Ask a New Question

YEs, it is the correct balanced equation

bobpursley

A 2.80 mol/L solution of iron (II) dichromate is combined with 5.00L of a
2.25 mol/L acidic solution of tin (II) bromide. Calculate the volume of iron (II) dichromate required.

FeCr2O7 + SnBr2 --> SnCr2O7 + FeBr2

Is this the right formula? or no?

Ask a New Question or answer this question.

Similar Questions

7) A 3.33 g sample of iron ore is transformed into a solution of iron (II) sulfate. And this solution is titrated with 0.0150 M
1. 0 answers
A 2.80 mol/L solution of iron (II) dichromate is combined with 5.00L of a2.25 mol/L acidic solution of tin (II) bromide.
1. 0 answers
A 2.80 mol/L solution of iron (II) dichromate is combined with 5.00L of a2.25 mol/L acidic solution of tin (II) bromide.
1. 1 answer
overall balanced reaction:14H+ + C2O7^2- + 6Fe^2+ -> 2Cr^3+ + 7H2O + 6Fe^3+ .5021g of impure sample containing potassium
1. 1 answer

more similar questions