Two moles of a monoatomic ideal gas is confined in a container and is heated such that its temperature increases by $10\,^oC$. The approximate change in its internal energy is ..... $J$. $(R = 8.31\, J/mole-K)$
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A mixture of $2$ moles of helium gas (atomic mass $=4 \ amu$ ), and $1$ mole of argon gas (atomic mass $=40 \ amu$ ) is kept at $300 \ K$ in a container. The ratio of the rms speeds $\left(\frac{\left. v _{ mms } \text { (helium }\right)}{ v _{\text {rms }} \text { (argon) }}\right)$ is :
A hydrogen cylinder is designed to withstand an internal pressure of $100 \,atm$. At $27^{\circ} C$, hydrogen is pumped into the cylinder which exerts a pressure of $20 \,atm$. At what temperature does the danger of explosion first sets in ......... $K$
The temperature of an open room of volume $30\ m^3$ increases from $17^o C$ to $27vC$ due to sunshine. The atmospheric pressure in the room remains $1 \times 10^5\ Pa$. Ifni and nr are the number of molecules in the room before and after heating, then $n_f-n_i$ will be :
At $300\,K$, the rms speed of oxygen molecules is $\sqrt{\frac{\alpha+5}{\alpha}}$ times to that of its average speed in the gas. Then, the value of $\alpha$ will be (used $\pi=\frac{22}{7}$ )
The specific heats, $C_P$ and $C_V$ of a gas of diatomic molecules, $A$, are given (in units of $J\, mol^{-1}\, K^{-1}$) by $29$ and $22$, respectively. Another gas of diatomic molecules $B$, has the corresponding values $30$ and $21$. If they are treated as ideal gases, then
A sample of an ideal gas occupies a volume $V$ at a pressure $P$ and absolute temperature $T,$ the mass of each molecule is $m.$ The expression for the density of gas is ($k =$ Boltzmann’s constant)
The temperature of the mixture of one mole of helium and one mole of hydrogen is increased from ${0^o}C$ to ${100^o}C$ at constant pressure. The amount of heat delivered will be ...... $cal$