Question

Pure magnesium metal is often found as ribbons and can easily burn in the presence of oxygen. When 3.97 g of magnesium ribbon burns with 8.05 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.

Answer 1

Answer:

The balanced chemical equation is given as:

$2Mg(s)+O_2(g)\rightarrow 2MgO(s)$

Explanation:

When magnesium metal burns in presence of oxygen it gives white color powdered compound called magnesium oxide.

The balanced chemical equation is given as:

$2Mg(s)+O_2(g)\rightarrow 2MgO(s)$

According to reaction, 2 moles of magnesium metal when reacts with 1 mole of oxygen gas it gives 2 moles of  solid magnesium oxide.