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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. Calculate the empirical formula of the oxide?

Chemistry

1 answer:

astraxan [27]3 years ago

7 0

Answer:

NiO

Explanation:

Firstly, we need to know the mass of oxygen used up. This is the difference between the mass of the nickel and the mass of the oxide. This is : 2.852 - 2.241 = 0.611g

Now we convert these masses to mole by dividing by their atomic masses. The atomic mass of oxygen is 16 while that of nickel is 59

O = 0.611/16 = 0.0381875

Ni = 2.241/59 = 0.037983050847458

The next thing is to divide each by the smaller number of moles, which is that of the nickel.

O = 0381875 /0.037983050847458= 1

Ni= 0.037983050847458/0.037983050847458= 1

The empirical formula is thus NiO

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ruslelena [56]

Answer:

<h2>117.94 moles</h2>

Explanation:

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2 years ago

What is the relationship between concentration and rate of reaction?

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3 years ago

A certain compound was found to have the molecular formula C5H12O2. To which of the following compound classes could the compoun

IgorC [24]

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Explanation :

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First we have to calculate the degree of unsaturation.

Formula used:

Degree of unsaturation = $\frac{2C+2+N-X-H}{2}$

where,

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H = number of hydrogen

N = number of nitrogen

X = number of halogen

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3 years ago

Convert 100mL to L. Show your work to receive full credit.

Ilya [14]

Answer:

100 ml = 0.1 L

I divided 100 by 1000 because 1000ml = 1L

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