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UNO [17]
3 years ago
5

What mass of magnesium would combine with exactly 16.0 grams of oxygen

Chemistry
1 answer:
TEA [102]3 years ago
3 0
1.65g MgO = 1g Mg
1.65 - 1 = 0.65 g of O in MgO

solve it using proportion:
1g Mg / 0.65g O = x (g) Mg / 16g O
or 1 / 0.65 = x / 16

24.6 g is the answer.

if 1 gram of oxygen requires 1.65 grams of Mg
then 16 grams of oxygen will require 16 ( 1.65) or 26.4 grams.
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Carbon-14 is an isotope used in carbon dating. The nucleus becomes Nitrogen-14 through beta decay. Its half-life is 5370 years.
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Answer:

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8 0
3 years ago
2. Consider the following reaction: 4 FeS2 + 11O2 → 2 Fe2O3 + 8 SO2
belka [17]
<h3>Answer:</h3>

Oxygen gas (O₂) is the rate limiting reactant and FeS₂ is the excess reactant.

<h3>Explanation:</h3>

From the questions we are given;

4FeS₂(s) + 11O₂(g) → 2Fe₂O₃(s) + 8SO₂(s)

  • Moles of FeS₂ are 26.62 moles
  • Moles of Oxygen, O₂ are 59.44 moles

We are supposed to determine the limiting and excess reactants;

  • From the equation of the reaction given; 4 moles of FeS₂ required 11 moles of Oxygen gas.

Working with the amount of reactants given;

  • 26.62 moles of FeS₂ will require 73.205 moles of O₂ and only 59.44 moles of O₂ are available.
  • On the other hand 59.44 moles of O₂ requires 21.615 moles of  FeS₂, and we are given 26.62 moles of FeS₂ which means FeS₂ is in excess.

Conclusion;

We can conclude that Oxygen gas (O₂) is the rate limiting reactant and FeS₂ is the excess reactant.

6 0
3 years ago
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Orlov [11]
Equation is as follow,

<span>                     2 AgNO</span>₃<span>  +  MgBr</span>₂<span>    </span>→    <span>2 AgBr  +  Mg(NO</span>₃<span>)</span>₂

According to eq.

    339.74 g (2 moles) AgNO₃ produces  =  375.54 g (2 moles) of AgBr
So,
                    22.5 g AgNO₃ will produce  =  X g of AgBr

Solving for X,
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                             X  =  24.87 g of AgBr
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The volume of a given quantity of a gas must increase if:
professor190 [17]
<span>D the temperature decreases and the pressure increases</span>
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