Use the ideal-gas equation of state to estimate the molar volume in $\mathrm{m}^{3} / \mathrm{mol}$ and the density of air in $\mathrm{kg} / \mathrm{m}^{3} \text { at } 40^{\circ} \mathrm{C}$ and a gauge pressure of 3.0 atm.

A fixed mass of an ideal gas is heated from 50 to $80^{\circ} \mathrm{C}$ at a constant volume of (a) 1 $m^3$ and (b) 3 $m^3$. For which case do you think the energy required will be greater? Why?

Complete the following table for an ideal gas. $$ \begin{array} & \text{P (atm)} & \text{V (L)} & \text{n (mol)} & \text{T}\\ \hline \text{0.300} & \text{2.00} & \text{ } & \text{155 K}\\ \end{array} $$

Complete the following table for an ideal gas.

$P (atm)$	$V (L)$	$n (mol)$	$T$
$6.74$	----	$2.00$	$155^{\circ}C$
$0.300$	$1.74$	----	$155 K$
$4.47$	$25.0$	$2.19$	---- $^{\circ}C$
----	$2.25$	$10.5$	$93 ^{\circ}C$

Complete the following table for an ideal gas.

$$\begin{matrix} \text{ } & \text{P (atm)} & \text{V (L)} & \text{n (mol)} & \text{T}\\ \hline \text{c.} & \text{4.47} & \text{25.0} & \text{2.01} & \text{ }\\ \end{matrix}$$

The flow of an ideal gas may be considered incompressible if the Mach number is less than 0.3. Determine the velocity level in ft/s and in m/s for Ma = 0.3 in the following gases: (a) standard air, (b) hydrogen at 68 $^{\circ} \mathrm{F}$.

Two ideal gases have the same mass density and the same absolute pressure. One of the gases is helium (He), and its temperature is 175 K. The other gas is neon(Ne). What is the temperature of the neon?

Indicate whether the following statements are true or false. Explain. An ideal gas (k = 1.4) has a velocity of 200 m/s, a temperature of 335 K, and a pressure of 8 bar. The corresponding stagnation temperature is less than 335 K.

The temperature of $1.75$ moles of an ideal gas increases from $10.2^{\circ} \mathrm{C}$ to $48.6^{\circ} \mathrm{C}$ as the gas is compressed adiabatically. Calculate $q, w, \Delta U$, and $\Delta H$ for this process, assuming that $C_{V, m}=3 R / 2$.

Complete the following table for an ideal gas. $$ \begin{array} & \text{P (atm)} & \text{V (L)} & \text{n (mol)} & \text{T}\\ \hline \text{ } & \text{2.25} & \text{ 10.5} & \text{$75^{\circ} \mathrm{C}$}\\ \end{array} $$

Using data from table, estimate the sonic velocity, in $\mathrm{m} / \mathrm{s}$, of steam at $60\ \text{bar}$, $360^{\circ} \mathrm{C}$. Compare the result with the value predicted by the ideal gas model.

A4-lbm mixture of 50% argon and 50% nitrogen by mole is in a tank at 300 psia, 320 R. How Large is the volume using a model of (a) ideal gas and (b) Kay’s rule with generalized compressibility charts?

An ideal gas expands to 10 times its original volume, maintaining a constant 440 K temperature. If the gas does 3.3 kJ of work on its surroundings,

(a) how much heat does it absorb, and

(b) how many moles of gas are there?

An ideal gas at 2500 kPa is throttled adiabatically to 150 kPa at the rate of $20 mol \cdot s^{–1}.$ Determine $\dot{S}_{G} \text { and } \dot{W}_{\text {lost }} \text { if } T_{\sigma}=300 \mathrm{K}$