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3 years ago

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

Chemistry

1 answer:

nlexa [21]3 years ago

4 0

Answer:

The empirical formula is = $NiO$

Explanation:

Given that:- Mass of nickel = 2.241 g

Mass of the oxide formed = 2.852 g

Mass of the oxygen reacted = Mass of the oxide formed - Mass of nickel = 2.852 g - 2.241 g = 0.611 g

Molar mass of nickel = 58.6934 g/mol

Moles of nickel = $\frac{2.241}{58.6934}\ mol$ = 0.03818 mol

Molar mass of oxygen = 15.999 g/mol

Moles of nickel = $\frac{0.611}{15.999}\ mol$ = 0.03818 mol

Taking the simplest ratio for Ni and O as:

0.03818 : 0.03818 = 1 : 1

The empirical formula is = $NiO$

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Hey there!

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user100 [1]

Let MM(x) be the molar mass of x.

MM(Pb) : MM(PbO)
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cross multiply and solve for x
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kondor19780726 [428]

Answer:

Here's what I get

Explanation:

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