Pure magnesium metal is often found as ribbons and can easily burn in the presence of oxygen. when 2.59 g of magnesium ribbon burns with 7.52 g of oxygen, a bright, white light and a white, powdery product are formed. enter the balanced chemical equation for this reaction. be sure to include all physical states.

Question

Gianna Golden

Chemistry

29 November, 10:11

Pure magnesium metal is often found as ribbons and can easily burn in the presence of oxygen. when 2.59 g of magnesium ribbon burns with 7.52 g of oxygen, a bright, white light and a white, powdery product are formed. enter the balanced chemical equation for this reaction. be sure to include all physical states.

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Brie · Answer 1

Burning Mg in the air and reacting with O2 forming a white powder of MnO

So the equation is going to be:

Mn + O2 ⇒ MnO (this equation is not conserved)

to make it equilibrium:

1 - First we should put 2Mno to equal the O2 on both sides.

So it will be:

Mg + O2⇒ 2MgO

2 - Second we should put 2Mn to equal the Mn on both sides.

2Mg + O2⇒ 2MgO (this equation is conserved)

After putting the physical states the final equilibrium equation is going to be:

Δ

2Mg (s) + O2 (g) ⇒ 2MgO (s)