of thermodynamics is a statement of:
1. conservation of heat
2. conservation of work
3. conservation of momentum
4. conservation of energy

Consider the process on a system shown in the figure. During the process, the work done by the system:
           

An ideal gas goes from the state $i$ to the state $f$ as shown in figure given below. The work done by the gas during the process,

The molar specific heat at a constant pressure of an ideal gas is $\dfrac{7}{2}R.$ The ratio of specific heat at constant pressure to that at constant volume is: