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In a combination reaction, 2.22 g of magnesium is heated with 3.75 g of nitrogen.
(c) After reaction, how many grams of each reactant and product are present?

Respuesta :

2.9g N2, 0g Mg, 3.07g Mg3N2 are present.

Equation

3Mg+N2-->Mg3N2

moles of N2 needed= (0.0913mol Mg)(1molN2/ 3molMg)

= 0.0304mol N2

moles of N2 excess=moles of N2 - moles of N2 needed

=0.1388mol N2- )0.0304 mol N2

=0.1034 mol N2

mass of N2= (0.1034 mol N2)(28.02g N2/ 1molN2)

mass of N2 =2.9g N2

moles of Mg= 0mol

mass of Mg  = (0mol)(24.31g Mg/ 1mol Mg)

mass of Mg = 0g

mass of Mg3N2 = (0.0304mol Mg3N2)(100.95g Mg3N2/ 1molMg3N2)

mass of Mg3N2= 3.07g Mg3N2

Why is this reaction called a combination?

A combination reaction is a chemical process in which two or more elements or molecules combine to form new compounds.

What is a combination reaction example?

Ba (s) + F2 (g) --> BaF2 is an illustration of a pair of elements reacting with each other (s)

learn more about combination reaction here

https://brainly.com/question/12842366

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