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2 years ago

In a combination reaction, 2.22 g of magnesium is heated with 3.75 g of nitrogen.

Chemistry

1 answer:

mariarad [96]2 years ago

8 0

Nitrogen is present in excess.

<h3>What is the no. of moles of nitrogen?</h3>

3Mg + N2 = Mg3N2

Moles of Mg = mass / molar mass = 2.22 / 24.3 = 0.0914

Moles of N2 = 3.75 / 28=0.1339

In conclusion, as we produce less amount of M g3N 2 when we assumed that M g was the limiting reagent, magnesium is the limiting reagent and nitrogen is the excess.

<h3>How can magnesium nitride be made through a direct reaction?</h3>

The elements can directly react to form magnesium nitride, as demonstrated in the equation 3 mg (s)+n2 (g)=Mg3N2 (s).

<h3>What is excess reactant?</h3>

Reactants that are not totally consumed are referred to as "excess reactants," whereas reactants that are completely consumed or reacted are referred to as "limited reactants." How much of the limiting reactants are consumed determines how much product is generated. In this section, the definition of excess reactant, examples, and calculations are discussed.

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Determine the concentrations of mgcl2, mg2 , and cl– in a solution prepared by dissolving 2.75 × 10–4 g mgcl2 in 1.75 l of water

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Answer:

M of MgCl₂ = 1.65 × 10⁻⁶ M

M of Mg²⁺ = 1.65 × 10⁻⁶ M

M of Cl⁻ = 3.30 × 10⁻⁶ M

Explanation:

1) MgCl₂

Molarity = number of moles of solute / volume of solution in liters, M = n / V

n = mass in grams / molar mass

molar mass of MgCl₂ = 24.305 g/mol + 2(35.543 g/mol) = 95.211 g/mol

n = 2.75 × 10⁻⁴ g / 95.211 g/mol = 2.89×10⁻³ moles

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2) Mg²⁺ and Cl⁻

Those are the ions in solution.

You assume 100% dissociation of the ionic compound (strong electrolyte).

Then the equation is: MgCl₂ → Mg²⁺ + 2Cl⁻

That means that 1 mol of MgCl₂ produces 1 mol of Mg²⁺ and 2 moles of Cl⁻.

That yields the same molarity concentration of Mg²⁺ , while the molarity concentration of Cl⁻ is the double.

So, the results are:

M of MgCl₂ = 1.65 × 10⁻⁶ M

M of Mg²⁺ = 1.65 × 10⁻⁶ M

M of Cl⁻ = 3.30 × 10⁻⁶ M

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