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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

<u>The empirical formula is = $NiO$ </u>

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Answer:

=16.49 L

Explanation:

Using the equation

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3 years ago

A 20.0 mL solution of NaOH is neutralized with 24.1 mL of 0.200 M HBr. What is the concentration of the original NaOH solution

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Answer:

0.241 M

Explanation:

We'll begin by writing the balanced equation for the reaction. This is given below:

HBr + NaOH —> NaBr + H₂O

From the balanced equation above,

The mole ratio of acid, HBr (nₐ) = 1

The mole ratio of base, NaOH (n₆) = 1

Finally, we shall determine the concentration of the NaOH solution. This can be obtained as follow:

Volume of base, NaOH (V₆) = 20 mL

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Concentration of acid, HBr (Cₐ) = 0.2 M

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Cross multiply

C₆ × 20 = 4.82

Divide both side by 20

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Answer:

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Explanation:

Ionic compounds are compound formed from the transfer of electron(s). One atom of the element loses electron(s) while the other atom gains electron(s).

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The chlorine atom on the other hand has 7 valency electrons, to attain octet configuration it will most likely gain 1 electron to become stable.

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