Chapter 21 ALEKS

H2(g)+2OH^-(aq)

-421.8kJ and -308.6kJ

2H2O(l)+2Cl2(g)

-49.8 kJ

MnO2(s)+4OH^-(aq)

-50.9 kJ

→+3Fe2+aq+NO−3aq4H+aq+3Fe3+aq+NOg2H2Ol

-53.8kJ

→+4Br−aq+O2g4H+aq+2Br2l2H2Ol

-62.9kJ

→+2NOg+2H2OlCl2g+2HNO2aq+2H+aq2Cl−aq

-72.4kJ

Write a balanced half-reaction for the oxidation of gaseous arsine AsH3 to aqueous arsenic acid H3AsO4 in basic aqueous solution. Be sure to add physical state symbols where appropriate.

AsH3(g)+8OH^-(aq)=H3AsO4(aq)+ 4H2O(l)+8e^-

Write a balanced half-reaction for the oxidation of bismuth ion Bi3+ to bismuth oxide ion BiO−3 in basic aqueous solution. Be sure to add physical state symbols where appropriate.

Bi^3+(aq)+6OH^-(aq)=BiO3^-(aq)+3H2O(l)+2e^-

Ca+I2=CaI2

Ca=Ca^2+ + 2e^- I2+ 2e^- = 2I^-

A galvanic cell at a temperature of 25.0°C is powered by the following redox reaction: →+2Cr3+aq3Cas+2Crs3Ca2+aq Suppose the cell is prepared with 1.65 M Cr3+ in one half-cell and 1.64 M Ca2+ in the other. Calculate the cell voltage under these conditions. Round your answer to 3 significant digits.

Find Standard Reduction potentials using the Aleks Data Table. Then take the Reduction minus the Oxidation (-.744)-(-2.868)=+2.12400V Plug equation into Q (1.64)^3/(1.65)^2= 1.6202 (2.12400)-(8.31446)(298.15)/(6)(9.64853*10^4) ln(1.6202)= 2.12193 +2.12

Write a balanced half-reaction for the oxidation of aqueous hydrogen peroxide H2O2 to gaseous oxygen O2 in basic aqueous solution. Be sure to add physical state symbols where appropriate.

H2O2(aq)+2OH^-(aq)=O2(g)+2H2O(l)+ 2e^-

Write a balanced half-reaction for the reduction of aqueous hydrogen peroxide H2O2 to liquid water H2O in basic aqueous solution. Be sure to add physical state symbols where appropriate.

H2O2(aq)+2e^-=2OH^-(aq)

Write a balanced half-reaction for the reduction of aqueous nitrous acid HNO2 to gaseous nitric oxide NO in basic aqueous solution. Be sure to add physical state symbols where appropriate.

HNO2(aq)+e^-=NO(g)+OH^-(aq)

Write a balanced half-reaction for the reduction of gaseous oxygen O2 to liquid water H2O in basic aqueous solution. Be sure to add physical state symbols where appropriate.

O2(g)+2H2O(l)+4e^-=4OH^-(aq)

2CO2(g)

R: 2CO2(g)+9H2O(l)+12e^-=C2H5OH(l)+12OH^-(aq) O: Fe^2+(aq)=Fe^3+(aq)+e^-

BiO3^-(aq)

R: BiO3^-(aq)+3H2O(l)+2e^-=Bi^3+(aq)+6OH^-(aq) O: C2O4^2-(aq)=2CO2(aq)+2e^-

Cr2O7^2-

R: Cr2O7^2-(aq)+7H2O(l)+6e^-=2Cr^3+(aq)+14OH^-(aq) O:2Cl^-(aq)=Cl2(g)+2e^-

Using standard reduction potentials from the ALEKS Data tab, calculate the standard reaction free energy ΔG0 for the following redox reaction. Be sure your answer has the correct number of significant digits. →+4Cu+aq+N2g4H2Ol+4Cu2+aq+N2H4aq4OH−aq

(-1.16V)-(0.153V)=-1.3130V -(4)(9.6485*10^4)(-1.3130V)= 5.0674*10^5 =506.74kJ 507kJ

A galvanic cell at a temperature of 25.0°C is powered by the following redox reaction:→+2IO−3aq+12H+aq5Cos+I2s+6H2Ol5Co2+aqSuppose the cell is prepared with 6.25 M IO−3 and 4.22 M H+ in one half-cell and 4.55 M Co2+ in the other. Calculate the cell voltage under these conditions. Round your answer to 3 significant digits.

(1.195)-(-0.28)= 1.4750V n=10 (4.55)^5/(6.25)^2(4.22)^12 = 1.5651*10^-6 (1.4750V)-(-0.034345)= 1.51V

10Br^-(aq)+ 2IO3^-(aq)

-124.kJ

→+I2s+6H2Ol5Cl2g+2IO−3aq+12H+aq10Cl−aq

-157.kJ

→+5Zns+2MnO−4aq16H+aq+5Zn2+aq+2Mn2+aq8H2Ol

-2189.kJ

2NO(g)+4H2O(l)

-232.kJ

2Br^-(aq)+MnO2(s)

-30.5kJ

→+Zns+MnO2s4H+aq+Zn2+aq+Mn2+aq2H2Ol kJ

-383.2kJ

2Zn(s)+N2(g)

1.5*10^2kJ

→+2MnO2s+8OH−aq3Br2l+2MnO−4aq+4H2Ol6Br−aq

-273.kJ

4I2(s)

R: I2(s)+2e^-=2I^-(aq) O: AsH3(g)+4H2O(l)=H3AsO4(aq)+8H^+(aq)+8e^-

NO3^-(aq)

R: NO3^-(aq)+2H^+(aq)+e^-=NO2(g)+H2O(l) O: Cu^+(aq)=Cu^2+(aq)+e^-

5Zn^2+(aq)+ 2Mn^2+(aq)+ 8H2O(l)= 5Zn(s)+ 2MnO4^-(aq)+ 16H^+(aq)

R: Zn^2+(aq)+2e^-=Zn(s) O: Mn^2+(aq)+4H2O(l)=MnO4^-(aq)+8H^+(aq)+5e^-

→+3Zns+2CrO2−4aq8H2Ol+3Zn2+aq+2CrOH3s10OH−aq

-3.7*10^2kJ

→+2NOg+4H2Ol3Zn2+aq+2NO−3aq+8H+aq3Zns

995.1kJ

A galvanic cell at a temperature of 25.0°C is powered by the following redox reaction:→+Sn2+aqBas+SnsBa2+aqSuppose the cell is prepared with 4.86 M Sn2+ in one half-cell and 4.42 M Ba2+ in the other. Calculate the cell voltage under these conditions. Round your answer to 3 significant digits.

n=2 2.78V

A galvanic cell at a temperature of 25.0°C is powered by the following redox reaction:→+3Cu2+aq2Als+3Cus2Al3+aqSuppose the cell is prepared with 4.92 M Cu2+ in one half-cell and 2.55 M Al3+ in the other. Calculate the cell voltage under these conditions. Round your answer to 3 significant digits.

n=6 2.03V

5Fe^2+(aq)+ MnO4^-(aq)

-355.kJ

I2(s)+6H2O(l)

124.kJ and -157.kJ

→+Zns2H2Ol+Zn2+aq+H2g2OH−aq

13.

Write a balanced half-reaction for the reduction of nitrate ion NO−3 to gaseous nitric oxide NO in basic aqueous solution. Be sure to add physical state symbols where appropriate.

NO3^-(aq)+2H2O(l)+3e^-=NO(g)+4OH^-(aq)

Write a balanced half-reaction for the reduction of nitrate ion NO−3 to gaseous nitrogen dioxide NO2 in basic aqueous solution. Be sure to add physical state symbols where appropriate.

NO3^-(aq)+H2O(l)+e^-=NO2(g)+2OH^-(aq)

A galvanic cell at a temperature of 25.0°C is powered by the following redox reaction:→+2VO+2aq+4H+aqFes+2VO2+aq+2H2OlFe2+aqSuppose the cell is prepared with 1.05 M VO+2 and 4.84 M H+ in one half-cell and 7.19 M VO2+ and 2.26 M Fe2+ in the other. Calculate the cell voltage under these conditions. Round your answer to 3 significant digits.

n=2 1.46V

A galvanic cell at a temperature of 25.0°C is powered by the following redox reaction:→+2MnO−4aq+16H+aq5Pbs+2Mn2+aq+8H2Ol5Pb2+aqSuppose the cell is prepared with 4.68 M MnO−4 and 0.317 M H+ in one half-cell and 5.88 M Mn2+ and 0.556 M Pb2+ in the other. Calculate the cell voltage under these conditions. Round your answer to 3 significant digits.

1.59V n=10

3Fe^2+(aq)+CrO4^-2(aq)

2.6*10^2

A galvanic cell at a temperature of 25.0°C is powered by the following redox reaction:→+2IO−3aq+12H+aq5Cos+I2s+6H2Ol5Co2+aqSuppose the cell is prepared with 3.70 M IO−3 and 4.09 M H+ in one half-cell and 3.57 M Co2+ in the other. Calculate the cell voltage under these conditions. Round your answer to 3 significant digits.

n=10 1.51

NO(g)+H2O(l)

20.5kJ

Write a balanced half-reaction for the oxidation of chromium ion Cr3+ to dichromate ion Cr2O2−7 in basic aqueous solution. Be sure to add physical state symbols where appropriate.

2Cr^+(aq)+14OH^-(aq)=CrO7^2-(aq)+7H2O(l)+6e^-

→+2CrOH3s+10OH−aq3Zn2+aq+2CrO2−4aq+8H2Ol3Zns

3.7*10^2kJ

A galvanic cell at a temperature of 25.0°C is powered by the following redox reaction:→+2MnO−4aq+16H+aq5Pbs+2Mn2+aq+8H2Ol5Pb2+aqSuppose the cell is prepared with 1.46 M MnO−4 and 2.85 M H+ in one half-cell and 7.25 M Mn2+ and 7.21 M Pb2+ in the other. Calculate the cell voltage under these conditions. Round your answer to 3 significant digits.

n=10 1.64V

Mn^2+(aq)+ 2H2O(l)

30.5kJ

→+I2s+6H2Ol10Fe3+aq+2IO−3aq+12H+aq10Fe2+aq

409.kJ

→+2H2Ol4Cu2+aq+O2g+4H+aq4Cu+aq

415.3kJ

2Cl^-(aq)+2H2O(l)

421.8kJ

→+6Cl−aq+2MnO−4aq4H2Ol+3Cl2g+2MnO2s8OH−aq

442.kJ

→+3Fe2+aq+MnO−4aq2H2Ol+3Fe3+aq+MnO2s4OH−aq

50.9kJ

→+4Cu+aq+N2g4H2Ol+4Cu2+aq+N2H4aq4OH−aq

507.kJ

4Br^-(aq)+N2(g)

859.kJ

6Cl^-(aq)+2CrO4^2-(aq)

861.kJ

Mn^2+(aq)+2H2O(l)

87.4kJ

Write a balanced half-reaction for the oxidation of solid iodine dioxide IO2 to iodate ion IO−3 in basic aqueous solution. Be sure to add physical state symbols where appropriate.

IO2(s)+2OH^-(aq)=IO3^-(aq)+H2O(l)+e^-

Write a balanced half-reaction for the oxidation of solid manganese dioxide MnO2 to permanganate ion MnO−4 in basic aqueous solution. Be sure to add physical state symbols where appropriate.

MnO2(s)+4OH^-(aq)=MnO4^-(aq)+2H2O(l)+3e^-

Write a balanced half-reaction for the reduction of permanganate ion MnO−4 to manganese ion Mn2+ in basic aqueous solution. Be sure to add physical state symbols where appropriate.

MnO4^-(aq)+4H2O(l)+5e^-=Mn^2+(aq)+8OH^-(aq)

Write a balanced half-reaction for the oxidation of manganese ion Mn2+ to solid manganese dioxide MnO2 in basic aqueous solution. Be sure to add physical state symbols where appropriate.

Mn^2+(aq)+4OH^-(aq)=MnO2(s)+2H2O(l)+2e^-

Write a balanced half-reaction for the reduction of gaseous nitrogen N2 to aqueous hydrazine N2H4 in basic aqueous solution. Be sure to add physical state symbols where appropriate.

N2(g)+4H2O(l)+4e^-=N2H4(aq)+4OH^-(aq)

Write a balanced half-reaction for the oxidation of gaseous nitric oxide NO to aqueous nitrous acid HNO2 in basic aqueous solution. Be sure to add physical state symbols where appropriate.

NO(g)+OH^-(aq)=HNO2(aq)+e^-

A galvanic cell at a temperature of 25.0°C is powered by the following redox reaction:→+Cu2+aqZns+CusZn2+aqSuppose the cell is prepared with 6.83 M Cu2+ in one half-cell and 0.616 M Zn2+ in the other. Calculate the cell voltage under these conditions. Round your answer to 3 significant digits.

n=2 1.13V

A galvanic cell at a temperature of 25.0°C is powered by the following redox reaction:→+2VO+2aq+4H+aqFes+2VO2+aq+2H2OlFe2+aqSuppose the cell is prepared with 4.34 M VO+2 and 2.85 M H+ in one half-cell and 6.46 M VO2+ and 4.55 M Fe2+ in the other. Calculate the cell voltage under these conditions. Round your answer to 3 significant digits.

n=2 1.46V

A galvanic cell at a temperature of 25.0°C is powered by the following redox reaction:→+MnO2s+4H+aq2Cr2+aq+Mn2+aq+2H2Ol2Cr3+aqSuppose the cell is prepared with 2.23 M H+ and 6.47 M Cr2+ in one half-cell and 4.53 M Mn2+ and 6.35 M Cr3+ in the other. Calculate the cell voltage under these conditions. Round your answer to 3 significant digits.

n=2 1.65V

A galvanic cell at a temperature of 25.0°C is powered by the following redox reaction:→+2Cr3+aq3Cas+2Crs3Ca2+aqSuppose the cell is prepared with 7.08 M Cr3+ in one half-cell and 5.43 M Ca2+ in the other. Calculate the cell voltage under these conditions. Round your answer to 3 significant digits.

n=6 2.12V