[bamster]

This is for a PreLab


Question is, Calculate the volume of the 1 mol/L copper(II) sulfate(CuSO4) solution required to react with 1.00g of iron fillings.Use the equation that will give you the most copper(II) sulfate.Add an addittional 10% to your calculated volume in order to have sufficient copper (II) sulfate to ensure an excess.

Use this equation

2Fe + 3Cu²⁺   2Fe³⁺ + 3Cu

[Borek]

What do you find difficult? This is pretty simple stoichiometry. How many moles of iron do you have? How many moles of copper sulfate needed?

Note: Fe²⁺ is most likely product here.

[bamster]

but how do you do the question

[Borek]

How many moles of iron do you have?

Look at the reaction equation. How many moles of copper do react with this number of moles of iron?

What volume of the solution contains this number of moles of copper sulfate?

Add 10%.

[bamster]

can someone show how to write the calculations?

[sjb]

For each cake I need to bake I need 3 eggs. How many eggs will I need for 23 cakes, add 10% to take care of spillage, accidental breakage in transit from the shop etc?

May not seem like relevant, but at least at the start it's basic stoichiometry again.

S

[AWK]

2Fe + 3Cu2+  2Fe3+ + 3Cu

should be

Fe + Cu²⁺ = Fe²⁺ + Cu