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1. Chemistry

   A cell is set up with copper and lead electrodes in contact with CuSO4(aq) and Pb(NO3)2(aq), respectively, at 25˚C. The standard reduction potentials are: Pb2+ + 2e- --> Pb E˚=-0.13 V Cu2+ + 2e- --> Cu E˚=+.34 V If sulfuric

2. Chemistry

   A cell is set up with copper and lead electrodes in contact with CuSO4(aq) and Pb(NO3)2(aq), respectively, at 25˚C. The standard reduction potentials are: Pb2+ + 2e- --> Pb E˚=-0.13 V Cu2+ + 2e- --> Cu E˚=+.34 V If sulfuric

3. AP Chemistry

   Sodium can be extracted by heating naturally occurring salt until it is molten. An electrochemical process is then used to extract the sodium. Cl2 is produced at the anode, and Na is collected at the cathode. 1. Write the

4. Chemistry

   Using the standard reduction potentials, calculate the equilibrium constant for each of the following reactions at 298 K. 10Br- + 2MnO4- + 16H+ -> 2Mn2+ + 8H20 + 5Br2 Work: 2Br- -> Br2 + 2e- (This would be multiplied by 5 to

1. Chemistry

   So we're doing oxidation-reduction reactions and batteries and voltages. We did a lab where we would take two metals, put it in a mixture (bleach/water/vinegar/salt) and used a voltmeter to see the DC voltage. Now we're supposed

2. Chemistry

   Given the following half-reactions and associated standard reduction potentials: AuBr−4(aq)+3e−→Au(s)+4Br−(aq) E∘red=−0.858V Eu3+(aq)+e−→Eu2+(aq) E∘red=−0.43V IO−(aq)+H2O(l)+2e−→I−(aq)+2OH−(aq)

3. Chemistry

   A voltaic cell is based on the reduction of Ag^+(aq) to Ag(s) and the oxidation of Sn(s) to SN^2+(aq). Write half-reactions for the cell's anode and cathode, and write a balanced cell reaction.

4. Chemistry

   Calculate the cell potential for the following reaction as written at 59 ¡ãC, given that [Cr2+] = 0.763 M and [Sn2+] = 0.0170 M. Standard reduction potentials: Sn2+(aq) + 2e¨C ¡ú Sn(s) E=¨C0.14 Cr2+(aq) + 2e¨C ¡ú Cr(s)

1. Chemistry

   (Use the information in the table below. Show the half reactions and the potentials for each half reaction.) Determine whether the following redox reaction is spontaneous as written. 2Al(s) + 3Zn2+(aq) → 2Al3+(aq) + 3Zn(s)

2. chemistry- electrochemical cell

   What makes this an oxidation-reaction? 3Ag2S+2Al(s) -> Al2S3+6 Ag(s)? Write the half-reactions showing the oxidation and reduction reactions. Identify which is the oxidation reaction and which is the reduction reason. What is

3. Chemistry need help

   using standard potentials given in the appendices calculate the standard cell potentials and the equilibrium constants for the following reactions. Zn(s)+( Fe^2+(aq)) ---> (Zn^2+(aq))+ Fe(s) If anyone can show work, then I can do

4. Chemistry

   Constants The following values may be useful when solving this tutorial. Constant Value E∘Cu 0.337 V E∘Fe -0.440 V R 8.314 J⋅mol−1⋅K−1 F 96,485 C/mol T 298 K Part A In the activity, click on the E∘cell and Keq

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