The Components of Matter

Name the type of organic compound from the following description of its functional group: 

(a) the polar group that has only single bonds and does not include O or N; 

(b) the group that is polar and has a triple bond; 

(c) the group that has single and double bonds and is acidic in water; 

(d) the group that has a double bond and must be at the end of a C chain.

Name the type of organic compound from the following description of its functional group: 

(a) N-containing group with single and double bonds; 

(b) the group that is not polar and has a double bond; 

(c) the polar group that has a double bond and cannot be at the end of a C chain; 

(d) the group that has only single bonds and is basic in water

What linkage joins the monomers in each strand of DNA? 

Draw the R group of (a) alanine; (b) histidine; (c) methionine.

Draw the R group of (a) glycine; (b) isoleucine; (c) tyrosine.

Write the sequence of the complementary DNA strand that pairs with each of the following DNA base sequences: 

(a) TTAGCC 

(b) AGACAT

Question: Write the sequence of the complementary DNA strand that pairs with each of the following DNA base sequences:

(a) GGTTAC 

(b) CCCGAA

Write the base sequence of the DNA template from which this RNA sequence was derived: UGUUACGGA. How many amino acids are coded for in this sequence?

Write the base sequence of the DNA template from which this RNA sequence was derived: GUAUCAAUGAACUUG. How many amino acids are coded for in this sequence?

Protein shapes are maintained by a variety of forces that arise from interactions between the amino-acid R groups. Name the amino acid that possesses each R group and the force that could arise in each of the following interactions:

When carbon dioxide dissolves in water, it undergoes a multistep equilibrium process, with $K_{overall} = 4.5\times {10}^{-7}$, which is simplified to the following:

$$\begin{gathered} {\text{CO}}_{\text{2}}{\text{(g) + H}}_{\text{2}}\text{O(l)}\rightleftharpoons {\text{H}}_{\text{2}}{\text{CO}}_{\text{3}}\text{(aq)} \\ {\text{H}}_{\text{2}}{\text{CO}}_{\text{3}}{\text{(aq) + H}}_{\text{2}}\text{O(l)}\rightleftharpoons {\text{HCO}}_{\text{3}}^{\text{ - }}{\text{(aq) + H}}_{\text{3}}{\text{O}}^{\text{ + }}\text{(aq)} \end{gathered}$$

(a) Classify each step as a Lewis or a Brønsted -Lowry reaction. 

(b) What is the pH of non-polluted rainwater in equilibrium with clean air (${\text{P}}_{{\text{CO}}_{\text{2}}}$in clean air $=3.2\times {10}^{-4}$atm; Henry’s law constant for  ${\text{CO}}_{\text{2}}$at 25C is $0.33$mol/L atm)?

(c) What is data-custom-editor="chemistry" $\left[{\text{CO}}_{\text{3}}^{\text{2}}\right]$ in rainwater ($K_0 of HC{O_3}^{-}=4.7\times {10}^{-11}$)? 

(d) If the partial pressure of  data-custom-editor="chemistry" ${\mathrm{CO}}_2$ in clean air doubles in the next few decades, what will the pH of rainwater become?

In humans, blood pH is maintained within a narrow range: acidosis occurs if the blood pH is below, and alkalosis occurs if the pH is above. Given that the pKw of blood is at  (body temperature), what is the normal range of [] and of in blood?

Pantothenic acid is shown below. This biologically active molecule is an optical isomer that behaves like a monoprotic Bronsted-Lowry acid in water.

(a) Use the molecular formula to write the equation for the reaction of pantothenic acid with water and the Ka expression. 

(b) Which C atom is the chiral center?

Classify the following as Arrhenius, Bronsted-Lowry, or Lewis acid-base reactions. A reaction may fit all, two, one, or none of the categories:

 $$\begin{gathered} {\text{a)Cu}}^{\text{2}}{\text{ + 4Cl}}^{\text{ - }}\text{ = } {\text{CuCl}}_{\text{4}}^{\text{2 - }} \\ {\text{(b)Al(OH)}}_{\text{3}}{\text{ + 3HNO}}_{\text{3}}\text{ = } {\text{Al}}^{\text{3 + }}{\text{ + 3H}}_{\text{2}}{\text{O + 3NO}}_{\text{3}}^{\text{ - }} \\ {\text{(c)N}}_{\text{2}}{\text{ + 3H}}_{\text{2}}\text{ = } {\text{2NH}}_{\text{3}} \\ {\text{(d)CN}}^{\text{ - }}{\text{ + H}}_{\text{2}}\text{O} \text{ = } {\text{HCN + OH}}^{\text{ - }} \end{gathered}$$

A $\mathbf{\text{50.0-mL}}$ volume of  ${\mathbf{\text{0.50 M Fe(NO}}}_{\mathbf{\text{3}}}{\mathbf{\text{)}}}_{\mathbf{\text{3}}}$is mixed with$\mathbf{\text{125 mL}}$ of ${\mathbf{\text{0.25 M Cd(NO}}}_{\mathbf{\text{3}}}{\mathbf{\text{)}}}_{\mathbf{\text{2}}}$. 

(a) If aqueous$\mathbf{\text{NaOH}}$ is added, which ion precipitates first? (See Appendix C.) 

(b) Describe how the metal ions can be separated using . 

(c) Calculate the${\mathbf{\text{[OH}}}^{\mathbf{\text{-}}}\mathbf{\text{]}}$ that will accomplish the separation.

Question: Question: Write equations to show whether the solubility of either of the following is affected by : 

(a) PbI₂; 

(b) Hg₂(CN₂).

The scene below depicts a saturated solution of ${\mathbf{\text{MCl}}}_{\mathbf{\text{2}}}\mathbf{\text{(s)}}$ in the presence of dilute aqueous $\mathbf{\text{NaCl}}$ ;each sphere represents: $\mathbf{1}\mathbf{.}\mathbf{0}\mathbf{\times }{\mathbf{10}}^{\mathbf{-}\mathbf{6}}\mathbf{mol}$ of ion, and the volume is  $\mathbf{\text{250.0 ml}}$ (solid MCl₂ is shown as green chunks; Na⁺ ions and water molecules are not shown).

1. Calculate the K_sp  of  ${\mathbf{MCl}}_{\mathbf{2}}$.
2.  If $\mathbf{M}{\mathbf{\left(}{\mathbf{NO}}_{\mathbf{3}}\mathbf{\right)}}_{\mathbf{2}}$  is added, there is increase, decrease or no change in Cl^-  particle ? In the K_sp ? In the mass of ${\mathbf{MCl}}_{\mathbf{2}}$ ?

The ${\mathbf{\text{MnO}}}_{\mathbf{\text{2}}}$ used in alkaline batteries can be produced by an electrochemical process of which one half-reaction is 

${\mathbf{\text{Mn}}}^{\mathbf{\text{2 + }}}{\mathbf{\text{(aq) + 2H}}}_{\mathbf{\text{2}}}\mathbf{\text{O(l)}}\mathbf{\to }{\mathbf{\text{MnO}}}_{\mathbf{\text{2}}}{\mathbf{\text{(s) + 4H}}}^{\mathbf{\text{ + }}}{\mathbf{\text{(aq) + 2e}}}^{\mathbf{\text{ - }}}$

If a current of is $\mathbf{\text{25.0 A}}$ used, how many hours are needed to produce $\mathbf{\text{1.00 kg}}$ of ${\mathbf{\text{MnO}}}_{\mathbf{\text{2}}}$? At which electrode is the ${\mathbf{\text{MnO}}}_{\mathbf{\text{2}}}$formed?

Car manufacturers are developing engines that use ${\mathbf{\text{H}}}_{\mathbf{\text{2}}}$ as fuel. In Iceland, Sweden, and other parts of Scandinavia, where hydroelectric plants produce inexpensive electric power, the ${\mathbf{\text{H}}}_{\mathbf{\text{2}}}$ can be made industrially by the electrolysis of water.

(a) How many coulombs are needed to produce $\mathbf{3}\mathbf{.}\mathbf{5}\mathbf{·}{\mathbf{10}}^{\mathbf{6}}\mathbf{ }\mathit{L}$ of ${\mathbf{\text{H}}}_{\mathbf{\text{2}}}$ gas at  $\mathbf{\text{12.0 atm}}$ and  ${\mathbf{\text{25}}}^{\mathbf{\text{o}}}\mathbf{\text{C}}$? (Assume the ideal gas law applies.) 

(b) If the coulombs are supplied at  $\mathbf{\text{1.44 V}}$, how many joules are produced? 

(c) If the combustion of oil yields $\mathbf{4}\mathbf{.}\mathbf{0}\mathbf{\times }{\mathbf{10}}^{\mathbf{4}}\mathbf{ }\mathbf{KJ}\mathbf{/}\mathbf{Kg}$ , what mass of oil must be burned to yield the number of joules in part (b)?

Tin is used to coat “tin” cans used for food storage. If the tin is scratched and the iron of the can exposed, will the iron corrode more or less rapidly than if the tin were not present? Inside the can, the tin itself is coated with a clear varnish. Explain.

An inexpensive and accurate method of measuring the quantity of electricity passing through a circuit is to pass it through a solution of a metal ion and weigh the metal deposited. A silver electrode immersed in an ${\mathbf{\text{Ag}}}^{\mathbf{\text{ + }}}$solution weighs $\mathbf{1}\mathbf{.}\mathbf{7854}\mathbf{ }\mathbf{g}$ before the current passes and weighs $\mathbf{1}\mathbf{.}\mathbf{8016}\mathbf{ }\mathbf{g}$ after the current has passed. How many coulombs have passed?

Use the emf series (Appendix D) to arrange the species.

(a) In order of decreasing strength as reducing agents

(b) In order of increasing strength as reducing agents:

Balance each skeleton reaction calculate , and state whether the reaction is spontaneous:

(a)${\mathbf{\text{Co(s) + H}}}^{\mathbf{\text{ + }}}{\mathbf{\text{(aq)Co}}}^{\mathbf{\text{2 + }}}{\mathbf{\text{(aq) + H}}}_{\mathbf{\text{2}}}\mathbf{\text{(g)}}$  (b) ${\mathbf{\text{Mn}}}^{\mathbf{\text{2 + }}}{\mathbf{\text{(aq) + Br}}}_{\mathbf{\text{2}}}{\mathbf{\text{(l)nMnO}}}_{\mathbf{\text{4}}}^{\mathbf{\text{ - }}}{\mathbf{\text{(aq) + Br}}}^{\mathbf{\text{ - }}}\mathbf{\text{(aq)}}$

(c) $\mathbf{\text{H}}{{\mathbf{\text{g}}}_{\mathbf{\text{2}}}}^{\mathbf{\text{2 + }}}{\mathbf{\text{(aq)Hg}}}^{\mathbf{\text{2 + }}}\mathbf{\text{(aq) + Hg(l)}}$

Both a D-sized and an AAA-size alkaline battery have an output of V. What property of the cell potential allows this to occur? What is different about these two batteries?

Two voltaic cells are to be joined so that one will run the other as an electrolytic cell. In the first cell, one half-cell has $\mathbf{Au}$ foil in data-custom-editor="chemistry" $\mathbf{1}\mathbf{.}\mathbf{00}\mathbf{MAu}{\left({\mathrm{NO}}_3\right)}_{\mathbf{3}}$ , and the other half-cell has a Cr bar in $\mathbf{1}\mathbf{.}\mathbf{00}\mathbf{MCr}{\left({\mathrm{NO}}_3\right)}_{\mathbf{3}}$ . In the second cell, one half-cell has a Co bar in $\mathbf{1}\mathbf{.}\mathbf{00}\mathbf{MCo}{\left({\mathrm{NO}}_3\right)}_{\mathbf{2}}$ , and the other half-cell has a  $\mathbf{Zn}$ bar in   - $\mathbf{1}\mathbf{.}\mathbf{00}\mathbf{MZn}{\left({\mathrm{NO}}_3\right)}_{\mathbf{2}}$-

(a) Calculate data-custom-editor="chemistry" ${\mathbf{E}}_{\mathbf{cell}}^{\mathbf{o}}$  for each cell. 

(b) Calculate the total potential if the two cells are connected as voltaic cells in series. 

(c) When the electrode wires are switched in one of the cells, which cell will run as the voltaic cell and which as the electrolytic cell? 

(d) Which metal ion is being reduced in each cell? 

(e) If  $\mathbf{2}\mathbf{.}\mathbf{00}\mathbf{ }\mathbf{g}$ of metal plates out in the voltaic cell, how much metal ion plates out in the electrolytic cell?

Curium-243 undergoes   decay to plutonium-239:

(a) Find the change in mass, $\Delta m$  (in kg). (Masses: ${}^{243}Cm=$${\text{243.0614amu;}}^{\text{239}}{\text{Pu = 239.0522amu;}}^{\text{4}}\text{He = 4.0026amu}$  ; $1amu=1.661\times {10}^{-24} g$.) 

(b) Find the energy released in joules.

(c) Find the energy released in  $\text{kJ/mol}$ of reaction, and comment on the difference between this value and a typical heat of reaction for a chemical change, which is a few hundred $\text{kJ/mol}$ .

A H nucleus decays with an energy of MeV. Convert this energy into (a) electron volts; (b) joules.

Arsenic- decays with an energy of ${\mathbf{\text{1.57×10}}}^{\mathbf{\text{ - 15}}}\mathbf{\text{ kJ}}$ per nucleus. Convert this energy into 

(a) eV;

(b) MeV.

Name the unidentified species, and write each transmutation process in shorthand notation:

 (a) gamma irradiation of a nuclide yields a proton, a neutron, and 29Si; 

(b) bombardment of 252Cf with 10B yields five neutrons and a nuclide; 

(c) bombardment of 238U with a particle yields three neutrons and 239Pu.

Lead-$\mathbf{206}$ is the end product of 238U decay. One ${}^{\mathbf{\text{206}}}\mathbf{\text{Pb}}$ atom has a mass of $\mathbf{\text{205.974440}}$amu. Calculate the binding energy 

(a) per nucleon in MeV;

(b) per atom in MeV;

(c) per mole in kJ.

Cobalt-$\mathbf{\text{59}}$ is the only stable isotope of this transition metal. One ${}^{\mathbf{\text{59}}}\mathbf{\text{Co}}$ atom has a mass of $\mathbf{\text{58.933198}}$amu. Calculate the binding energy

 (a) per nucleon in MeV;

(b) per atom in MeV;

(c) per mole in kJ.

In what main way is fission different from radioactive decay? Are all fission events in a chain reaction identical? Explain.

Plutonium "triggers" for nuclear weapons were manufactured at the Rocky Flats plant in Colorado. An $\mathbf{\text{85 - kg}}$ worker inhaled a dust particle containing $\mathbf{1}\mathbf{ }\mathbf{\text{μg}}$ of ${}_{\mathbf{\text{94}}}{}^{\mathbf{\text{239}}}\mathbf{\text{Pu}}$, which resided in his body for $\mathbf{\text{16h}}({\text{t}}_{\text{1/2}}$ of ${}^{\mathbf{\text{239}}}\mathbf{\text{Pu = 2.41×10}}^{\mathbf{\text{4}}}\mathbf{\text{ yr}}$, each disintegration released $\mathbf{\text{5.15 MeV}}$). 

(a) How many rads did he receive? 

(b) How many grays?

Cerium (Ce) and ytterbium (Yb) exhibit some oxidation states in addition to +3. 

(a) Write the electron configurations of Ce²⁺ , Ce³⁺ and Ce⁴⁺ . 

(b) Write the electron configurations of Yb²⁺ , Yb²⁺ and Yb⁴⁺ . 

(c) In addition to the 3+ ions, the ions Ce⁴⁺ and Yb²⁺ are stable. Suggest a reason for this stability.

Do both members of the following pairs have the same number of protons? Neutrons? Electrons?

$\left(a\right)\mathbf{ }{}_{\mathbf{1}}{}^{\mathbf{3}}\mathit{H}\mathbf{ }\mathit{a}\mathit{n}\mathit{d}\mathbf{ }{}_{\mathbf{2}}{}^{\mathbf{3}}\mathit{H}\mathit{e}\mathbf{ }\left(b\right)\mathbf{ }{}_{\mathbf{6}}{}^{\mathbf{14}}\mathit{C}\mathbf{ }\mathit{a}\mathit{n}\mathit{d}\mathbf{ }{}_{\mathbf{7}}{}^{\mathbf{15}}\mathit{N}\mathbf{ }\left(c\right)\mathbf{ }{}_{\mathbf{9}}{}^{\mathbf{19}}\mathit{F}\mathbf{ }\mathit{a}\mathit{n}\mathit{d}\mathbf{ }{}_{\mathbf{9}}{}^{\mathbf{18}}\mathit{F}\mathbf{ }$

Which pair(s) consist(s) of atoms with the same Z value? N value? A value?

Write the ${}_{\mathbf{Z}}{}^{\mathbf{A}}\mathit{X}$ notation for each atomic depiction

(a)(b) (c)

Write the ${}_{\mathbf{Z}}{}^{\mathbf{A}}\mathit{X}$ notation for each atomic depiction:

(a)(b)(c)

Balance each skeleton reaction, calculate and state whether the reaction is spontaneous:

(a) ${\mathbf{\text{Ag(s) + Cu}}}^{\mathbf{\text{2 + }}}{\mathbf{\text{(aq)Ag}}}^{\mathbf{\text{ + }}}\mathbf{\text{(aq) + Cu(s)}}$

(b) ${\mathbf{\text{Cd(s) + Cr}}}_{\mathbf{\text{2}}}{\mathbf{\text{O}}}_{\mathbf{\text{7}}}^{\mathbf{\text{2 - }}}{\mathbf{\text{(aq)Cd}}}^{\mathbf{\text{2 + }}}{\mathbf{\text{(aq) + Cr}}}^{\mathbf{\text{3 + }}}\mathbf{\text{(aq)}}$  

c)    ${\mathbf{\text{Ni}}}^{\mathbf{\text{2 + }}}{\mathbf{\text{(aq) + Pb(s)Ni(s) + Pb}}}^{\mathbf{\text{2 + }}}\mathbf{\text{(aq)}}$

(a) T2248i (b) S3479e (c) B511Draw atomic depictions similar to those in Problem 2.43 for $\mathbf{\left(}\mathit{a}\mathbf{\right)}\mathbf{ }{}_{\mathbf{22}}{}^{\mathbf{48}}\mathit{T}\mathit{i}\mathbf{ }\mathbf{\left(}\mathit{b}\mathbf{\right)}\mathbf{ }{}_{\mathbf{34}}{}^{\mathbf{79}}\mathit{S}\mathit{e}\mathbf{ }\mathbf{\left(}\mathit{c}\mathbf{\right)}\mathbf{ }{}_{\mathbf{5}}{}^{\mathbf{11}}\mathit{B}$

Balance each skeleton reaction, calculate ${E^{\circ }}_{cell}$ and state whether the reaction is spontaneous:

(a) ${\text{Cu}}^{\text{ + }}{\text{(aq) + PbO}}_{\text{2}}\text{(s) + S}{{\text{O}}_{\text{4}}}^{\text{2 - }}{\text{(aq)PbSO}}_{\text{4}}{\text{(s) + Cu}}^{\text{2 + }}\text{(aq)[acidic]}$

(b) ${\text{H}}_{\text{2}}{\text{O}}_{\text{2}}{\text{(aq) + Ni}}^{\text{2 + }}{\text{(aq)O}}_{\text{2}}\text{(g) + Ni(s)[acidic]}$

(c) ${\text{MnO}}_{\text{2}}{\text{(s) + Ag}}^{\text{ + }}\text{(aq)Mn}{{\text{O}}_{\text{4}}}^{\text{ - }}\text{(aq) + Ag(s)[basic]}$

Draw atomic depictions similar to those in Problem 2.43 for  $\mathbf{\left(}\mathit{a}\mathbf{\right)}\mathbf{ }{}_{\mathbf{82}}{}^{\mathbf{207}}\mathit{P}\mathit{b}\mathbf{ }\mathbf{\left(}\mathit{b}\mathbf{\right)}\mathbf{ }{}_{\mathbf{5}}{}^{\mathbf{9}}\mathit{B}\mathit{e}\mathbf{ }\mathbf{\left(}\mathit{c}\mathbf{\right)}\mathbf{ }{}_{\mathbf{33}}{}^{\mathbf{75}}\mathit{A}\mathit{s}$

Use the following half-reactions to write three spontaneous reactions, calculate ${E^{\circ }}_{cell}$ for each reaction, and rank the strengths of the oxidizing and reducing agents:

(1) ${\mathbf{\text{Al}}}^{\mathbf{\text{3 + }}}{\mathbf{\text{(aq) + 3e}}}^{\mathbf{\text{ - }}}\mathbf{\text{nAl(s)}}$${\mathit{E}}^{\mathbf{\circ }}\mathbf{=}\mathbf{-}\mathbf{1}\mathbf{.}\mathbf{66}\mathit{V}$  (2) ${\mathbf{\text{N}}}_{\mathbf{\text{2}}}{\mathbf{\text{O}}}_{\mathbf{\text{4}}}{\mathbf{\text{(g) + 2e}}}^{\mathbf{\text{ - }}}{\mathbf{\text{n2NO}}}_{\mathbf{\text{2}}}^{\mathbf{\text{ - }}}\mathbf{\text{(aq)}}$${\mathit{E}}^{\mathbf{\circ }}\mathbf{=}\mathbf{0}\mathbf{.}\mathbf{867}\mathit{V}$

(3)${\mathbf{\text{SO}}}_{\mathbf{\text{4}}}^{\mathbf{\text{2 - }}}{\mathbf{\text{(aq) + H}}}_{\mathbf{\text{2}}}{\mathbf{\text{O(l) + 2e}}}^{\mathbf{\text{ - }}}{\mathbf{\text{nSO}}}_{\mathbf{\text{3}}}^{\mathbf{\text{2 - }}}{\mathbf{\text{(aq) + 2OH}}}^{\mathbf{\text{ - }}}\mathbf{\text{(aq)}}$ ${\mathit{E}}^{\mathbf{\circ }}\mathbf{=}\mathbf{0}\mathbf{.}\mathbf{93}\mathit{V}$acidic solutions react spontaneously to the process of reduction and oxidation also used into half reaction and the electrons and atoms on both sides.                   

Gallium has two naturally occurring isotopes, ⁶⁹Ga (isotopic mass 68.9256 amu, abundance 60.11%) and ⁷¹Ga (isotopic mass 70.9247 amu, abundance 39.89%). Calculate the atomic mass of gallium.

Use the following half-reactions to write three spontaneous reactions, calculate ${E^{\circ }}_{cell}$  for each reaction, and rank the strengths of the oxidizing and reducing agents:

(1) ${\mathbf{\text{Au}}}^{\mathbf{\text{ + }}}{\mathbf{\text{(aq) + e}}}^{\mathbf{\text{ - }}}\mathbf{\text{nAu(s)}}\mathbf{ }{\mathbf{\text{E}}}^{\mathbf{\text{0}}}\mathbf{\text{ = 1.69V}}$

(2)  ${\mathbf{\text{N}}}_{\mathbf{\text{2}}}{\mathbf{\text{O(g) + 2H}}}^{\mathbf{\text{ + }}}{\mathbf{\text{(aq) + 2e}}}^{\mathbf{\text{ - }}}{\mathbf{\text{nN}}}_{\mathbf{\text{2}}}{\mathbf{\text{(g) + H}}}_{\mathbf{\text{2}}}\mathbf{\text{O(l)}}$

(3)$\mathit{C}{\mathit{r}}^{\mathbf{3}}\mathbf{+}\mathbf{\left(}\mathit{a}\mathit{q}\mathbf{\right)}\mathbf{+}\mathbf{3}{\mathit{e}}^{\mathbf{-}}\mathit{n}{\mathit{E}}^{\mathbf{\circ }}\mathbf{=}\mathbf{1}\mathbf{.}\mathbf{77}\mathit{V}{\mathit{E}}^{\mathbf{\circ }}\mathbf{=}\mathbf{-}\mathbf{0}\mathbf{.}\mathbf{74}\mathit{V}$

Magnesium has three naturally occurring isotopes, ²⁴Mg(isotopic mass 23.9850 amu, abundance 78.99%), ²⁵Mg(isotopic mass 24.9858 amu, abundance 10.00%), and ²⁶Mg (isotopic mass 25.9826 amu, abundance 11.01%). Calculate the atomic mass of magnesium.

Use the following half-reactions to write three spontaneous reactions  , calculate${E^{\circ }}_{cell}$ for each reaction, and rank the strengths of the oxidizing and reducing agents:

(1)  $\mathbf{2}\mathit{H}\mathit{C}\mathit{I}\mathit{O}\mathbf{\left(}\mathit{a}\mathit{q}\mathbf{\right)}\mathbf{+}\mathbf{2}{\mathit{H}}^{\mathbf{+}}\mathbf{\left(}\mathit{a}\mathit{q}\mathbf{\right)}\mathbf{+}\mathbf{2}{\mathit{e}}^{\mathbf{-}}\mathit{C}{\mathit{I}}_{\mathbf{2}}\mathbf{\left(}\mathit{g}\mathbf{\right)}\mathbf{+}\mathbf{2}{\mathit{H}}_{\mathbf{2}}\mathbf{\left(}\mathit{I}\mathbf{\right)}{\mathit{E}}^{\mathbf{\circ }}\mathbf{=}\mathbf{1}\mathbf{.}\mathbf{63}\mathit{V}$ 

(2)   $\mathit{P}{\mathit{t}}^{\mathbf{2}\mathbf{+}}\mathbf{\left(}\mathit{a}\mathit{q}\mathbf{\right)}\mathbf{+}\mathbf{2}{\mathit{e}}^{\mathbf{-}}\mathit{P}\mathit{t}\mathbf{\left(}\mathit{s}\mathbf{\right)}\mathbf{ }\mathbf{ }\mathbf{ }\mathbf{ }{\mathit{E}}^{\mathbf{\circ }}\mathbf{=}\mathbf{1}\mathbf{.}\mathbf{20}\mathit{V}$

(3)    $\mathit{P}\mathit{b}\mathit{S}{\mathit{O}}_{\mathbf{4}}\mathbf{\left(}\mathit{S}\mathbf{\right)}\mathbf{+}\mathbf{2}{\mathit{e}}^{\mathbf{-}}\mathit{P}\mathit{b}\mathbf{\left(}\mathit{s}\mathbf{\right)}\mathbf{+}\mathit{S}{{\mathit{O}}_{\mathbf{4}}}^{\mathbf{2}\mathbf{-}}\mathbf{\left(}\mathit{a}\mathit{q}\mathbf{\right)}\mathbf{ }\mathbf{ }\mathbf{ }{\mathit{E}}^{\mathbf{\circ }}\mathbf{=}\mathbf{-}\mathbf{0}\mathbf{.}\mathbf{31}\mathit{V}$        

Chlorine has two naturally occurring isotopes,${}^{\mathbf{35}}\mathit{C}\mathit{l}$(isotopic mass 34.9689 amu) and ³⁷Cl (isotopic mass 36.9659 amu). If chlorine has an atomic mass of 35.4527 amu, what is the percent abundance of each isotope?

C65uCopper has two C65unaturally occurring isotopes,${}^{\mathbf{63}}\mathit{C}\mathit{u}$ (isotopic mass 62.9396 amu) and ${}^{\mathbf{65}}\mathit{C}$(isotopic mass 64.9278 amu). If copper has an atomic mass of 63.546 amu, what is the percent abundance of each isotope.

Give systematic names for the following formulas:

1. $\mathit{K}\mathbf{\left[}\mathbf{A}\mathbf{g}{\mathbf{\left(}\mathbf{C}\mathbf{N}\mathbf{\right)}}_{\mathbf{2}}\mathbf{\right]}$
2. $\mathit{N}{\mathit{a}}_{\mathbf{2}}\mathbf{\left[}\mathbf{C}\mathbf{d}\mathbf{C}{\mathbf{l}}_{\mathbf{4}}\mathbf{\right]}$
   
3. $\mathbf{\left[}\mathbf{C}\mathbf{o}{\mathbf{\left(}\mathbf{N}{\mathbf{H}}_{\mathbf{3}}\mathbf{\right)}}_{\mathbf{4}}\mathbf{\left(}{\mathbf{H}}_{\mathbf{2}}\mathbf{O}\mathbf{\right)}\mathbf{B}\mathbf{r}\mathbf{\right]}\mathit{B}{\mathit{r}}_{\mathbf{2}}$
   

A voltaic cell with Mn/Mn and Cd/Cd2 half-cells has the following initial concentrations: =$\left[M{n}^{2+}\right]\mathbf{=}\mathbf{0}\mathbf{.}\mathbf{090}\mathit{M}$; [Cd2] =$0.060$ M.

 (a) What is the initial $E_{cell}$? 

(b) What is $E_{cell}$ when [Cd2] reaches $0.050$ M? 

(c) What is $\left[M{n}^{2+}\right]$ when $E_{cell}$ reaches $0.050$V? 

(d) What are the equilibrium concentrations of the ions?