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Chemistry
Q:
Elemental sodium is commercially produced by electrolysis of ____. A valuable by-product, ____, is simultaneously produced during the electrolysis.
A.NaCl(), Cl2(g)
B.NaH(g), H2(g)
C.NaCl(aq), NaOH(aq)
D.Na2O2(), O2(g)
E.Na2S(s), S8(s)
Q:
The principal product of the reaction of potassium and oxygen is not K2O. The product is named ____ and has the formula ____.
A.dipotassium trioxide, K2O3
B.potassium monoxide, KO
C.potassium superoxide, KO2
D.potassium peroxide, K2O2
E.potassium trioxide, KO3
Q:
Which of the following statements concerning sodium and potassium is/are CORRECT?
1/ The sodium concentration in seawater is over three times greater than the concentration of potassium.
2/ Plants contain roughly four to six times more sodium than potassium.
3/ Roman soldiers were paid in sodium chloride.
A.1 only
B.2 only
C.3 only
D.1 and 3
E.1, 2, and 3
Q:
All of the following statements concerning sodium are correct EXCEPT
A.most sodium compounds are water soluble.
B.sodium is soft and easily cut with a knife.
C.sodium is usually found in nature as the reduced metal or as a sulfide salt.
D.sodium ions help regulate osmotic pressure in the human body.
E.sodium is commercially prepared by electrolysis of molten NaCl.
Q:
All of the following elements or compounds react with water to produce hydrogen gas EXCEPT ____.
A.Na(s)
B.MgH2(s)
C.Ca(s)
D.LiH(s)
E.CaO(s)
Q:
Metal hydrides are used to remove traces of water from nonpolar solvents. Write a balanced chemical equation for the reaction of lithium hydride and water.
A.LiH2(s) + 2 H2O() Li(s) + 2 H3O+(aq)
B.2 LiH(s) + 2 H2O() 2 LiOH(s) + H2(g)
C.2 LiH(s) + H2O() Li2O(s) + 2 H2(g)
D.2 LiH(s) + H2O() Li2O(s) + 4 H+(aq)
E.LiH(s) + H2O() Li(s) + H3O+(aq)
Q:
Catalytic steam reformation of hydrocarbons (such as methane) produce a mixture of
A.CO2 and H2O.
B.C and H2.
C.O2 and H2.
D.CH4 and H2O.
E.CO and H2.
Q:
Which of the following chemical equations shows the formation of synthesis gas?
A.2 H2O(g) 2 H2(g) + O2(g)
B.16 CH4(g) + 7 O2(g) 2 C8H18(g) + 14 H2O(g)
C.C(s) + 2 H2(g) CH4(g)
D.CO(g) + H2O(g) CO2(g) + H2(g)
E.C(s) + H2O(g) H2(g) + CO(g)
Q:
Approximately 300 billion liters of hydrogen is produced annually. The majority of the hydrogen is used in the production of ____.
A.ammonia
B.hydrogen chloride
C.methane
D.sulfuric acid
E.water
Q:
Which of the following is not a likely oxidation number for iodine?
A.-1
B.0
C.+1
D.+2
E.+7
Q:
Which of the following compounds is a common oxide for phosphorus?
A.PO
B.P2O3
C.PO3
D.PO5
E.P4O10
Q:
Predict the formula of the product of a reaction of silicon and oxygen.
A.SiO
B.SiO2
C.Si2O3
D.SiO3
E.SiO4
Q:
Use your knowledge of group properties to predict the chemical formula for selenic acid.
A.HSeO2
B.H2SeO3
C.H2SeO4
D.H3SeO3
E.H3SeO4
Q:
Predict the chemical formula for the bromite ion.A.Br-B.BrO4-C.BrO3-D.BrO2-E.BrO-
Q:
What is the highest oxidation state of arsenic?A.-3B.0C.+3D.+5E.+8
Q:
What is the charge on a nonmetallic, monatomic ion from Group 5A?
A.5+
B.1+
C.1"
D.3"
E.5"
Q:
Which two elements are most abundant in our solar system?
A.hydrogen and helium
B.hydrogen and oxygen
C.helium and iron
D.hydrogen and iron
E.carbon and oxygen
Q:
Which list contains the three most abundant elements in the Earth's crust?
A.hydrogen, helium, and lithium
B.sodium, calcium, and iron
C.oxygen, nitrogen, and iron
D.carbon, nitrogen, and oxygen
E.oxygen, aluminum, and silicon
Q:
Explain the function of a salt bridge in a voltaic cell.
Q:
Write balanced reduction and oxidation half-reactions for the processes that occur at the cathode and anode of a fuel cell used aboard NASA's space shuttles.
Q:
When a secondary battery provides electrical energy, it is acting as a voltaic cell. When the battery is recharging, it is operating as a(n) ________ cell.
Q:
If electric current is passed through a solution of molten KBr, the product at the cathode is ________.
Q:
The use of electrical energy to produce chemical change is known as ________. An example of this process is the reduction of NaCl() to produce Na(s).
Q:
Gold and platinum are commonly used as inert electrodes in laboratory experiments. In commercial applications, such as batteries, ________ is more commonly used for inert electrodes because it is far less expensive.
Q:
In an electrolytic cell, reduction occurs at the ________ and oxidation occurs at the ________.
Q:
One kind of battery used in watches contains mercury(II) oxide. As current flows, the mercury(II) oxide is reduced to mercury.HgO(s) + H2O() + 2 e- Hg() + 2 OH-(aq)If 2.3 10-5 amperes flows continuously for 1200 days, what mass of Hg() is produced?A.2.5 gB.5.0 gC.9.9 gD.13 gE.15 g
Q:
Al3+ is reduced to Al(s) at an electrode. If a current of 2.75 ampere is passed for 36 hours, what mass of aluminum is deposited at the electrode? Assume 100% current efficiency.A.9.2 10-3 gB.3.3 101 gC.9.9 101 gD.1.0 102 gE.3.0 102 g
Q:
What charge, in coulombs, is required to deposit 1.5 g Mg(s) from a solution of Mg2+(aq)?
A.4.1 102 C
B.6.0 103 C
C.1.2 104 C
D.2.9 105 C
E.3.1 106 C
Q:
Calculate the standard reduction potential for the following reaction at 25 C,AuCl4-(aq) + 3 e- Au(s) + 4 Cl-(aq)given the following thermodynamic information.Au3+(aq) + 3 e- Au(s) E = +1.50 VAu3+(aq) + 4 Cl-(aq) AuCl4-(aq) Kf = 2.3 1025A.-1.28 VB.-0.50 VC.+1.00 VD.+1.28 VE.+3.85 V
Q:
Given the following standard reduction potentials,Pb2+(aq) + 2 e- Pb(s) E = -0.126 VPbSO4(s) + 2 e- Pb(s) + SO42-(aq) E = -0.355 Vdetermine Ksp for PbSO4(s) at 25 C.A.3.4 10-28B.1.8 10-8C.5.6 10-5D.5.6 107E.2.9 1037
Q:
Calculate the equilibrium constant for the following reaction at 25 C,2 IO3-(aq) + 5 Hg() + 12 H+(aq) I2(s) + 5 Hg2+(aq) + 6 H2O()given the following thermodynamic information.IO3-(aq) + 6 H+(aq) + 5 e- I2(s) + 3 H2O() E = +1.20 VHg2+(aq) + 2 e- Hg() E = +0.86 VA.3 10-58B.6 105C.3 1011D.6 1028E.3 1057
Q:
Calculate the equilibrium constant for the reaction below at 25 C,Co(s) + 2 Cr3+(aq) Co2+(aq) + 2 Cr2+(aq)given the following thermodynamic information.Co2+(aq) + 2 e- Co(s) E = -0.28 VCr3+(aq) + e- Cr2+(aq) E = -0.41 VA.4.0 10-5B.2.5 104C.1.0 105D.1.2 105E.1.3 105
Q:
If DrG for the following reaction is -22.2 kJ/mol-rxn, calculate .Cu2+(aq) + 2 Ag(s) + 2 Cl-(aq) Cu(s) + 2 AgCl(s)A.-0.460 VB.-0.115 VC.+0.115 VD.+0.230 VE.+0.559 V
Q:
Calculate DrG for the disproportionation reaction of Cu+ at 25 C,2 Cu+(aq) Cu2+(aq) + Cu(s)given the following thermodynamic information.Cu+(aq) + e- Cu(s) E = +0.518 VCu2+(aq) + 2 e- Cu(s) E = +0.337 VA.-165 kJ/molrxnB.-135 kJ/molrxnC.-34.9 kJ/molrxnD.+17.5 kJ/molrxnE.+135 kJ/molrxn
Q:
for the following galvanic cell is -1.80 V.Fe2+(aq) + 2 Cl-(aq) Fe(s) + Cl2(g)What is DrG for this reaction?A.-174 kJB.86.8 kJC.107 kJD.174 kJE.347 kJ
Q:
The standard cell potential of the following electrochemical cell is 0.19 V.
Pt | Sn4+(aq, 1.0 M), Sn2+(aq, 1.0 M) || Cu2+(aq, 0.200 M) | Cu
Which factor will increase measured cell potential of the galvanic cell?
A.switching from a platinum to a graphite anode
B.increasing the size of the anode
C.decreasing the concentration of Cu2+
D.increasing the concentration of Sn4+
E.decreasing the temperature of the cell
Q:
What is the pH of the solution at the cathode if = -0.362 V for the following electrochemical cell at 25 C?Pt | H2(g, 1.0 atm) | H+(aq, 1.00 M) || H+(aq) | H2(g, 1.0 atm) | PtA.1.77B.3.06C.6.11D.7.89E.12.23
Q:
The following electrochemical cell has a potential of +0.326 V at 25 C.Pt | H2(g, 1.00 atm) | H+(aq, 1.00 M) || Cl-(aq) | AgCl(s) | AgThe standard reduction potential,E, of AgCl(s) = +0.222 V. What is the Cl-(aq) concentration?A.1.9 10-19 MB.5.5 10-10 MC.0.018 MD.1.03 ME.1.8 109 M
Q:
Calculate the cell potential, at 25 C, based upon the overall reactionZn2+(aq) + 2 Fe2+(aq) Zn(s) + 2 Fe3+(aq)if [Zn2+] = 1.50 10-4 M, [Fe3+] = 0.0200 M, and [Fe2+] = 0.0100 M. The standard reduction potentials are as follows:Zn2+(aq) + 2 e- Zn(s) E = -0.763 VFe3+(aq) + e- Fe2+(aq) E = +0.771 VA.-1.665 VB.-1.534 VC.-1.439 VD.-0.008 VE.+0.008 V
Q:
Calculate Ecell for the following electrochemical cell at 25 CPt(s) | Fe3+(aq, 0.100 M), Fe2+(aq, 0.040 M) || Cl-(aq, 0.50 M) | AgCl(s) | Ag(s)given the following standard reduction potentials.AgCl(s) + e- Ag(s) + Cl-(aq) E = +0.222 VFe3+(aq) + e-Fe2+(aq) E = +0.771 VA.-1.034 VB.-0.590 VC.-0.508 VD.-0.555 VE.+1.034 V
Q:
Calculate Ecell for the following electrochemical cell at 25 CPt(s) | H2(g, 1.00 atm) | H+(aq, 1.00 M) || Sn2+(aq, 0.350 M), Sn4+(aq, 0.020 M) | Pt(s)given the following standard reduction potentials.Sn4+(aq) + 2 e- Sn2+(s) E = +0.15 V2 H+(aq) + 2 e- H2(g) E = 0.00 VA.-0.19 VB.+0.08 VC.+0.11 VD.+0.19 VE.+0.22 V
Q:
A Faraday, F, is defined as
A.the charge on a single electron.
B.the charge, in coulombs, carried by one mole of electrons.
C.the voltage required to reduce one mole of reactant.
D.the moles of electrons required to reduce one mole of reactant.
E.the charge passed by one ampere of current in one second.
Q:
Which of the following equations is a correct form of the Nernst equation?
A.
B.
C.
D.
E.
Q:
Calculate for the electrochemical cell below,Ag(s) | AgCl(s) | Cl-(aq) || Cu2+(aq) | Cu(s)given the following standard reduction potentials.Cu2+(aq) + 2 e- Cu(s) E = +0.337 VAgCl(s) + e- Ag(s) + Cl-(aq) E = +0.222 VA.-0.115 VB.-0.107 VC.+0.115 VD.+0.452 VE.+0.559 V
Q:
Calculate for the electrochemical cell below,Pb(s) |PbCl2(s) | Cl-(aq, 1.0 M) || Fe3+(aq, 1.0 M), Fe2+(aq, 1.0 M) | Pt(s)given the following reduction half-reactions.Pb2+(aq) + 2 e-Pb(s) E = -0.126 VPbCl2(s) + 2 e- Pb(s) + 2 Cl-(aq) E = -0.267 VFe3+(aq) + e- Fe2+(aq) E = +0.771 VFe2+(aq) + e- Fe(s) E = -0.44 VA.-0.504 VB.-0.062 VC.+0.504 VD.+1.038 VE.+1.604 V
Q:
Calculate for the reaction below,5 Cd(s) + 2 MnO4-(aq) + 16 H+(aq) 5 Cd2+(aq) + 2 Mn2+(aq) + 8 H2O()given the following standard reduction potentials.MnO4-(aq) + 8 H+(aq) + 5 e- Mn2+(aq) + 4 H2O() E = +1.52 VCd2+(aq) + 2 e- Cd(s) E = -0.40 VA.-1.12 VB.+1.04 VC.+1.92VD.+5.04 VE.+8.40 V
Q:
Calculate for the reaction below,2 AgBr(aq) + 2 Hg(l) 2 Ag(s) + Hg2Br2(s)given the following standard reduction potentials.Hg2Br2(s) + 2 e- 2 Hg(l) + 2 Br-(aq) E = +0.140 VAgBr(aq) + e- Ag(s) + Br-(aq) E = +0.071 VA.-0.211 VB.-0.069 VC.+1.97 VD.+0.069 VE.+0.211 V
Q:
Given the following two half-reactions, write the overall reaction in the direction in which it is spontaneous and calculate the standard cell potential.Pb2+(aq) + 2 e- Pb(s) E = -0.126 VFe3+(aq) + e- Fe2+(s) E = +0.771 VA.Pb2+(aq) + 2 Fe2+(s) Pb(s) + 2 Fe3+(aq) = +0.897 VB.Pb2+(aq) + Fe2+(s) Pb(s) + Fe3+(aq) = +0.645 VC.Pb(s) + 2 Fe3+(aq) Pb2+(aq) + 2 Fe2+(s) = +1.416 VD.Pb(s) + 2 Fe3+(aq) Pb2+(aq) + 2 Fe2+(s) = +0.897 VE.Pb(s) + Fe3+(aq) Pb2+(aq) + Fe2+(s) = +0.645 V
Q:
Given the following two half-reactions, write the overall balanced reaction in the direction in which it is spontaneous and calculate the standard cell potential.Ga3+(aq) + 3 e- Ga(s) E = -0.53 VSn4+(aq) + 2 e- Sn2+(aq) E = +0.15 VA.2 Ga3+(aq) + 3 Sn2+(aq) 2 Ga(s) + 3 Sn4+(aq) = +0.68 VB.3 Ga3+(aq) + 2 Sn2+(aq) 3 Ga(s) + 2 Sn4+(aq) = -1.89 VC.2 Ga(s) + 3 Sn4+(aq) 2 Ga3+(aq) + 3 Sn2+(aq) = +0.68 VD.3 Ga(s) + 2 Sn4+(aq) 3 Ga3+(aq) + 2 Sn2+(aq) = +0.38 VE.2 Ga(s) + 3 Sn4+(aq) 2 Ga3+(aq) + 3 Sn2+(aq) = +1.89 V
Q:
Consider the following half-reactions:Cl2(g) + 2 e- 2 Cl-(aq) E = +1.36 VAg+(aq) + e- Ag(s) E = +0.80 VCu2+(aq) + 2 e- Cu(s) E = +0.34 VSn2+(aq) + 2 e- Sn(s) E = -0.14 VAl3+(aq) + 3 e- Al(s) E = -1.66 VWhich of the above elements or ions will reduce Cu2+(aq)?A.Ag(s) and Sn2+(aq)B.Cl-(aq) and Ag(s)C.Cl2(g) and Ag+(aq)D.Sn(s) and Al(s)E.Sn2+(aq) and Al3+(aq)
Q:
Consider the following half-reactions:Ag+(aq) + e- Ag(s) E = +0.80 VCu2+(aq) + 2 e- Cu(s) E = +0.34 VPb2+(aq) + 2 e- Pb(s) E = -0.13 VFe2+(aq) + 2 e- Fe(s) E = -0.44 VAl3+(aq) + 3 e- Al(s) E = -1.66 VWhich of the above metals or metal ions will oxidize Pb(s)?A.Ag+(aq) and Cu2+(aq)B.Ag(s) and Cu(s)C.Fe2+(aq) and Al3+(aq)D.Fe(s) and Al(s)E.Cu2+(aq) and Fe2+(aq)
Q:
Which of the following species are likely to behave as oxidizing agents: Li(s), H2(g), MnO4-(aq), and Cl-(aq)?A.Li(s) onlyB.MnO4-(aq) onlyC.H2(g) and Cl-(aq)D.Li(s) and MnO4-(aq)E.Cl-(aq) only
Q:
Use the standard reduction potentials below to determine which element or ion is the best reducing agent.NO3-(aq) + 4 H+(aq) + 3 e- NO(g) + 2 H2O() E = +0.955 VPd2+(aq) + 2 e- Pd(s) E = +0.90 V2 H+(aq) + 2 e- H2(g) E = 0.00 VA.Pd2+(aq)B.Pd(s)C.H+(aq)D.H2(g)E.NO3-(aq)
Q:
Use the standard reduction potentials below to determine which element or ion is the best oxidizing agent.O2(g) + 4 H+(aq) + 4 e- 2 H2O() E = +1.229 VHg22+(aq) + 2 e- 2 Hg() E = +0.789 VI2(s) + 2 e- 2 I-(aq) E = +0.535 VA.I2(s)B.O2(g)C.I-(aq)D.Hg22+(aq)E.H2O()
Q:
An SHE electrode has been assigned a standard reduction potential, E, of 0.00 Volts. Which reaction occurs at this electrode?A.2 H2O() + 2 e- H2(g) + 2 OH-(aq)B.O2(g) + 4 e- 2 O2-(aq)C.Hg2Cl2(s) + 2 e- 2 Hg() + 2 Cl-(aq)D.Li+(aq) + e- Li(s)E.2 H+(aq) + 2 e- H2(g)
Q:
Which of the following are standard conditions for an electrochemical cell?
1/ Solutes in aqueous solution has a concentration of 1 M.
2/ Gaseous reactants or products have a pressure of 1 bar.
3/ Solids are present in quantities of 1 mole.
A.1 only
B.2 only
C.3 only
D.1 and 2
E.1, 2, and 3
Q:
The unit for electromotive force, emf, is the Volt. A Volt is equal to
A.one joule per second.
B.one coulomb per joule.
C.one joule per coulomb.
D.one coulomb per second.
E.one second per joule.
Q:
The fuel cells used aboard NASA's Space Shuttles are electrochemical cells that generate electricity from which overall chemical reaction?
A.Fe2O3(s) + Al(s) Fe(s) + Al2O3(s)
B.Pb(s) + PbO2(s) + 2 H2SO4(aq) 2 PbSO4(s) + 2 H2O()
C.2 NiO(OH)(s) + Cd(s) + H2O() 2 Ni(OH)2(s) + Cd(OH)2(s)
D.2 H2(g) + O2(g) 2 H2O()
E.N2H4() + O2(g) N2(g) + 2 H2O()
Q:
Which of the following statements is/are CORRECT?
1/ A nickel-cadmium battery is an example of a secondary or rechargable battery, often used in rechargable cordless appliances.
2/ Hydrogen-oxygen fuel cells use the heat of combustion of hydrogen to recharge lead storage batteries.
3/ LeClanch cells are the most efficient rechargable batteries, but they are rarely used due their high cost of production.
A.1 only
B.2 only
C.3 only
D.1 and 3
E.1, 2, and 3
Q:
Write a balanced net ionic equation for the overall reaction represented by the cell notation below.Ag(s) | AgI(s) | I-(aq) || Fe2+(aq), Fe3+(aq) | PtA.Fe3+(aq) + Ag(s) + I-(aq) Fe2+(aq) + AgI(s)B.Fe2+(aq) + Ag(s) + I-(aq) Fe3+(aq) + AgI(s)C.Fe3+(aq) + AgI(s) Fe2+(aq) + Ag(s) + I-(aq)D.Fe2+(aq) + AgI(s) Fe3+(aq) + Ag(s) + I-(aq)E.Fe3+(aq) + 2 I-(aq) Fe2+(aq) + I2(s)
Q:
Write a balanced chemical equation for the overall reaction represented by the cell notation below.
Zn(s) | Zn2+(aq) || H+(aq) | H2(g) | Pt(s)
A.H2(g) + Zn(s) 2 H+(aq) + Zn2+(aq)
B.2 H+(aq) + Zn2+(aq) H2(g) + Zn(s)
C.2 H+(aq) + Zn(s) H2(g) + Zn2+(aq)
D.2 H+(aq) + Zn(s) ZnH2(s)
E.H2(g) + Zn2+(aq) 2 H+(aq) + Zn(s)
Q:
What is a correct cell notation for a voltaic cell based on the reaction below?Cu2+(aq) + Pb(s) + SO42-(aq) Cu(s) + PbSO4(s)A.Pb(s) | PbSO4(s) || Cu2+(aq) || Cu(s)B.Cu(s) | Cu2+(aq) || SO42-(aq) | PbSO4(s) | Pb(s)C.Cu(s) | Cu2+(aq), SO42-(aq) | PbSO4(s) | Pb(s)D.Cu(s) | Cu2+(aq), SO42-(aq) || PbSO4(s) || Pb(s)E.Pb(s) | PbSO4(s) | SO42-(aq) || Cu2+(aq) || Cu(s)
Q:
What is the correct cell notation for a voltaic cell based on the reaction below?
Cu2+(aq) + Fe(s) Cu(s) + Fe2+(aq)
A.Cu(s) | Cu2+(aq) || Fe2+(aq) | Fe(s)
B.Fe(s) || Fe2+(aq), Cu2+(aq) | Cu(s)
C.Cu(s) || Cu2+(aq), Fe2+(aq) || Fe(s)
D.Cu(s) | Fe2+(aq) || Cu2+(aq) | Fe(s)
E.Fe(s) | Fe2+(aq) || Cu2+(aq) | Cu(s)
Q:
All of the following statements concerning voltaic cells are true EXCEPT
A.a salt bridge allows cations and anions to move between the half-cells.
B.electrons flow from the cathode to the anode in the external circuit.
C.oxidation occurs at the anode.
D.a voltaic cell can be used as a source of energy.
E.a voltaic cell consists of two-half cells.
Q:
Write a balanced chemical equation for the following reaction in a basic solution.ClO-(aq) + Cr(OH)3(s) Cl-(aq) + CrO42-(aq)A.3 ClO-(aq) + 2 Cr(OH)3(s) + 4 OH-(aq) 3 Cl-(aq) + 2 CrO42-(aq) + 5 H2O()B.ClO-(aq) + Cr(OH)3(s) + 3 OH-(aq) Cl-(aq) + CrO42-(aq) + 3 H2O()C.2 ClO-(aq) + 3 Cr(OH)3(s) + 3 OH-(aq) 2 Cl-(aq) + 3 CrO42-(aq) + 6 H2O()D.4 ClO-(aq) + Cr(OH)3(s) + 4 OH-(aq) Cl-(aq) + CrO42-(aq) + 6 H2O()E.ClO-(aq) + Cr(OH)3(s) Cl-(aq) + CrO42-(aq) + 3 H+(aq)
Q:
Write a balanced chemical equation for the oxidation of Cd(s) by concentrated nitric acid, producing NO2(g) and Cd2+(aq).A.HNO3(aq) + Cd(s) Cd2+(aq) + NO2(g) + OH-(aq)B.2 HNO3(aq) + Cd(s) Cd2+(aq) + 2 NO2(g) + 2 OH-(aq)C.HNO3(aq) + Cd(s) + H+(aq) Cd2+(aq) + NO2(g) + H2O()D.4 HNO3(aq) + Cd(s) Cd2+(aq) + 2 NO2(g) + 2H2O() + 2 NO3-(aq)E.HNO3(aq) + Cd(s) Cd2+(aq) + NO2(g)
Q:
Write a balanced chemical equation for the following reaction in an acidic solution.Cr2O72-(aq) + Ni(s) Cr3+(aq) + Ni2+(aq)A.Cr2O72-(aq) + 3 Ni(s) + 14 H+(aq) 2 Cr3+(aq) + 3 Ni2+(aq) + 7 H2O()B.Cr2O72-(aq) + Ni(s) + 14 H+(aq) 2 Cr3+(aq) + Ni2+(aq) + 7 H2O()C.Cr2O72-(aq) + 3 Ni(s) 2 Cr3+(aq) + 3 Ni2+(aq) + O2-(aq)D.Cr2O72-(aq) + Ni(s) + 14 H+(aq) 2 Cr3+(aq) + Ni2+(aq) + 7 H2O()E.Cr2O72-(aq) + 3 Ni(s) + 7 H+(aq) 2 Cr3+(aq) + 3 Ni2+(aq) + 7 OH-(aq)
Q:
Write a balanced half-reaction for the reduction of CrO42-(aq) to Cr(OH)3(s) in a basic solution.A.CrO42-(aq) + 3 OH-(aq) + 3 e- Cr(OH)3(s) + 2 O2(g)B.CrO42-(aq) + 3 H+(aq) + 3 e- Cr(OH)3(s)C.CrO42-(aq) + 3 H+(aq) Cr(OH)3(s) + 2 e-D.CrO42-(aq) + 4 H2O() + 3 e- Cr(OH)3(s) + 5 OH-(aq)E.CrO42-(aq) + 3 OH-(aq) Cr(OH)3(s) + 2 O2(g)
Q:
Write a balanced half-reaction for the reduction of NO3-(aq) to NO(g) in an acidic solution.A.NO3-(aq) + 4 H+(aq) NO(g) + 2 H2O()B.NO3-(aq) + 4 H+(aq) + 3 e- NO(g) + 2 H2O()C.NO3-(aq) + 3 e- NO(g) + O2(g)D.NO3-(aq) + 4 e- NO(g) + O2(g)E.NO3-(aq) + 4 H+(aq) NO(g) + 2 H2O() + 2 e-
Q:
Write a balanced half-reaction for the reduction of hydrogen peroxide to water in an acidic solution.A.2 H2O2() 2 H2O() + O2(g)B.2 H2O2() + 2e- 2 H2O() + O2(g)C.H2O2() + 2 H+(aq) + 2 e- 2 H2O()D.H2O2() + 4 H+(aq) + 2 e- 2 H2O() + H2(g)E.H2O2() + 2 H+(aq) + 4 e-2 H2(g) + O2(g)
Q:
The following reaction occurs spontaneously.2 Fe(s) + 3 Cl2(aq) 2 Fe3+(aq) + 6 Cl-(aq)Write the balanced reduction half-reaction.A.Fe(s) Fe3+(aq) + e-B.Fe(s) + 3 e- Fe3+(aq)C.Fe(s) + 3/2 Cl2(aq) FeCl3(aq)D.Cl2(aq) 2 Cl-(aq) + 2 e-E.Cl2(aq) + 2 e- 2 Cl-(aq)
Q:
The following reaction occurs spontaneously.2 H+(aq) + Ca(s) Ca2+(aq) + H2(g)Write the balanced oxidation half-reaction.A.2 H+(aq) + 2 e- H2(g)B.2 H+(aq) H2(g) + 2 e-C.H2(g) 2 H+(aq) + 2 e-D.Ca(s) + 2 e- Ca2+(aq)E.Ca(s) Ca2+(aq) + 2 e-
Q:
Assuming the following reaction proceeds in the forward direction,
Fe3+(aq) + Co(s) Fe2+(aq) + Co2+(aq)
A.Fe3+(aq) is oxidized and Co(s) is reduced.
B.Fe3+(aq) is oxidized and Co2+(aq) is reduced.
C.Co(s) is oxidized and Fe3+(aq) is reduced.
D.Co(s) is oxidized and Co2+(aq) is reduced.
E.Fe2+(aq) is oxidized and Co(s) is reduced.
Q:
Assuming the following reaction proceeds in the forward direction,
3 Sn4+(aq) + 2 Cr(s) 3 Sn2+(aq) + 2 Cr3+(aq)
A.Sn4+(aq) is the reducing agent and Cr(s) is the oxidizing agent.
B.Cr(s) is the reducing agent and Sn2+(aq) is the oxidizing agent.
C.Sn4+(aq) is the reducing agent and Sn2+(aq) is the oxidizing agent.
D.Cr(s) is the reducing agent and Cr3+(aq) is the oxidizing agent.
E.Cr(s) is the reducing agent and Sn4+(aq) is the oxidizing agent.
Q:
In any chemical process, energy must be conserved. This is a statement of the ________ law of thermodynamics.
Q:
Calculate DrG for the following reaction at 425 C,
2 HI(g) H2(g) + I2(g)
given K = 0.018. (R = 8.314 J/Kmol)
A.6.12 103 J
B.1.05 104 J
C.1.42 104 J
D.2.33 104 J
E.3.34 105 J
Q:
The solubility product equilibrium constant, Ksp, of silver bromide is 5.4 10-13 at 298 K.
AgBr(s) Ag+(aq) + Br-(aq)
What is DrG? (R = 8.314 J/Kmol)
A.-3.0 101 kJ/mol
B.-5.87 kJ/mol
C.5.87 kJ/mol
D.3.0 101 kJ/mol
E.7.0 101 kJ/mol
Q:
What is the equilibrium constant for reaction below at 25 C? (R = 8.314 J/Kmol)2 NO(g) + O2(g) 2 NO2(g)given DfG [NO(g)] = +86.6 kJ/mol and DfG [NO2(g)] = +51.2 kJ/mol.A.3.9 10-13B.1.0C.2.6 1012D.1.6 106E.3.8 1028
Q:
What is the equilibrium constant for the reaction below at 25 C? (R = 8.314 J/Kmol)MgCO3(s) MgO(s) + CO2(g)given DfG [MgCO3(s)] = -1028.2 kJ/mol, DfG [MgO(s)] = -568.8 kJ/mol, and DfG [CO2(g)] = -394.4 kJ/mol.A.4.0 10-12B.0.97C.1.0D.1.0 104E.2.5 1011
Q:
The standard free energy change associated with the dissolution of ammonium nitrate in water is -6.73 kJ/mol at 298.15 K.NH4NO3(s) NH4NO3(aq)What is the equilibrium constant for the reaction? (R = 8.314 J/Kmol)A.1.9 10-3B.6.6 10-2C.1.0D.15E.5.2 102