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chemistry and chemical reactivity

Questions and Answers of Chemistry And Chemical Reactivity

Use cell notation to depict an electrochemical cell based upon the following reaction that is product-favored at equilibrium. Cu(s) + Cl₂(g) → 2 Cl(aq) + Cu²+ (aq)
Use cell notation to depict an electrochemical cell based upon the following reaction that is product-favored at equilibrium. Fe³+ (aq) + Ag(s) + Cl(aq) → Fe²+ (aq) + AgCl(s)
What are the similarities and differences between dry cells, alkaline batteries, and Ni-cad batteries?
What reactions occur when a lead storage battery is recharged?
Calculate the value of E° for each of the following reactions. Decide whether each is product-favored at equilibrium in the direction written. (a) 2 1 (aq) + Zn²+ (aq) → 1₂(s) + Zn(s) (b) Zn²+
Calculate the value of E° for each of the following reactions. Decide whether each is product-favored at equilibrium in the direction written. [Reaction (d) is carried out in basic solution.] (a)
Balance each of the following unbalanced equations; then calculate the standard potential, E°, and decide whether each is product-favored at equilibrium as written. (All reactions are carried out in
Balance each of the following unbalanced equations; then calculate the standard potential, E°, and decide whether each is product-favored at equilibrium as written. (All reactions are carried out in
Consider the following half-reactions:(a) Based on E° values, which metal is the most easily oxidized?(b) Which metals on this list are capable of reducing Fe2+(aq) to Fe(s)?(c) Write a balanced
Consider the following half-reactions:(a) Choosing from among the reactants in these half-reactions, identify the strongest and weakest oxidizing agents.(b) Which of the oxidizing agents listed is
From the following list, identify those elements that are easier to oxidize than H2(g).(a) Cu(b) Zn(c) Fe(d) Ag(e) Cr
Which of the following elements is the best reducing agent under standard conditions?(a) Cu(b) Zn(c) Fe(d) Ag(e) Cr
Which of the following ions is most easily reduced?(a) Cu2+(aq)(b) Zn2+(aq)(c) Fe2+(aq)(d) Ag+(aq)(e) Al3+(aq)
From the following list, identify the ions that are more easily reduced than H+(aq).(a) Cu2+(aq)(b) Zn2+(aq)(c) Fe2+(aq)(d) Ag+(aq)(e) Al3+(aq)
(a) Which halogen is most easily reduced in acidic solution: F2, Cl2, Br2, or I2?(b) Identify the halogens that are better oxidizing agents in acidic solution than MnO2(s).
(a) Which ion is most easily oxidized to the elemental halogen in acidic solution: F−, Cl−, Br−, or I−?(b) Identify the halide ions that are more easily oxidized in acidic solution than
Calculate the potential delivered by a voltaic cell using the following reaction if all dissolved species are 2.5 × 10−2 M and the pressure of H2 is 1.0 bar. Zn(s) + 2 H₂O(l) + 2 OH (aq)
Calculate the potential developed by a voltaic cell using the following reaction if all dissolved species are 0.015 M. 2 Fe²+ (aq) + H₂O₂(aq) + 2 H+ (aq) → 2 Fe³+ (aq) + 2 H₂O(l)
One half-cell in a voltaic cell is constructed from a silver wire electrode in a 0.25 M solution of AgNO3. The other half-cell consists of a zinc electrode in a 0.010 M solution of Zn(NO3)2.
One half-cell in a voltaic cell is constructed from a copper wire electrode in a 4.8 × 10−3 M solution of Cu(NO3)2. The other half-cell consists of a zinc electrode in a 0.40 M solution of
One half-cell in a voltaic cell is constructed from a silver wire electrode in a AgNO3 solution of unknown concentration. The other half-cell consists of a zinc electrode in a 1.0 M solution of
Calculate ΔrG° and the equilibrium constant for the following reactions. (a) 2 Fe³+ (aq) + 21 (aq): (b) 1₂(aq) + 2 Br(aq) = 2 Fe²+ (aq) + ₂(aq) 21-(aq) + Br₂(l)
One half-cell in a voltaic cell is constructed from an iron electrode in an Fe(NO3)2 solution of unknown concentration. The other half-cell is a standard hydrogen electrode. A potential of 0.49 V is
Calculate ΔrG° and the equilibrium constant for the following reactions. (a) Zn²+ (aq) + Ni(s) Zn(s) + Ni²+ (aq) (b) Cu(s) + 2 Ag+ (aq) = Cu²+ (aq) + 2 Ag(s)
Use standard reduction potentials (Appendix M) for the half-reactions AgBr(s) + e− → Ag(s) + Br−(aq) and Ag+(aq) + e− → Ag(s) to calculate the value of Ksp for AgBr.Data given in Appendix M
Use the standard reduction potentials (Appendix M) for the half-reactions [Zn(OH)4]2−(aq) + 2 e− → Zn (s) + 4 OH−(aq) and Zn2+(aq) + 2e− → Zn(s) to calculate the value of Kformation for
Diagram the apparatus used to electrolyze molten NaCl. Identify the anode and the cathode. Trace the movement of electrons through the external circuit and the movement of ions in the electrolysis
Diagram the apparatus used to electrolyze aqueous CuCl2. Identify the reaction products, the anode, and the cathode. Trace the movement of electrons through the external circuit and the movement of
Which product, O2 or F2, is more likely to form at the anode in the electrolysis of an aqueous solution of KF? Explain your reasoning.
Which product, Ca or H2, is more likely to form at the cathode in the electrolysis of CaCl2? Explain your reasoning.
An aqueous solution of KBr is placed in a beaker with two inert platinum electrodes. When the cell is attached to an external source of electrical energy, electrolysis occurs.(a) Hydrogen gas and
An aqueous solution of Na2S is placed in a beaker with two inert platinum electrodes. When the cell is attached to an external battery, electrolysis occurs.(a) Hydrogen gas and hydroxide ion form at
In the electrolysis of a solution containing Ni2+(aq), metallic Ni(s) deposits on the cathode. Using a current of 0.150 A for 12.2 minutes, what mass of nickel will form?
In the electrolysis of a solution containing Ag+(aq), metallic Ag(s) deposits on the cathode. Using a current of 1.12 A for 2.40 hours, what mass of silver forms?
Electrolysis of a solution of CuSO4(aq) to give copper metal is carried out using a current of 0.66 A. How long should electrolysis continue to produce 0.50 g of copper?
Electrolysis of a solution of Zn(NO3)2(aq) to give zinc metal is carried out using a current of 2.12 A. How long should electrolysis continue in order to prepare 2.5 g of zinc?
A voltaic cell can be built using the reaction between Al metal and O2 from the air. If the Al anode of this cell consists of 84 g of aluminum, how many hours can the cell produce 1.0 A of
Give the electron configuration for each of the following ions, and tell whether each is paramagnetic or diamagnetic.(a) Cr3+(b) V2+(c) Ni2+(d) Cu+
The reduction potentials for the Group 3A metals, E°, are given below. What trend or trends do you observe in these data? What can you learn about the chemistry of the Group 3A elements from these
Comparing the chemistry of carbon and silicon.(a) Write balanced chemical equations for the reactions of H2O(ℓ) with CH4 (forming CO2 and H2) and SiH4 (forming SiO2 and H2).(b) Using thermodynamic
Identify among the transition metals:(a) The metal with the highest melting point.(b) A commonly used metal in construction.(c) A radioactive f-block element.(d) One of the metals in nitrogenase, a
Identify two transition metal cations with each of the following electron configurations.(a) [Ar]3d6(b) [Ar]3d10(c) [Ar]3d5(d) [Ar]3d8
Identify a cation of a first series transition metal that is isoelectronic with each of the following.(a) Fe3+(b) Zn2+(c) Fe2+(d) Cr3+
Match up the isoelectronic ions on the following list. Cu+ Mn2+ Fe2+ Co3+ Fe3+ Zn2+ Ti2+ V3+
The lanthanide contraction is given as an explanation for the fact that the 6th period transition metals have(a) Lower densities than the 5th period transition elements.(b) Atomic radii similar to
Describe how the atomic radii of the transition metals change across a period and rationalize this change based on electronic structure.
In the reactionwhat element is oxidized and what element is reduced?(a) Sulfur is reduced, iron is oxidized.(b) Copper is reduced, sulfur is oxidized.(c) Sulfur is reduced, copper is oxidized.(d)
What is the most common form that iron is found in the Earth’s crust?(a) Free metal(b) Iron oxide(c) Iron sulfide(d) Iron silicate
In the pyrometallurgy of iron, what two species serve as reducing agents?
Lime (CaO) is usually added to the blast furnace in the metallurgy of iron where it reacts with impurities present in iron ore. What of the following best describes its function?(a) CaO acts as an
Which of the following ligands is expected to be monodentate, and which might be polydentate?(a) CH3NH2(b) CH3CN(c) N3−(d) en(e) Br−(f) Phen
Give the name or structural formula for each of the following ligands. Name ethylenediamine (a) (b) oxalate ion (c) (d) Formula NH3 SCN-
One of the following nitrogen compounds or ions is not capable of serving as a ligand: NH4+, NH3, NH2−. Identify this species, and explain your answer.
Give the name or structural formula for each of the following ligands. Name acetylacetonate (a) (b) nitrite ion (c) (d) Formula H₂O NO₂
Give the oxidation number of the metal ion in each of the following compounds.(a) [Mn(NH3)6]SO4(b) K3[Co(CN)6](c) [Co(NH3)4Cl2]Cl(d) Cr(en)2Cl2
Give the oxidation number of the metal ion in each of the following complexes.(a) [Fe(NH3)6]2+(b) [Zn(CN)4]2−(c) [Co(NH3)5(NO2)]+(d) [Cu(en)2]2+
Give the formula of a complex constructed from one Ni2+ ion, one ethylenediamine ligand, three ammonia molecules, and one water molecule. Is the complex neutral or is it charged? If charged, give the
Give the formula of a complex constructed from one Cr3+ ion, two ethylenediamine ligands, and two ammonia molecules. Is the complex neutral or is it charged? If charged, give the charge.
Write formulas for the following ions or compounds.(a) Dichlorobis(ethylenediamine)nickel(II)(b) Potassium tetrachloroplatinate(II)(c) Potassium dicyanocuprate(I)(d) Tetraamminediaquairon(II)
Write formulas for the following ions or compounds.(a) Diamminetriaquahydroxochromium(II) nitrate(b) Hexaammineiron(III) nitrate(c) Pentacarbonyliron(0) (where the ligand is CO)(d) Ammonium
Name the following ions or compounds.(a) [Ni(C2O4)2(H2O)2]2−(b) [Co(en)2Br2]+(c) [Co(en)2(NH3)Cl]2+(d) Pt(NH3)2(C2O4)
Name the following ions or compounds.(a) [Co(H2O)4Cl2]+(b) Co(H2O)3F3(c) [Pt(NH3)Br3]−(d) [Co(en)(NH3)3Cl]2+
Give the name or formula for each ion or compound, as appropriate.(a) Pentaaquahydroxoiron(III) ion(b) K2[Ni(CN)4](c) K[Cr(C2O4)2(H2O)2](d) Ammonium tetrachloroplatinate(II)
Give the name or formula for each ion or compound, as appropriate.(a) Tetraaquadichlorochromium(III) chloride(b) [Cr(NH3)5SO4]Cl(c) Sodium tetrachlorocobaltate(II)(d) [Fe(C2O4)3]3−
A coordination compound has the formula [Co(en)2Cl2]Cl (en = ethylenediamine, H2NCH2CH2NH2). What types of isomerism (geometric isomerism, optical isomerism, structural isomerism) are possible with
What types of isomerism (geometric isomerism, optical isomerism, structural isomerism) are possible in the compound diamminechlorothiocyanatoplatinum(II)? Identify all possible answers.
Draw all possible geometric isomers for each of the following ions or molecules.(a) Fe(NH3)4Cl2(b) Pt(NH3)2(SCN)(Br) (SCN− is bonded to Pt2+ through S)(c) Co(NH3)3(NO2)3 (NO2− is bonded to Co3+
In which of the following complexes are geometric isomers possible? If isomers are possible, draw their structures and label them as cis or trans, or as fac or mer.(a) [Co(H2O)4Cl2]+(b) Co(NH3)3F3(c)
Determine whether the following complexes have a chiral metal center.(a) [Fe(en)3]2+(b) Trans-[Co(en)2Br2]+(c) Fac-[Co(en)(H2O)Cl3](d) Square-planar Pt(NH3)(H2O)(Cl)(NO2)
Four geometric isomers are possible for [Co(en)(NH3)2(H2O)Cl]+. Draw the structures of all four. (Two of the isomers are chiral, meaning that each has a non superimposable mirror image.)
According to ligand field theory, what is the force of attraction between a metal and a ligand in a coordination complex?
Which of the following statements about ligand field theory are correct?(a) Ligands donate an electron pair to a metal ion.(b) Each ligand donates an electron pair to the metal.(c) Coordination of
In an octahedral complex, the d orbitals split into two groups. Which d orbitals are in the lower energy group? (Assume the ligands lie along the x, y, and z axes.)
In a square planar complex which d orbital is at lowest energy? Which d orbital is at highest energy? (Assume the ligands lie along the x and y axes.)
The following are low-spin complexes. Use the ligand field model to find the electron configuration of the central metal ion in each ion. Determine which are diamagnetic. Give the number of unpaired
The following are high-spin complexes. Use the ligand field model to find the electron configuration of the central metal ion in each ion. Determine the number of unpaired electrons, if any, in
Determine the number of unpaired electrons in the following tetrahedral complexes. All tetrahedral complexes are high spin.(a) [FeCl4]2−(b) Na2[CoCl4](c) [MnCl4]2−(d) (NH4)2[ZnCl4]
Determine the number of unpaired electrons in the following tetrahedral complexes. All tetrahedral complexes are high spin.(a) [Zn(H2O)4]2+(b) VOCl3(c) Mn(NH3)2Cl2(d) [Cu(en)2]2+
Xenon trioxide, XeO3, reacts with aqueous base to form the xenate anion, HXeO4−. This ion reacts further with OH− to form the perxenate anion, XeO64−, in the following reaction:Identify the
Identify, based on the position in the periodic table, the actinide elements among those in the following list: Co, Cm, Cd, Ce, Cf.
Identify, based on the position in the periodic table, the actinide elements among those in the following list: Ta, Tc, Ti, Th, Tm.
Use the periodic table to identify the elements in the following list with unfilled 4d orbitals: rhodium, rhenium, ruthenium, rutherfordium, radium.
Use the periodic table to identify the elements in the following list with unfilled 3d orbitals: cadmium, cerium, cobalt, chromium, copper.
Identify the following as either chemical or physical properties of most transition metals:(a) Can be oxidized.(b) Have unpaired electrons (paramagnetism).(c) Solids at 25°C.(d) Metallic luster.(e)
Iron is the most abundant transition element in nature. Identify common chemical and physical properties of this element.
Identity among the transition metals:(a) The most dense element.(b) The metal with the lowest melting point.(c) A radioactive d-block element.(d) An essential element in the human body.
Use the table of standard reduction potentials (Appendix M) to calculate ΔrG° for the following reactions at 298 K.Data given in Appendix M (a) 3 Cu(s) + 2NO3(aq) + 8 H+ (aq) → 3 Cu²+ (aq) + 2
Write balanced equations for the following reduction half-reactions involving organic compounds. (a) HCO₂H CH₂O (b) C6H5CO₂H → C6H₂CH3 (c) CH,CH,CHO→ (d) CH3OH →
Balance the following equations involving organic compounds. (a) Ag*(aq) + CH;CHO(aq)— Ag(s) + C6H5CO₂H(aq) (b) CH₂CH₂OH + Cr₂O,2 (aq) → CH3CO₂H(aq) + Cr³+ (aq) (acid solution) (acid
A voltaic cell is constructed in which one half-cell consists of a silver wire in an aqueous solution of AgNO3. The other half-cell consists of an inert platinum wire in an aqueous solution
An expensive but lighter alternative to the lead storage battery is the silver-zinc battery.The electrolyte is 40% KOH, and silver–silver oxide electrodes are separated from zinc–zinc hydroxide
The specifications for a lead storage battery include delivery of a steady 1.5 A of current for 15 hours.(a) What is the minimum mass of lead that will be used in the anode?(b) What mass of PbO2 must
Manganese may play an important role in chemical cycles in the oceans. Two reactions involving manganese (in acid solution) are the reduction of nitrate ions (to NO) with Mn2+ ions and the oxidation
Dinitrogen monoxide, N2O (commonly called nitrous oxide), is prepared by the careful decomposition of ammonium nitrate and is used as an oxidizing agent in rocket engines as well as a weak general
Living organisms derive energy from the oxidation of food, typified by glucose.Electrons in this redox process are transferred from glucose to oxygen in a series of at least 25 steps. It is
Iron(II) ion undergoes a disproportionation reaction to give Fe(s) and the iron(III) ion. That is, iron(II) ion is both oxidized and reduced within the same reaction.(a) What two half-reactions make
Copper(I) ion disproportionates to copper metal and copper(II) ion. (See Study Question 99.)(a) What two half-reactions make up the disproportionation reaction?(b) Use values of the standard
The simplest way to write the reaction for discharge in a lithium-ion battery is(a) What are the oxidation numbers for cobalt in the two substances in the battery?(b) In such a battery, what reaction
A lithium-ion camera battery is rated at 7500 mAh. That is, it can deliver 7500 milliamps (mA) or 7.5 amps of steady current for an hour.(a) How many moles of electrons can the battery deliver in one
Can either sodium or potassium metal be used as a sacrificial anode to protect the iron hull of a ship?

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