Dariana Using the Nernst equation to calculate nonstandard cell voltage A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: Sn" (aq) + Ba (s)→ Sn (s) + Ba-™ (aq) 2+ Suppose the cell is prepared with 2.40 M Sn in one half-cell and 0.623 M Ba' 2+ in the other. Calculate the cell voltage under these conditions. Round your answer to 3 significant digits. alo

|| Using the Nernst equation to calculate nonstandard cell voltage A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 0 2+ 2+ Cu (aq) + Zn (s) → Cu (s) + Zn²+ (aq) 2+ 2+ Suppose the cell is prepared with 1.39 M Cu in one half-cell and 2.14 M Zn in the other. Calculate the cell voltage under these conditions. Round your answer to 3 significant digits. 0 x10 ロ・ロ X μ

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the Nernst equation to calculate nonstandard cell voltage A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2+ 2+ Sn²+ (aq) + Ba(s) → Sn (s) + Ba²+ (aq) 2+ 2+ in one half-cell and 3.14 M Ba Suppose the cell is prepared with 2.84 M Sn Calculate the cell voltage under these conditions. Round your answer to 3 significant digits. 0 ロ・ロ μ 00 09 Ś ? in the other.

Calculate the cell voltage under these conditions. Round your answer to 3 significant digits.

A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: Cu?* (aq)+Zn (s) → Cu (s) +Zn²* (aq) Suppose the cell is prepared with 3.40 M Cu´" in one half-cell and 5.47 M Zn2+ in the other. Calculate the cell voltage under these conditions. Round your answer to 3 significant digits. x10

A chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard reduction potential CrO2−4 (aq)+4H2O(l)+3e−→  CrOH3(s)+5OH−(aq) =E0red−0.13V Cl2(g)+2e−→  2Cl−(aq) =E0red+1.359V   Answer the following questions about this cell. Write a balanced equation for the half-reaction that happens at the cathode. Write a balanced equation for the half-reaction that happens at the anode.   Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is spontaneous as written. Do you have enough information to calculate the cell voltage under standard conditions? If you said it was possible to calculate the cell voltage, do so and enter your answer here. Be sure your answer has the correct number of significant digits. V

A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2+ Cu2+ (aq) + Zn (s) → Cu (s) + Zn²+ (aq) 2+ Suppose the cell is prepared with 3.51 M Cu²*+ in one half-cell and 1.20 M Zn²+ in the other. Calculate the cell voltage under these conditions. Round your answer to 3 significant digits. 日 ☐ x10 ☐ μ ロ・ロ

A certain metal M forms a soluble nitrate salt MNO33 . Suppose the left half cell of a galvanic cell apparatus is filled with a 5.00M solution of MNO33 and the right half cell with a 25.0mM solution of the same substance. Electrodes made of M are dipped into both solutions and a voltmeter is connected between them. The temperature of the apparatus is held constant at 35.0°C.   What voltage will the voltmeter show? Assume its positive lead is connected to the positive electrode.Be sure your answer has a unit symbol, if necessary, and round it to 2 significant digits.

A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: MnO₂ (s) + 4H* (aq) + 2Cr²+ (aq) → Mn²+ (aq) + 2H₂O (1) + 2Cr³+ (aq) 2+ 2+ 3+ Suppose the cell is prepared with 3.73 MH* and 1.42 M Cr²+ in one half-cell and 4.21 M Mn²+ and 3.05 M Cr³+ in the other. Calculate the cell voltage under these conditions. Round your answer to 3 significant digits. 1 x10 X μ 00 Ś