Hey Chemistry folks
Can someone help me out with the following Q
1) write the half equation(partial ionic equation) for the oxidation of chlorine gas (Cl2) to Hypochlorous acid (HOCL)
2) the oxidant and the reactant of : 2KMnO4(aq) + 5H2S(aq) + 6HCL(aq) -----> 2MnCl2(aq) + 5S(s) + 2KCl(aq) + 8H2O(l)
3) write balanced equations for the following redox reactions: Under certain conditions, zinc can react with concentrated nitric acid (HNO3) to form the zinc ion (Zn^2+) the ammonium ion (NH4^+) and water.
Any solutions to the Q, will be much appreciated!
1. 2H2O(l) + Cl2(g) --> 2HOCl(aq) + 2H+(aq) + 2e-
2. oxidant and
reductant? The oxidant gets reduced, and oxidises something else by taking electrons: [KMnO4] (+7 to +2) (Mn)
Reductant will give away electrons to reduce something and is oxidised: [H2S/S2-] (-2 to 0) (S) I've separated S2- from H2S as it's in the aqueous state..
3. (Zn(s) --> Zn2+(aq) + 2e-)*4
8e- + 9H+(aq) + HNO3(aq) --> NH4+(aq) +3H2O(l)
4Zn(s) + 9H+(aq) + HNO3(aq) --> 4Zn2+(aq) + NH4+(aq) + 3H2O(l)