Question 3 :
Which of the following is not the component of heat pump?<br><br>

Question 4 :
Diffusion of a gas in a room is not reversible because:

Question 5 :
In an adiabatic expansion, the temperature of 5 moles of gas $\gamma =1.5$ falls from $87^{0}C$ to $27^{0}C$, then the work done is<br>

Question 8 :
A new soft drink bottle is opened, allowing gas to escape into the atmosphere. As the gas escapes, its degree of disorder increases.&#160;Identify by which of the following law this can be explained ?

Question 9 :
During what kind of process is there no change in internal energy?

Question 11 :
An automobile engine absorbs $1600 \ J$ of heat from a hot reservoir and expel $1000\ J$ to a cold reservoir in each cycle. What maximum work is done in each cycle?

Question 12 :
When the temperature of an iron sphere of mass $1\ kg$ falls from $30 ^oC$ &#160;to $25 ^oC$ , then $550\ cal$ of heat is released. The heat capacity of the iron sphere will be ( in $cal ^o\ C^{-1}$ )

Question 13 :
During an adiabatic process, the pressure of a&#160;gas is proportional to the cube of its adiabatic&#160;temperature. The value of&#160; $\dfrac {C_{p}}{C_{v}}$ for that gas is :<br/>

Question 15 :
The ratio of densities of two substances is 2 : 3 and that of specific heats is 1 : 2. The ratio of thermal capacities per unit volume is<br>

Question 17 :
A cycle pump becomes hot near the nozzle after a few quick strokes even if they are smooth because

Question 18 :
We consider a thermodynamic system. If $\bigtriangleup U$ represents the increase in its internal energy and W the work done by the system. Which of the following statments is true

Question 19 :
On an isothermal process, there are two points $A$ and $B$ at which pressures and volumes are $(2P_o,\:V_o)$ and $(P_o,\:2V_o)$ respectively. If $A$ and $B$ are connected by a straight line, find the pressure at a POINT on this straight line at which temperature is maximum

Question 21 :
Assertion: In adiabatic expansion, temperature of gas always decreases. Reason: In adiabatic process exchange of heat is zero.

Question 22 :
At $27^{o}C$ a gas is compressed suddenly such that its pressure becomes ($\dfrac{1}{8}$)th of original pressure. Final temperature will be ($\gamma$ = 5/3)

Question 23 :
An ideal heat engine working between temperature T and T has an efficiency&#160;$\eta $, the new efficiency if both the source and sink temperature are doubled, will be

Question 25 :
A certain amount of heat is required to raise the temperature of $x\ g$ of a substance through $t_1 ^oC$. The same amount of heat when taken away from $y\ g$ of water, it cools through $t_2 ^oC$.Therefore, the specific heat of the substance is

Question 27 :
During the adiabatic change of ideal gas, The relation between the pressure and the density will be -

Question 28 :
The thermal capacity of a body is 80 cal, then its water equivalent is

Question 29 :
$200\ g$ mass of a certain metal at $83^{\circ}C$ is immersed in $300\ g$ of water of $30^{\circ}C$. Final temperature of combination is $33^oC$.Calculate the specific heat capacity of metal. Assume that the specific heat capacity of water is $4.2 J g^{-1} K^{-1}$

Question 30 :
A diatomic gas does $80\ J$ of work when expanded isobarically. The heat given to the gas during this process is

Question 31 :
Efficiency of a heat engine whose sink is at a temperature of $300 \ K$ is $40$%. To increase the efficiency to $60$%, keeping the sink temperature constant, the source temperature must be increased by :<br/>

Question 32 :
A cylinder of mass $1$kg is given heat of $20000$J at atmospheric pressure. If initially temperature of cylinder is $20^o$C, find change in internal energy of the cylinder.<br>(Given that Specific heat capacity of cylinder $=400$J $kg^{-1}$ $^0C^{-1}$, Coefficient of volume expansion $=9\times 10^{-5}$ $^0C^{-1}$, Atmospheric pressure $=10^5$ $N/m^2$ and Density of cylinder $=9000$ $kg/m^3$).<br>

Question 33 :
Piston cylinder device initially contains $0.5 m^3$ of nitrogen gas at $400 kPa$ and $27^o$C. An electric heater within the device is at turned on and is allowed to pass a current of $2 A$ for $5 \ min$ from a $120 V$ source. Nitrogen expands at constant pressure and a heat loss of $2800 J$ occurs during the process.<br/>$R = \dfrac{25}{3} kJ/kmol-K$The final temperature of nitrogen is:

Question 34 :
A gas in a cylinder held at a constant pressure of $1.7\,\times\, 10^{5}$ Pa and is cooled and compressed from $1.20\, m^{3}\, to\,&#160;0.8\, m^{3}$. The internal energy of the gas decreses by $1.1\, \times\, 10^{5}$ J.<br/>Does it matter whether or not the gas is ideal? Mark 1-&gt;Yes and 0-&gt;No

Question 35 :
If three different liquid of different masses specific heats and temperature are mixed with each other then what is the temperature of the mixture at thermal equilibrium. If,<br/>$m_1,\,s_1,\,T_1\rightarrow$ specification for liquid<br/>$m_2,\,s_2,\,T_2\rightarrow$ specification for liquid<br/>$m_3,\,s_3,\,T_3\rightarrow$ specification for liquid

Question 36 :
In a particular experiment, a gas undergoes adiabatic expansion satisfying the equation $\displaystyle { VT }^{ 3 }$=constant. The ration of specific heats, $\displaystyle Y $ is:

Question 37 :
In a thermodynamic processes, If the amount of work done on the gas by its surrounding is 320 J and the internal energy is increased by 560 J. Calculate the how much heat is transferred between the gas and its surrounding.

Question 38 :
Three black bodies $A , B$ and $C$ in the form of cubes of sides in the ratio of $3 : 4 : 5$ are kept at the same high temperature. The ratio of the quantity of heat lost per second by $A , B$ and $C$ will be

Question 39 :
Water of mass $m_2$ = 1 kg is contained in a copper calorimeter of mass&#160;$m_1$&#160;&#160;= 1 kg. Their common temperature&#160;t = $10^{0}C$. Now a piece of ice of mass&#160;$m_3$&#160;&#160;= 2 kg and temperature is $-11^{0}C$&#160;dropped into the calorimeter.&#160;Neglecting any heat loss, the final temperature of system is. [specific heat of copper = 0.1 Kcal/ kg$^{0}C$, specific&#160;heat of water = 1 Kcal/kg$^{0}C$, specific heat of ice = 0.5 Kcal/kg$^{0}C$, latent heat of fusion of ice = 78.7 Kcal/kg]