A 2.241 g sample of nickel reacts with oxygen to form 2.852 g of the metal oxide. Calculate the empirical formula of the oxide.

Question

Give the number of moles of each element to support you answer.

Answer 1

YOU can figure the moles of oxygen, and Ni.

molesNi= 2.241/atomicweightNi

molesO=(2.852-2.241)/15.999

now, get the mole ratio: MolesNi/molesO

(ie, divide both moles by the lowest number).

The formula will be Ni_nO<sub>m</sub)

where n/m= mole ratio above. If it is a weird number, such as .33, get it to
.33/1=n/m multiply by 3, so that n/m =1/3 In this case it should be weird.</sub>

Answer 2

It shouldn't be weird, it should be a simple whole number.

Answer 3

so

O=.0382
Ni=.0382 also?

Answer 4

Doesn't that look like 1:1. It does to me.