se the cell voltage method described in Worked examples 6 and 7 above to answer question 21, parts a to d.

Data From Question 21:

Use the data in Appendix 2 (page 474) to predict whether or not the following reactions are feasible. If a reaction does occur, write a balanced equation for it.

a Can MnO₄ ^– ions oxidise Cl^– ions to Cl₂ in acidic conditions?
b Can MnO₄^– ions oxidise F^– ions to F₂ in acidic conditions?
 c Can H⁺ ions oxidise V²⁺ ions to V³⁺ ions?
 d Can H⁺ ions oxidise Fe²⁺ ions to Fe³⁺ ions?

Data From Appendix 2:

Transcribed Image Text:

6 Will bromine oxldise silver to silver lons? Step 1 Write the equation for the suggested reaction. Br, + Ag → Br + Ag Step 2 Write the two half-equations: Br, + e= Br Ag 一Ag +e Step 3 Include the value of E* for each half-reaction but reverse the sign of the half-equation showing oxidation (loss of electrons). This Is because the data book values are always for the reduction reaction. Br, + e- Br E = +1.07V Ag Ag* +e E° =-0.80V Step 4 Add the two voltages. This Is because we are combining the two half-equations. =+1.07 + (-0.80) = +0.27V Step 5 lf the value of the sum of the two voltages Is positive the reaction will occur as written. If the value of the sum of the two voltages is negative the reaction will not occur. Inthis case the sum of the two voltages is positive so bromine will oxidise slver to slver lons. 7 Will lodine oxidise silver to silver lons? Step1 Write the equation for the suggested reaction. 弘+ Ag→I+Ag Step 2 The two half-equations are: + e Ag- Ag +e Step 3 Write the E values, with the sign reversed for the oxidation reaction. E = +0.54V Ag- Ag* +e E =-0.80V Step 4 Add the two voltages. = +0.54 + (-0.80) =-0.26V Step 5 The sum of the two voltages Is negative, so lodine will not oxidise silver to silver lons.