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An ideal heat engine exhausting heat at 27°C have
40% efficiency. Then it takes heat from a reservoir at
(1) 127°C
(2) 227°C
(3) 327°
(4) 427°

Which is correct?
(1) In an adiabatic process pressure, volume and
temperature all changes
(2) An adiabatic process may be a fast process
(3) An adiabatic process may be a slow process
(4) An isothermal process is a fast process

The work done in an isothermal process in a
particular gas depends upon only
(1) Volume change
(2) Pressure change
(3) Change in internal energy
(4) On both (1) & (2)

Specific heat of a substance during isothermal
process is
(1) Infinite
(2) Zero
(3) Positive
(4) Negative

If the temperature of source & sink in heat engine is
at 1000 K & 500 K respectively, then efficiency
can be
(1) 20%
(2) 30%
(3) 50%
(4) All of these

$\frac{\mathrm{Slope} \mathrm{of} \mathrm{isothermal} \mathrm{curve}}{\mathrm{slope} \mathrm{of} \mathrm{adiabatic} \mathrm{curve}}$ is equal to 
1. 1
2. $\frac{1}{2}$
3. $\mathrm{\gamma }$
4. $\frac{1}{\mathrm{\gamma }}$

In an adiabatic process, work done versus change of
temperature $∆$T is

According to the figure select the correct statement

(1) The work in this process greater than isothermal
process between A & B
(2) The corresponding V - T curve is a parabola
(3) Both (1) & (2) are correct
(4) Only (2) is correct

The volume and temperature graph is given in the figure below. If pressures for the two processes are different, then which one,  of the following, is true?
        

In a thermodynamical system for a diatomic gas
V versus T graph is as shown below. The ratio of
heat absorbed to work done is

1. $\frac{7}{2}$
2. $\frac{2}{5}$
3. $\frac{3}{5}$
4. $\frac{5}{3}$

In isochoric process, which of the following is
correct?

n moles of an ideal gas is heated at constant pressure
from 50°C to 100°C, the increase in internal energy
of the gas is $\left(\frac{{\mathrm{C}}_{\mathrm{p}}}{{\mathrm{C}}_{\mathrm{v}}}=\mathrm{\gamma } \mathrm{and} \mathrm{R}=\mathrm{gas} \mathrm{constant}\right)$
1. $\frac{50 \mathrm{nR}}{\mathrm{\gamma }-1}$
2. $\frac{100 \mathrm{nR}}{\mathrm{\gamma }-1}$
3. $\frac{50 \mathrm{n\gamma R}}{\mathrm{\gamma }-1}$
4. $\frac{25 \mathrm{n\gamma R}}{\mathrm{\gamma }-1}$

In an adiabatic expansion of O2 gas the volume
increased by 1.0%, the percentage change in
pressure is
(1) 1.0%
(2) 0.7%
(3) 1.4%
(4) 1.7%

One mole of an ideal diatomic gas expands
adiabatically. Work done by the gas as its
temperature changes from T₁ to T₂ is
1. $\frac{5}{2}R\left(T_1-T_2\right)$
2. $\frac{5}{2}R\left(T_2-T_1\right)$
3. $\frac{3}{2}R\left(T_1-T_2\right)$
4. $\frac{3}{2}R\left(T_2-T_1\right)$

In an isochoric process of an ideal diatomic gas,
100 J heat is supplied. The work done by the gas is
(1) 100 J
(2) 60 J
(3) 40 J
(4) Zero

In an adiabatic process, work done by the gas is
15 R (R is gas constant). The increase in internal
energy of the gas is $\left(\mathrm{\gamma }=\frac{5}{3}\right)$
(1) 15 R
(2) –15 R
(3) 25 R
(4) –25 R

Gas within a closed chamber undergoes the
processes shown in the PV diagram. The net heat
added to the system during one complete cycle is

(1) 2 J
(2) –2 J
(3) 9 J
(4) – 9 J

A gas kept in an open vessel exposed to atmospheric
pressure is heated to double its temperature. If initially
there were n moles in the vessel, then the number of
moles in the vessel after heating will be
(1) Remain same
(2) Become half
(3) Become double
(4) Becomes 1.5 times

Which of the following graph represents adiabatic
expansion of a gas on V-T graph?

Figure shows P-V graph for an ideal gas. Select the
correct alternative.

(1) If AB is isothermal, AC may be adiabatic
(2) If AB is adiabatic, AC may be isothermal
(3) Both AB and AC are isothermal
(4) Both AB and AC are adiabatic