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Brrunno [24]
3 years ago
6

When magnesium combines with sulfur to form magnesium sulfide, it is oxidized to Mg2+. Which statement is true about this reacti

on?
A. 

It involves gain of electrons.

B. 

It involves loss of electrons.

C. 

It involves loss of oxygen.

D. 

It involves gain of hydrogen.

​
Chemistry
1 answer:
Vlad1618 [11]3 years ago
6 0
<h3><u>Answer;</u></h3>

B. It involves loss of electrons.

<h3><u>Explanation;</u></h3>
  • Oxidation occurs when electrons are lost by an atom while reduction refers to the gain of electrons by an atom.
  • <u><em>In this case, magnesium atom reacts with sulfur to form magnesium sulfide by loosing two electrons and forming magnesium ion (Mg2+). Therefore magnesium undergoes oxidation.</em></u>
  • Sulfur, on the other hand will gain electrons to form Sulfide ions, therefore it undergoes reduction.
  • Therefore;<em><u> In magnesium sulfide (MgS), magnesium loses two electrons and becomes a cation with a positive-two charge. Likewise, sulfur obtains the two electrons lost from magnesium and becomes an anion with a negative-two charge. However, the overall charge of MgS is zero.</u></em>
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Answer:

<em><u>The molarity of the CoBr2•4H2O solution is  7.64 × 10-2 M</u></em>

Explanation:

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We then need to determine the number of moles of CoBr2•4H2O since this is the only information missing for us to find molarity. Notice that the volume of the solution is already given.

We’re given the mass of CoBr2•4H2O. We can use the molar mass of CoBr2•4H2O4 to find the moles.

•The molar mass of CoBr2•4H2O is:

CoBr2•4H2O  

1 Co x 58.93 g/mol Co = 58.93 g/mol

2 Br x 79.90 g/mol Br = 159.80 g/mol

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________________________________________

                           Sum = <u>290.79 g/ mo</u>

The moles of CoBr2•4H2O is:

= 10.0 g CoBr2•4H2O x  \frac{ 1 mol  CoBr_2 . 4H_2O}{290.79 g CoBr_2 .  4H_2O}

= <u>0.0344  mol CoBr2•4H</u>

We know that the volume of the solution is 450 mL.

We can now calculate for molarity:

Convert mL to L → 1 mL = 10-3 L

Formula:

Molarity (M)= Mole of solute / Liters of solution

= 0.0344  mol CoBr2•4H  / 450 mL x 1 ml / 10^ -3 L

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