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.*
In an ideal gas at temperature $T,$ the average force that a molecule applies on the walls of a closed container depends on $T$ as $T^q$ . A good estimate for $q$ is
One mole of an ideal gas at $STP$ is heated in an insulated closed container until the average speed of its molecules is doubled. Its pressure would therefore increase by factor.
A horizontal uniform glass tube of $100 \,cm$, length sealed at both ends contain $10 \,cm$ mercury column in the middle. The temperature and pressure of air on either side of mercury column are respectively $81°C$ and $76\, cm$ of mercury. If the air column at one end is kept at $0°C$ and the other end at $273°C$, the pressure of air which is at $0°C$ is (in $cm$ of $Hg$)
Two thermodynamical process are shown in the figure. The molar heat capacity for process $A$ and $B$ are $C_A$ and $C_B$. The molar heat capacity at constant pressure and constant volume are represented by $C_P$ and $C_V$, respectively. Choose the correct statement.
If three moles of monoatomic gas $\left(\gamma=\frac{5}{3}\right)$ is mixed with two moles of a diatomic gas $\left(\gamma=\frac{7}{5}\right)$, the value of adiabatic exponent $\gamma$ for the mixture is:
Consider an ideal gas confined in an isolated closed chamber. As the gas undergoes an adiabatic expansion, the average time of collision between molecules increases as $V ^q$, where $V$ is the volume of the gas. The value of $q$ is $\left( {\gamma = \frac{{{C_P}}}{{{C_V}}}} \right)$
When the temperature of a gas is raised from $27^o C$ to $90^o C$, the percentage increase in the $r.m.s.$ velocity of the molecules will be ..... $\%$
The following graph represents the $T-V$ curves of an ideal gas (where $T$ is the temperature and $V$ the volume) at three pressures $P_1, P_2$ and $P_3$ compared with those of Charles's law represented as dotted lines.