Editing AP Review Set 1
ApchemWiki
|
RecentChanges
|
Preferences
<center><b>AP Review Set #1 (Electrochemistry)</b></center> <br> <b>Problem #1</b>(ninety seven)<br> In an electrolytic cell, a current of 0.250 ampere is passed through a solution of a chloride of iron, producing solid Fe and chloride gas (Cl<sub>2</sub>).<br> a. Write the equation for the half-reaction that occurs at the anode.<br> b. When the cell operates for 2.00 hours, 0.521 grams of iron is deposited at one electrode. Determine the formula of the chloride of iron in the original solution.<br> c. Write the balanced equation for the overall reaction that occurs in the cell.<br> d. How many liters of chlorine gas, measured at 25 degreeC and 750mmHg, are produced when the cell operates as described in part B?<br> e. Calculate the current that would produce chlorine gas from the solution at a rate of 3.00 grams per hour.<br> <br> <br> <b>Problem #2</b><br> <br> A galvanic cell (electrochemical cell) is made from zinc and iron (from Fe<sup>2+</sup> to Fe<sup>0</sup> or visa versa).<br> a. Determine the overall chemical reaction and E<sub>cell</sub><sup>0</sup><br> b. Sketch the cell including direction of flow of electrons, anode (half-cell rxn, material of anode,and solution at anode), cathode(same as anode).<br> c. Calculate deltaG<sup>0</sup> and K for this reaction at 25 degreeC.<br> d. Calculate E<sub>cell</sub> at 25degreeC when [Zn<sup>2+</sup>]= 0.10M and [Fe<sup>2+</sup>] = 1.0E-5M.<br>
View other revisions
ApchemWiki
|
RecentChanges
|
Preferences