In the Deacon process for the manufacture of chlorine, HCl and $\mathrm{O}_{2}$ to form $\mathrm{Cl}_{2} \text { and } \mathrm{H}_{2} \mathrm{O}$. Sufficient air $\left(21 \mathrm{mole} \% \mathrm{O}_{2}, 79 \% \mathrm{N}_{2}\right)$ is fed to provide 35% excess oxygen, and the fractional conversion of HCl is 85%. a) Calculate the mole fractions of the product stream components, using atomic species balances in your calculation. b) Again calculate the mole fractions of the product stream components, only this time use the extent of reaction in the calculation. c) An alternative to using air as the oxygen source would be to feed pure oxygen to the reactor. Running with oxygen imposes a significant extra process cost relative to running with air, but also offers the potential for considerable savings. Speculate on what the cost and savings might be. What would determine which way the process should be run?

Nitric acid is produced commercially by the Ostwald process. In the first step ammonia is oxidized to nitric oxide:

$$4 \mathrm{NH}_3(g)+5 \mathrm{O}_2(g) \longrightarrow 4 \mathrm{NO}(g)+6 \mathrm{H}_2 \mathrm{O}(g)$$

The stopcock between the two reaction containers is opened, and the reaction proceeds using proper catalysts. Calculate the partial pressure of $\mathrm{NO}$ after the reaction is complete. Assume $100 \%$ yield for the reaction, assume the final container volume is $3.00 \mathrm{~L}$, and assume the temperature is constant.

The Deacon process for producing chlorine gas from hydrogen chloride is used in situations where $\mathrm{HCl}$ is available as a by-product from other chemical processes.

$$\begin{aligned} 4 \mathrm{HCl}(\mathrm{g})+\mathrm{O}_2(\mathrm{~g}) \rightleftharpoons 2 \mathrm{H}_2 \mathrm{O}(\mathrm{g}) &=2 \mathrm{Cl}_2(\mathrm{~g}) \\ \Delta_{\mathrm{r}} \mathrm{H}^{\circ} &=-114 \mathrm{~kJ} \mathrm{~mol}^{-1} \end{aligned}$$

A mixture of $\mathrm{HCl}, \mathrm{O}_2, \mathrm{H}_2 \mathrm{O}$, and $\mathrm{Cl}_2$ is brought to equilibrium at $400^{\circ} \mathrm{C}$. What is the effect on the equilibrium amount of $\mathrm{Cl}_2(\mathrm{~g})$ if
(e) the temperature is raised to $500^{\circ} \mathrm{C}$ ?

The Deacon process for producing chlorine gas from hydrogen chloride is used in situations where $\mathrm{HCl}$ is available as a by-product from other chemical processes.

$$\begin{aligned} 4 \mathrm{HCl}(\mathrm{g})+\mathrm{O}_2(\mathrm{~g}) \rightleftharpoons 2 \mathrm{H}_2 \mathrm{O}(\mathrm{g}) &=2 \mathrm{Cl}_2(\mathrm{~g}) \\ \Delta_{\mathrm{r}} \mathrm{H}^{\circ} &=-114 \mathrm{~kJ} \mathrm{~mol}^{-1} \end{aligned}$$

A mixture of $\mathrm{HCl}, \mathrm{O}_2, \mathrm{H}_2 \mathrm{O}$, and $\mathrm{Cl}_2$ is brought to equilibrium at $400^{\circ} \mathrm{C}$. What is the effect on the equilibrium amount of $\mathrm{Cl}_2(\mathrm{~g})$ if
(d) a catalyst is added to the reaction mixture?

Chlorine is produced by the reaction: $4 \mathrm{HCl}(g)+\mathrm{O}_{2}(g) \rightarrow 2 \mathrm{H}_{2} \mathrm{O}(g)+2 \mathrm{Cl}_{2}(g)$ The feed stream to the reactor consists of 60 mol-% HCl, 36 mol-% $O_2,$ and 4 mol-% $N_2,$ and it enters the reactor at $550^\circ C.$ If the conversion of HCl is 75% and if the process is isothermal, how much heat must be transferred to or from the reactor per mole of the entering gas mixture?

Plot the polynomial $y = 0.1 x ^ { 5 } - 0.2 x ^ { 4 } - x ^ { 3 } + 5 x ^ { 2 } - 41.5 x + 235$ in the domain $- 6 \leq x \leq 6 .$ First create a vector for $x ,$ next use the polyval function to cal- culate $y ,$ and then use the plot function.

The Deacon process for producing chlorine gas from hydrogen chloride is used in situations where $\mathrm{HCl}$ is available as a by-product from other chemical processes.

$$\begin{aligned} 4 \mathrm{HCl}(\mathrm{g})+\mathrm{O}_2(\mathrm{~g}) \rightleftharpoons 2 \mathrm{H}_2 \mathrm{O}(\mathrm{g}) &=2 \mathrm{Cl}_2(\mathrm{~g}) \\ \Delta_{\mathrm{r}} \mathrm{H}^{\circ} &=-114 \mathrm{~kJ} \mathrm{~mol}^{-1} \end{aligned}$$

A mixture of $\mathrm{HCl}, \mathrm{O}_2, \mathrm{H}_2 \mathrm{O}$, and $\mathrm{Cl}_2$ is brought to equilibrium at $400^{\circ} \mathrm{C}$. What is the effect on the equilibrium amount of $\mathrm{Cl}_2(\mathrm{~g})$ if
(a) additional $\mathrm{O}_2(\mathrm{~g})$ is added to the mixture at constant volume?

The Deacon process for producing chlorine gas from hydrogen chloride is used in situations where $\mathrm{HCl}$ is available as a by-product from other chemical processes.

$$\begin{aligned} 4 \mathrm{HCl}(\mathrm{g})+\mathrm{O}_2(\mathrm{~g}) \rightleftharpoons 2 \mathrm{H}_2 \mathrm{O}(\mathrm{g}) &=2 \mathrm{Cl}_2(\mathrm{~g}) \\ \Delta_{\mathrm{r}} \mathrm{H}^{\circ} &=-114 \mathrm{~kJ} \mathrm{~mol}^{-1} \end{aligned}$$

A mixture of $\mathrm{HCl}, \mathrm{O}_2, \mathrm{H}_2 \mathrm{O}$, and $\mathrm{Cl}_2$ is brought to equilibrium at $400^{\circ} \mathrm{C}$. What is the effect on the equilibrium amount of $\mathrm{Cl}_2(\mathrm{~g})$ if
(c) the mixture is transferred to a vessel of twice the volume?

A mining company is considering a new project. Because the mine has received a permit, the project would be legal; but it would cause significant harm to a nearby river. The firm could spend an additional $10 million at Year 0 to mitigate the environmental problem, but it would not be required to do so. Developing the mine (without mitigation) would cost$60 million, and the expected cash inflows would be $20 million per year for 5 years. If the firm does invest in mitigation, the annual inflows would be$21 million. The risk-adjusted WACC is 12%. a. Calculate the NPV and IRR with and without mitigation. b. How should the environmental effects be dealt with when this project is evaluated? c. Should this project be undertaken? If so, should the firm do the mitigation?

The reaction between ethylene and hydrogen bromide to form ethyl bromide is carried out in a continuous reactor. The product stream is analyzed and found to contain 51.7 mole% $\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{Br}$ and 17.3% HBr. The feed to the reactor contains only ethylene and hydrogen bromide. Calculate the fractional conversion of the limiting reactant and the percentage by which the other reactant is in excess. If the molar flow rate of the feed stream is 165 mol/s, what is the extent of reaction?

Choose a word to replace the italicized word in each sentence. All of the possible choices for each sentence have similar definitions, but the correct answer will have a connotation that best suits the context. For example, the words "delete," "destroy," and "obliterate" all mean "to remove or wipe out," but no one would ever say, "I destroyed the name from the document." The correct choice will be the word that has the best specific meaning and does not render the sentence awkward in tone or content. When chokes seem close, look for a clue in the context that makes one choice better than the other. Note that the correct answer is not always the primary vocabulary word from the lesson.

$$\begin{matrix} \text{lackeys} & \text{nervous} & \text{dead} & \text{impelled}\\ \text{uncontrollable} & \text{defunct} & \text{creative} & \text{slaves}\\ \text{moved} & \text{companions} & \text{judicious} & \text{cruel}\\ \text{insecure} & \text{} & \text{} & \text{}\\ \end{matrix}$$

 The company was once the largest manufacturer of steam boilers in the world, but it failed to adapt to new technology and is now invalid. Better word: _______

If $a^{2}=b$ and a > 0, then a is the (negative square root, principal square root) of b.

Simplify the radical expression.

$$\sqrt{3 x} \cdot \sqrt{51 x^{3}}$$

Methane reacts with chlorine to produce methyl chloride and hydrogen chloride. Once formed, the methyl chloride may undergo further chlorination to form methylene chloride $\left(\mathrm{CH}_{2} \mathrm{Cl}_{2}\right)$, chloroform, and carbon tetrachloride. A methyl chloride production process consists of a reactor, a condenser, a distillation column, and an absorption column. A gas stream containing 80.0 mole% methane and the balance chlorine is fed to the reactor. In the reactor a single-pass chlorine conversion of essentially 100% is attained, the mole ratio of methyl chloride to methylene chloride in the product is 5:1, and negligible amounts of chloroform and carbon tetrachloride are formed. The product stream flows to the condenser. Two streams emerge from the condenser: the liquid condensate, which contains essentially all of the methyl chloride and methylene chloride in the reactor effluent, and a gas containing the methane and hydrogen chloride. The condensate goes to the distillation column in which the two component species are separated. The gas leaving the condenser flows to the absorption column where it contacts an aqueous solution. The solution absorbs essentially all of the HCl and none of the $\mathrm{CH}_{4}$ in the feed. The liquid leaving the absorber is pumped elsewhere in the plant for further processing, and the methane is recycled to join the fresh feed to the process (a mixture of methane and chlorine). The combined stream is the feed to the reactor. a) Choose a quantity of the reactor feed as a basis of calculation, draw and label a flowchart, and determine the degrees of freedom for the overall process and each single unit and stream mixing point. Then write in order the equations you would use to calculate the molar flow rate and molar composition of the fresh feed, the rate at which HCl must be removed in the absorber, the methyl chloride production rate, and the molar flow rate of the recycle stream. Do no calculations. b) Calculate the quantities specified in Part (a), either manually or with an equation-solving program. c) What molar flow rates and compositions of the fresh feed and the recycle stream are required to achieve a methyl chloride production rate of 1000 kg/h?