REDOXEQU basic 1 - Contents
- Page 1Half equations 1 - ReviewPrinciples of balancing redox equations using half equations
- 16 marksPage 2Example 1If copper metal is immersed in aqueous AgNO3, silver is precipitated, and the solution turns blue due to formation of Cu2+.
- 17 marksPage 3Example 2An aqueous solution of bromine is decolorised when it is added dropwise to aqueous iron(II) sulfate (FeSO4).
- Page 4Half equations 2 - ReviewIntroduction to principles required to balance redox equations using polyatomic oxidants or reductants in acidic solution
- 17 marksPage 5Example 3The dichromate ion (Cr2O72–) reacts with SO2 in acidic aqueous solution to give SO42– and Cr3+.
- 25 marksPage 6Example 4Copper reacts with concentrated nitric acid (HNO3) reacts to give Cu2+ and NO2 gas.
- 23 marksPage 7Example 5The permanganate ion (MnO4–) reacts with Fe2+ in acidic aqueous solution to give Fe3+ and Mn2+.