Lilac12

Thank you so much that was really helpful, I think I've gotten to the final answer now!

Thank you for replying! I think that I already have the empirical formula for dichromate but all I've got so far is this: K2CrO7 + Fe(NO3)2 I tried to search up what acidified dichromate means but I couldn't find anything, does it just mean I add H+ And then I have no clue how to know which part of it will go through reduction and which will go through oxidisation. For example, a previous question in the booklet asked the same question, except it had the balanced equation given to me of: 5Fe{2+} + MnO4{-} + 8H{+} --> 5Fe{3+} + Mn{2+} + 4H2O So I knew that the oxidation was where electrons were lost, which was: 5Fe{2+} --> 5Fe{3+} + 5e and the reduction was where electrons were gained, which was: MnO4{-} + 8H{+} + 5e --> Mn{2+} + 4H2O So if I knew the whole equation I would know how to write out each half equation, so really my question is how do I do my question I posted without knowing the equation and if there is a way I'm meant to get or know the equation?

This question isn't for homework but it was in a booklet we were given to help us revise, except we weren't given an answer booklet or worked solutions along with it. I don't even understand how to write out each side of the equation, let along do the oxidation and reduction reactions. The question is below: "Write half-equations and hence a balance overall ionic equation for the reaction of acidified potassium dichromate solution and a solution of iron (ll) nitrate. (Note the potassium and nitrate ions are spectator ions)." I'd really appreciate and explanation of how to get to the final answer!