Fungal Laccase a Blue Protein Found in Wood Rotting Fungi
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Give the balanced equation for each of the following. a. The combustion of ethanol $\left(\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}\right)$ forms carbon dioxide and water vapor. A combustion reaction refers to a reaction of a substance with oxygen gas. b. Aqueous solutions of lead(II) nitrate and sodium phosphate are mixed, resulting in the precipitate formation of lead(II) phosphate with aqueous sodium nitrate as the other product. c. Solid zinc reacts with aqueous $\mathrm{HCl}$ to form aqueous zinc chloride and hydrogen gas. d. Aqueous strontium hydroxide reacts with aqueous hydrobromic acid to produce water and aqueous strontium bromide.
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18. Consider the following diagram when answering the questions on the next page.>a. Compare balls A and B in terms of potential energy in both the initial and final setups. b. Ball A has stopped moving in the final setup, but energy must be conserved. What happened to the potential energy of ball A?
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Balance the following equations: a. $\mathrm{Ca}(\mathrm{OH})_{2}(a q)+\mathrm{H}_{3} \mathrm{PO}_{4}(a q) \rightarrow \mathrm{H}_{2} \mathrm{O}(l)+\mathrm{Ca}_{3}\left(\mathrm{PO}_{4}\right)_{2}(s)$ b. $\mathrm{Al}(\mathrm{OH})_{3}(s)+\mathrm{HCl}(a q) \rightarrow \mathrm{AlCl}_{3}(a q)+\mathrm{H}_{2} \mathrm{O}(l)$ c. $\mathrm{AgNO}_{3}(a q)+\mathrm{H}_{2} \mathrm{SO}_{4}(a q) \rightarrow \mathrm{Ag}_{2} \mathrm{SO}_{4}(s)+\mathrm{HNO}_{3}(a q)$
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Give the balanced equation for each of the following chemical reactions: a. Glucose $\left(\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}\right)$ reacts with oxygen gas to produce gaseous carbon dioxide and water vapor. b. Solid iron(III) sulfide reacts with gaseous hydrogen chloride to form solid iron(III) chloride and hydrogen sulfide gas. c. Carbon di sulfide liquid reacts with ammonia gas to produce hydrogen sulfide gas and solid ammonium thiocyanate $\left(\mathrm{NH}_{4} \mathrm{SCN}\right) .$
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Aluminum ions react with the hydroxide ion to form the precipitate $\mathrm{Al}(\mathrm{OH})_{3}(s)$ , but can also react to form the soluble complex ion $\mathrm{Al}(\mathrm{OH})_{4}{ }^{-} .$ In terms of solubility, $\mathrm{Al}(\mathrm{OH})_{3}(s)$ will be more soluble in very acidic solutions as well as more soluble in very basic solutions. a. Write equations for the reactions that occur to increase the solubility of $\mathrm{Al}(\mathrm{OH})_{3}(s)$ in very acidic solutions and in very basic solutions.>b. Let's study the $\mathrm{pH}$ dependence of the solubility of $$\mathrm{Al}(\mathrm{OH})_{3}$(s)$ in more detail. Show that the solubility of $\mathrm{Al}(\mathrm{OH})_{3}$ , as a function of $\left[\mathrm{H}^{+}\right]$ , obeys the equation \[ $S=$\left[\mathrm{H}^{+}\right]$^{3} K_{\mathrm{sp}} / K_{\mathrm{w}}{ }^{3}+K K_{\mathrm{w}} /$\left[\mathrm{H}^{+}\right]$$ \] where S= solubility $=\left[\mathrm{Al}^{3+}\right]+\left[\mathrm{Al}(\mathrm{OH})_{4}^{-}\right]$ and K is the equilibrium constant for \[ $$\mathrm{Al}(\mathrm{OH})_{3}$(s)$+\mathrm{OH}^{-}(a q) \rightleftharpoons \mathrm{Al}(\mathrm{OH})_{4}^{-}(a q) \] c. The value of K is 40.0 and $K_{\text {sp }}$ for $\mathrm{Al}(\mathrm{OH})_{3}$ is $2 \times 10^{-32}$ . Plot the solubility of $\mathrm{Al}(\mathrm{OH})_{3}$ in the pH range 4-12.
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A balloon filled with 39.1 moles of helium has a volume of $876 \mathrm{~L}$ at $0.0^{\circ} \mathrm{C}$ and 1.00 atm pressure. At constant pressure, the temperature of the balloon is increased to $38.0^{\circ} \mathrm{C}$ , causing the balloon to expand to a volume of $998 \mathrm{~L}$ . Calculate q, w , and $\Delta E$ for the helium in the balloon. (The molar heat capacity for helium gas is $20.8 \mathrm{~J}{ }^{\circ} \mathrm{C}^{-1} \mathrm{~mol}^{-1}$ .)
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The enthalpy change for a reaction is a state function and it is an extensive property. Explain.
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Dimethylnitrosamine, $\left(\mathrm{CH}_{3}\right)_{2} \mathrm{~N}_{2} \mathrm{O}$ , is a carcinogenic (cancercausing) substance that may be formed in foods, beverages, or gastric juices from the reaction of nitrite ion (used as a food preservative) with other substances. a. What is the molar mass of dimethylnitrosamine? b. How many moles of $\left(\mathrm{CH}_{3}\right)_{2} \mathrm{~N}_{2} \mathrm{O}$ molecules are present in $250 \mathrm{mg}$ dimethylnitrosamine? c. What is the mass of $0.050$ mole of dimethylnitrosamine? d. How many atoms of hydrogen are in 1.0 mole of dimethylnitrosamine? e. What is the mass of $1.0 \times 10^{6}$ molecules of dimethylnitrosamine? f. What is the mass in grams of one molecule of dimethylnitrosamine?
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One mole of $\mathrm{H}_{2} \mathrm{O}(g)$ at 1.00 atm and $100 .{ }^{\circ} \mathrm{C}$ occupies a volume of $30.6 \mathrm{~L}$ . When 1 mole of $\mathrm{H}_{2} \mathrm{O}(g)$ is condensed to 1 mole of $\mathrm{H}_{2} \mathrm{O}(l)$ at 1.00 atm and $100 .{ }^{\circ} \mathrm{C}$, 40.66 \mathrm{~kJ} of heat is released. If the density of $\mathrm{H}_{2} \mathrm{O}(l)$ at this temperature and pressure is $0.996 \mathrm{~g} / \mathrm{cm}^{3}$ , calculate $\Delta E$ for the condensation of 1 mole of water at $1.00 \mathrm{~atm}$ and $100 .{ }^{\circ} \mathrm{C}$
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Arrange the following substances in order of increasing mass percent of carbon. a. caffeine, $\mathrm{C}_{8} \mathrm{H}_{10} \mathrm{~N}_{4} \mathrm{O}_{2}$ b. sucrose, $\mathrm{C}_{12} \mathrm{H}_{22} \mathrm{O}_{11}$ c. ethanol, $\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}$
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A common demonstration in chemistry courses involves adding a tiny speck of manganese(IV) oxide to a concentrated hydrogen peroxide $\left(\mathrm{H}_{2} \mathrm{O}_{2}\right)$ solution. Hydrogen peroxide decomposes quite spectacularly under these conditions to produce oxygen gas and steam (water vapor). Manganese(IV) oxide is a catalyst for the decomposition of hydrogen peroxide and is not consumed in the reaction. Write the balanced equation for the decomposition reaction of hydrogen peroxide.
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Consider a mixture of air and gasoline vapor in a cylinder with a piston. The original volume is $40 . \mathrm{cm}^{3}$ . If the combustion of this mixture releases $950 . \mathrm{J}$ of energy, to what volume will the gases expand against a constant pressure of 650 . torr if all the energy of combustion is converted into work to push back the piston?
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The percent by mass of nitrogen for a compound is found to be 46.7\%. Which of the following could be this species?
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Iron oxide ores, commonly a mixture of $\mathrm{FeO}$ and $\mathrm{Fe}_{2} \mathrm{O}_{3}$ , are given the general formula $\mathrm{Fe}_{3} \mathrm{O}_{4}$ . They yield elemental iron when heated to a very high temperature with either carbon monoxide or elemental hydrogen. Balance the following equations for these processes: \[ \begin{aligned} $\mathrm{Fe}_{3} \mathrm{O}_{4}$(s)+\mathrm{H}_{2}(g) & \longrightarrow \mathrm{Fe}(s)+\mathrm{H}_{2} \mathrm{O}(g) \\ $\mathrm{Fe}_{3} \mathrm{O}_{4}$(s)+\mathrm{CO}(g) & \longrightarrow \mathrm{Fe}(s)+\mathrm{CO}_{2}(g) \end{aligned} \]
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Assuming gasoline is pure $\mathrm{C}_{8} \mathrm{H}_{18}(l)$ , predict the signs of q and w for the process of combusting gasoline into $\mathrm{CO}_{2}(g)$ and $\mathrm{H}_{2} \mathrm{O}(g)$ .
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A system undergoes a process consisting of the following two steps: Step 1: The system absorbs $72 \mathrm{~J}$ of heat while $35 \mathrm{~J}$ of work is done on it. Step 2: The system absorbs $35 \mathrm{~J}$ of heat while performing $72 \mathrm{~J}$ of work. Calculate $\Delta E$ for the overall process.
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Calculate the internal energy change for each of the following. a. One hundred (100.) joules of work are required to compress a gas. At the same time, the gas releases $23 \mathrm{~J}$ of heat. b. A piston is compressed from a volume of $8.30 \mathrm{~L}$ to $2.80 \mathrm{~L}$ against a constant pressure of $1.90 \mathrm{~atm}$ . In the process, there is a heat gain by the system of 350. J. c. A piston expands against $1.00 \mathrm{~atm}$ of pressure from $11.2 \mathrm{~L}$ to $29.1 \mathrm{~L}$ . In the process, $1037 \mathrm{~J}$ of heat is absorbed.
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Chloral hydrate \left($\mathrm{C}_{2} \mathrm{H}_{3} \mathrm{Cl}_{3} \mathrm{O}_{2}$\right) is a drug formerly used as a sedative and hypnotic. It is the compound used to make "Mickey Finns" in detective stories. a. Calculate the molar mass of chloral hydrate. b. What amount (moles) of $\mathrm{C}_{2} \mathrm{H}_{3} \mathrm{Cl}_{3} \mathrm{O}_{2}$ molecules are in $500.0 \mathrm{~g}$ chloral hydrate? c. What is the mass in grams of $2.0 \times 10^{-2}$ mole of chloral hydrate? d. What number of chlorine atoms are in $5.0 \mathrm{~g}$ chloral hydrate?>e. What mass of chloral hydrate would contain $1.0 \mathrm{~g} \mathrm{Cl}$ ? f. What is the mass of exactly 500 molecules of chloral hydrate?
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