Question

Pure magnesium metal is often found as ribbons and can easily burn in the presence of oxygen. When 3.44 g of magnesium ribbon burns with 6.82 gof 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

`\rm \text{The balanced equation is is $\large \boxed{\text{2Mg + O$_(2) \longrightarrow \,$ 2MgO}}$}`

Step-by-step explanation:

Mg + O₂ ⟶ MgO

1. Balance O.

We have 2 atoms of O on the left and 1 O on the right.

Put a 1 in front of O₂ and a 2 in front of MgO.

Mg + 1O₂ ⟶ 2MgO

2. Balance Mg:

We have fixed 2 Mg on the right. We need 2 Mg on the 2 Mg on the left. Put a 2 in front of Mg.

2Mg + 1O₂ ⟶ 2MgO

Every formula now has a coefficient. The equation should be balanced.

3. Check that atoms balance:

`\begin{array}{ccc}\textbf{Atom} & \textbf{On the left} & \textbf{On the right}\\\text{Mg} & 2 &2\\\text{O} & 2 & 2\\\end{array}`

The equation is now balanced.

`\rm \text{The balanced equation is is $\large \boxed{\textbf{2Mg + O$_{\mathbf{2}} \longrightarrow \, $ 2MgO}}$}`