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valentinak56 [21]
3 years ago
7

What is the mass of 2.3 x 1021 formula units of cobalt(II) bromate?

Chemistry
1 answer:
MissTica3 years ago
6 0

Molecular mass of Cobalt(II) Bromide  = 218.7412 g/mol .

<u>Explanation:</u>

<u>Percent composition by element: </u>

The procedure to find the Molecular mass of Cobalt(II) Bromide:

The symbol of the Cobalt is Co.

The symbol of the Bromate is Br.

The Element cobalt have the Atomic Mass of 58.933200 with 1 number of atom.

The Element Bromine have the Atomic Mass of 79.904 with 2 number of atoms.

<u>Molecular weight calculation: </u>

To find the molecular mass we have to sum both of the Atomic masses:

For Cobalt(II) Bromide: We have to multiple the Atomic mass of  bromate with 2 and then sum the atomic masses  

58.9332+79.904 \times 2 =218.7412g/mol

Molecular mass of Cobalt(II) Bromide  = 218.7412 g/mol

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a student adds 3.5 moles of solute to enough water to make a 1500mL solution. what is the concentration?
aksik [14]
<h2>Hello!</h2>

The answer is:

MolarConcentration=\frac{3.5moles}{volume(1.5L)}=2.33molar

<h2>Why?</h2>

Since there is not information about the solute but only its mass, we need to assume that we are calculating the molar concentration of a solution or molarity. So, need to use the following formula:

MolarConcentration=\frac{mass(solute)}{volume(solution)}

Now, we know that the mass of the solute is equal  3.5 moles and the volume is equal to 1500 mL or 1.5L

Then, substituting into the equation, we have:

MolarConcentration=\frac{3.5moles}{1.5L}=2.33molar

Have a nice day!

7 0
3 years ago
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Answer:

Ca, Zn, Ni, Al, Fe

Explanation:

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Metals that are high up in the activity series are very reactive. They displace metals that are lower in the activity series from an aqueous solution of their salts.

The metals; Ca, Zn, Ni, Al, Fe are all above Pb in the activity series hence they will cause Pb2+ ions to come out of solution as solid Pb.

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Answer:

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