Explain why the noble gases tend not to react.

The following table presents the solubilities of several gases in water at $25^{\circ} \mathrm{C}$ under a total pressure of gas and water vapor of 1 atm.

(a) What volume of $\mathrm{CH}_4(g)$ under standard conditions of temperature and pressure is contalned in $4.0 \mathrm{I}$ of a saturated solution at $25^{\circ} \mathrm{CZ}$

Most gases become more soluble in liquid as the temperature........

(a) find the equilibrium points of the system, (b) using HPGSystemSolver, sketch the direction field and phase portrait of the system, and (c) briefly describe the behavior of typical solutions.

$$\frac{d x}{d t}=y\left(x^2+y^2-1\right)$$

$$\frac{d y}{d t}=-x\left(x^2+y^2-1\right)$$

An equilibrium mixture of car exhaust gases consisting of $10.0$ volumes of $\mathrm{CO}_2, 1.00$ volume of unreacted $\mathrm{O}_2$, and $50.0$ volumes of unreacted $\mathrm{N}_2$ leaves the engine at $4.0 \mathrm{~atm}$ and $800 . \mathrm{K}$.
(a) Given this equilibrium, what is the partial pressure of $\mathrm{CO}$ ? $2 \mathrm{CO}_2(\mathrm{~g}) \rightleftharpoons 2 \mathrm{CO}(\mathrm{g})+\mathrm{O}_2(\mathrm{~g}) \quad K_{\mathrm{p}}=1.4 \times 10^{-28}$ at $800 . \mathrm{K}$

What is the relationship between fossil fuels and greenhouse gases?

Gaseous indium dihydride is formed from the elements at elevated temperature:

$$\ln (g)+\mathrm{H}_2(g) \rightleftharpoons \ln _2(g) \quad K_{\mathrm{p}}=1.48 \text { at } 973 \mathrm{~K}$$

Partial pressures measured in a reaction vessel are: $P_{\mathrm{ln}}=0.0600 \mathrm{~atm}, P_{\mathrm{H}_2}=0.0350 \mathrm{~atm}, P_{\mathrm{lnH}_2}=0.0760 \mathrm{~atm}$.
(a) Calculate $Q_p$, and determine the direction of reaction to attain equilibrium.
(b) Determine the equilibrium partial pressures of all the gases.

__________List the following gases in order of increasing rate of effusion. (Assume all gases are at the same temperature and pressure.)

(a) $\mathrm{He}$

(b) $\mathrm{Xe}$

(c) $\mathrm{HCl}$

(d) $\mathrm{Cl}_2$

Although Mendeleev predicted the existence of several undiscovered elements, he did not predict the existence of the noble gases, the lanthanides, or the actinides. Propose reasons why Mendeleev was not able to predict the existence of the noble gases.

Charles's law was discovered by Joseph Louis GayLussac in 1802, based on unpublished work done by Jacques Charles in about 1787. Charles had found that a number of gases expand to the same extent over the same $80^{\circ}$ temperature interval. You will be observing the relationship between the temperature and volume of a gas similar to that studied by Charles.

When solid ammonium carbamate sublimes, it dissociates completely into ammonia and carbon dioxide according to the following equation:

$$\begin{align*} \left(\mathrm{NH}_4\right)\left(\mathrm{H}_2 \mathrm{NCO}_2\right)(\mathrm{s}) \rightleftharpoons 2 \mathrm{NH}_3(\mathrm{~g})+\mathrm{CO}_2(\mathrm{~g}) \end{align*}$$

At $25^{\circ} \mathrm{C}$, the experiment shows that the total pressure of the gases in equilibrium with the solid is $0.116 \mathrm{~atm}$. What is the equilibrium constant, $K_{\mathrm{p}}$?

Write equilibrium constant expressions for the following reactions. For gases, use either pressures or concentrations.\

$$\left(\mathrm{NH}_4\right)_2 \mathrm{CO}_3(\mathrm{~s}) \rightleftarrows 2 \mathrm{NH}_3(\mathrm{~g})+\mathrm{CO}_2(\mathrm{~g})+\mathrm{H}_2 \mathrm{O}(\mathrm{g})$$

Explain why the noble gases are unreactive.

A sealed glass bulb contains a mixture of $\mathrm{NO}_2$ and $\mathrm{N}_2 \mathrm{O}_4$ gases. Describe what happens to the following properties of the gases when the bulb is heated from $20^{\circ} \mathrm{C}$ to $40^{\circ} \mathrm{C}$ :

(a) color,

(b) pressure,

(c) average molar mass,

(d) degree of dissociation (from $\mathrm{N}_2 \mathrm{O}_4$ to $\mathrm{NO}_2$ ),

(e) density. Assume that volume remains constant. (Hint: $\mathrm{NO}_2$ is a brown gas; $\mathrm{N}_2 \mathrm{O}_4$ is colorless.)