Chemistry AS

Hey everyone ,
I was doing some chemistry questions and got stuck on this one:

Calculate the maximum mass of hydrated nickel(II) sulphate ,NiSO4.7H20 which could be formed from 2.95 g of nickel.

Could anyone help out ,if you could ,PLEASE do show the steps that you used! I am confused ,whether to convert into moles or not.

Reply 1

Georgiecat

Presuming you're making it from pure nickel:
mol = mass/Mr
So moles of nickel = 2.95/58.7 = 0.05025553662
Presumably Ni produces NiSO4.7H20 in a 1:1 ratio, so there must be 0.05025553662 moles of NiSO4.7H20 produced from 2.95g of Ni
Mr of NiSO4.7H20 = 280.8
mass = mol x Mr
mass = 0.05025553662 x 280.8
mass = 14.11175468g = 14.1g (3.s.f)