Homework Answers
Number of moles of electron transferred in the reaction is determined by loss or gain of electron.
So there are to method
1) balance the half reaction.amd see how many electrons are participating in balancing reaction. That will be n.
Or just see the Br- oxidation number is (-) and it is going to Br2 oxidation number is (0). So it change is 1 and there are 6 Br- so it has total charge is 6. And that is n.now u can do same with MnO4^-
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How do you find n (number moles of electrons transfered inbthe reaction) to use in the...
for the following reaction, how do you find how many electrons transferred? i understand you must...
for
the following reaction, how do you find how many electrons
transferred? i understand you must write out and balance the half
reactions but i am not sure how to do that. thanks
Identify the oxidation numbers for all the elements in the reactants and products for 2 MnO," (aq) + 39- (aq) + 4H2O(1) 3S() + 2 MnO,(s) + 8 OH(aq) Identify the oxidation numbers by dragging the appropriate labels to their respective targets. Reset Help 2 MnO2 (aq)...
TIL ELECTROCHEMISTRY Calculating standard reaction free energy from standard... Using standard reduction potentials from the ALEKS...
TIL ELECTROCHEMISTRY Calculating standard reaction free energy from standard... Using standard reduction potentials from the ALEKS Data tab, calculate the standard reaction free energy AGº for the following redox reaction. Round your answer to 3 significant digits. 2MnO, (5) +80H" (aq) + 3Br, (1) - 2 Mno, (aq) +4H20 (1) +6Br" (ag) E х ?
Calculate ∆Go for the voltaic cell shown above. n= moles of electrons transferred F= 96500 Coulomb...
Calculate ∆Go for the voltaic cell shown above.
n= moles of electrons transferred
F= 96500 Coulomb (charge on one mol of electrons)
Use the units kJ in your answer.
salt bridge Use these half-cell potentials: Cr2O72- (aq) + 14 H+ + 6e 2 Cr3+ (aq) + 7 H20 (1) O=1.36 Cl2 (9) + 2e → 2 C1 =1.33 Calculate AGº for the voltaic cell shown above. n= moles of electrons transferred F= 96500 Coulomb (charge on one mol of electrons)...
Using standard reduction potentials from the ALEKS Data tab, calculate the standard reaction free energy AGº...
Using standard reduction potentials from the ALEKS Data tab, calculate the standard reaction free energy AGº for the following redox reaction. Round your answer to 3 significant digits. 3 Mn²+ (aq) +2H20 (1)+2 (aq) + MnO2 (s) + 4H+ (aq) +2Fe2+ (aq) kJ Х
how do you find the total number of electrons transferred in the following reaction? oxidation states...
how
do you find the total number of electrons transferred in the
following reaction? oxidation states in blue
4 H2O2(aq) +C1,07(8)+2 OH-(aq) —> 2C1Oz (aq)+5 H2O(1) + 4 O2(8)
Free-energy change, AGº, is related to cell potential, Eº, by the equation AG° = -nFE° where...
Free-energy change, AGº, is related to cell potential, Eº, by the equation AG° = -nFE° where n is the number of moles of electrons transferred and F = 96,500 C/(mol e ) is the Faraday constant. When Eº is measured in volts, AGⓇ must be in joules since 1 J =1C.V. Part A Calculate the standard free-energy change at 25°C for the following reaction: Mg(s) + Fe2+ (aq)Mg2+ (aq) + Fe(s) Express your answer to three significant figures and include...
Free-energy change, ΔG∘, is related to cell potential, E∘, by the equation ΔG∘=−nFE∘ where n is...
Free-energy change, ΔG∘, is related to cell potential, E∘, by the equation ΔG∘=−nFE∘ where n is the number of moles of electrons transferred and F=96,500C/(mol e−) is the Faraday constant. When E∘ is measured in volts, ΔG∘ must be in joules since 1 J=1 C⋅V. Calculate the standard cell potential at 25 ∘C for the reaction X(s)+2Y+(aq)→X2+(aq)+2Y(s) where ΔH∘ = -679 kJ and ΔS∘ = -195 J/K .
The equilibrium constant, K, for a redox reaction is related to the standard potential, E∘, by...
The equilibrium constant, K, for a redox reaction is related to the standard potential, E∘, by the equation lnK=nFE∘RT where n is the number of moles of electrons transferred, F (the Faraday constant) is equal to 96,500 C/(mol e−) , R (the gas constant) is equal to 8.314 J/(mol⋅K) , and T is the Kelvin temperature. Calculate the standard cell potential (E∘) for the reaction X(s)+Y+(aq)→X+(aq)+Y(s) if K = 5.51×10−3.
Calculating Standard reaction et energy from standard Using standard reduction potentials from the ALEKS Data tab,...
Calculating Standard reaction et energy from standard Using standard reduction potentials from the ALEKS Data tab, calculate the standard reaction free energy AG for the following redox reaction Round your answer to 3 significant digits. 6Br" (aq) +2 MnO, (aq) + 4H,0(1) 3Br (1) + 2 MnO,($)+8OH(aq) x 5 ?
Using standard reduction potentials from the ALEKS Data tab, calculate the standard reaction free energy AGº...
Using standard reduction potentials from the ALEKS Data tab, calculate the standard reaction free energy AGº for the following redox reaction. Round your answer to 4 significant digits. 2Br (aq) + 2H2O(l) → Br2 (1) +H2 (g) +20H (aq) [kJ xo Х 5 ?
for
the following reaction, how do you find how many electrons
transferred? i understand you must write out and balance the half
reactions but i am not sure how to do that. thanks
Identify the oxidation numbers for all the elements in the reactants and products for 2 MnO," (aq) + 39- (aq) + 4H2O(1) 3S() + 2 MnO,(s) + 8 OH(aq) Identify the oxidation numbers by dragging the appropriate labels to their respective targets. Reset Help 2 MnO2 (aq)...
TIL ELECTROCHEMISTRY Calculating standard reaction free energy from standard... Using standard reduction potentials from the ALEKS Data tab, calculate the standard reaction free energy AGº for the following redox reaction. Round your answer to 3 significant digits. 2MnO, (5) +80H" (aq) + 3Br, (1) - 2 Mno, (aq) +4H20 (1) +6Br" (ag) E х ?
Calculate ∆Go for the voltaic cell shown above.
n= moles of electrons transferred
F= 96500 Coulomb (charge on one mol of electrons)
Use the units kJ in your answer.
salt bridge Use these half-cell potentials: Cr2O72- (aq) + 14 H+ + 6e 2 Cr3+ (aq) + 7 H20 (1) O=1.36 Cl2 (9) + 2e → 2 C1 =1.33 Calculate AGº for the voltaic cell shown above. n= moles of electrons transferred F= 96500 Coulomb (charge on one mol of electrons)...
Using standard reduction potentials from the ALEKS Data tab, calculate the standard reaction free energy AGº for the following redox reaction. Round your answer to 3 significant digits. 3 Mn²+ (aq) +2H20 (1)+2 (aq) + MnO2 (s) + 4H+ (aq) +2Fe2+ (aq) kJ Х
how
do you find the total number of electrons transferred in the
following reaction? oxidation states in blue
4 H2O2(aq) +C1,07(8)+2 OH-(aq) —> 2C1Oz (aq)+5 H2O(1) + 4 O2(8)
Free-energy change, AGº, is related to cell potential, Eº, by the equation AG° = -nFE° where n is the number of moles of electrons transferred and F = 96,500 C/(mol e ) is the Faraday constant. When Eº is measured in volts, AGⓇ must be in joules since 1 J =1C.V. Part A Calculate the standard free-energy change at 25°C for the following reaction: Mg(s) + Fe2+ (aq)Mg2+ (aq) + Fe(s) Express your answer to three significant figures and include...
Calculating Standard reaction et energy from standard Using standard reduction potentials from the ALEKS Data tab, calculate the standard reaction free energy AG for the following redox reaction Round your answer to 3 significant digits. 6Br" (aq) +2 MnO, (aq) + 4H,0(1) 3Br (1) + 2 MnO,($)+8OH(aq) x 5 ?
Using standard reduction potentials from the ALEKS Data tab, calculate the standard reaction free energy AGº for the following redox reaction. Round your answer to 4 significant digits. 2Br (aq) + 2H2O(l) → Br2 (1) +H2 (g) +20H (aq) [kJ xo Х 5 ?
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