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18 Nov 2019

The following reaction occurs in pure water:

H2O(l) + H2O(l) ----> H3O+(aq) + OH-(aq)

which is often written as H2O(l) ---> H+(aq) + OH-(aq) and has a value of ∆G° = 79.9 kJ/mol at 25.0°C.

Calculate the value of ∆G for this system under the following conditions at 25°C and 1 atm.

[OH-] = 5.0×10-2M
[H+] = 7.1×10-2M

(Enter your answer to three significant figures.)

∆G = _______________J

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Patrina Schowalter
Patrina SchowalterLv2
3 May 2019

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Pls Pls only answer if you are going to answer all of them and not just one or two thanks i got alot in my hands cuz of finals, and don't have time to do them, Appreciate it, trust that they'll be right , I posted this once but they only did one instead of all six so yeah thanks

1) The electrochemical cell described by the balanced chemical equation has a standard emf of 0.35 V. Calculate the value (J) for the Wmax that the cell can do under standard conditions. Round your answer to 3 significant figures.

2MnO42-(aq) + 2Hg2+(aq) → 2MnO4-(aq) + Hg22+(aq)

St. Red. Pot. (V)
MnO4-/MnO42- +0.56
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F = 96485 C

2) The voltaic cell described by the balanced chemical reaction has a standard emf of 4.05 V. Calculate the equilibrium constant (Kc) for the reaction at 25 oC. Round your answer to 3 significant figures. F2(g) + Mn(s) → 2F-(aq) + Mn2+(aq)

St. Red. Pot. (V)
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Pt(s) l VO2+(aq), VO2+(aq), H+(aq) ll H+(aq), MnO4-(aq) l MnO2(s) l Pt(s)

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VO2+/VO2+ +1.00
MnO4-/MnO2 +1.68
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4) The galvanic cell described by the cell notation has an Eo of 1.23 V. Calculate the value (kJ) for the ΔG˚ of the cell. Round your answer to 3 significant figures.

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a -1310 b. +1180 c. -691 d. +1310 e. -1180

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b. Al(OH)3 (aq)+3H+ ---> Al3+(aq)+3H2O(l)

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d. C6H12O6(s)+6O2(g) ---> 6CO2+6H2O(l)

e. CO­2(g)+H2(g) ---> CO(g)+ H2O(g)­­­­­­­­

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