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1 year ago

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

Chemistry

1 answer:

mariarad [96]1 year 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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3 years ago

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Explanation:

<em>...the reaction is: Ag+ + SCN- => AgSCN(s) Calculate the percent As2O3 in the sample. (F.W. As2O3 = 197.84 g/mol).</em>

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From the mass and density we could calculate the volume of the solution as:

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Let's convert the volume from mL to L as molarity is moles of solute per liter of solution.

$111mL(\frac{1L}{1000mL})$

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