Experience the future of education. Simply download our apps or reach out to us for more information. Let's shape the future of learning together!No signup needed.*
$1c{m^3}$ of water at its boiling point absorbs $540$ calories of heat to become steam with a volume of $1671c{m^3}$.If the atmospheric pressure = $1.013 \times {10^5}N/{m^2}$ and the mechanical equivalent of heat = $4.19J/calorie$, the energy spent in this process in overcoming intermolecular forces is ..... $cal$
The volume of $1\; mole$ of an ideal gas with the adiabatic exponent $\gamma$ is changed according to the relation $V=\frac bT$ where $b =$ constant. The amount of heat absorbed by the gas in the process if the temperature is increased by $\triangle T$ will be
An ideal gas at a pressures of $1$ atmosphere and temperature of ${27^o}C$ is compressed adiabatically until its pressure becomes $8$ times the initial pressure, then the final temperature is ..... $^oC$ ($\gamma = 3/2$)
A sample of an ideal gas is contained in a cylinder. The volume of the gas is suddenly decreased. A student makes the following statements to explain the change in pressure of the gas
$I.$ The average kinetic energy of the gas atoms increases
$II.$ The atoms of the gas hit the walls of the cylinder more frequently
$III.$ Temperature of the gas remains unchanged
Which of these statements is true?
An ideal gas goes from state $A$ to state $B$ via three different processes as indicated in the $P-V$ diagram. If $Q_1, Q_2, Q_3$ indicate the heat absorbed by the gas along the three processes and $\Delta U_1, \Delta U_2, \Delta U_3$
indicate the change in internal energy along the three processes respectively, then
A system is given $300$ calories of heat and it does $600$ joules of work. How much does the internal energy of the system change in this process ..... $J$. ($J = 4.18$ joules/cal)