Questions: Methanol (CH4O) is used as a fuel in race cars. Gaseous methanol burns in oxygen (O2) to form carbon dioxide, CO2, and water vapor, H2O. Write a balanced equation for this equilibrium. Include all physical states of matter.

Methanol (CH4O) is used as a fuel in race cars. Gaseous methanol burns in oxygen (O2) to form carbon dioxide, CO2, and water vapor, H2O.

Write a balanced equation for this equilibrium. Include all physical states of matter.

Transcript text: Methanol $\left(\mathrm{CH}_{4} \mathrm{O}\right)$ is used as a fuel in race cars. Gaseous methanol burns in oxygen $\left(\mathrm{O}_{2}\right)$ to form carbon dioxide, $\mathrm{CO}_{2}$, and water vapor, $\mathrm{H}_{2} \mathrm{O}$. Part: $0 / 6$ Part 1 of 6 Write a balanced equation for this equilibrium. Include all physical states of matter.

Solution

Solution Steps

Step 1: Write the Unbalanced Chemical Equation

First, we write the unbalanced chemical equation for the combustion of methanol. Methanol ($\mathrm{CH}_4\mathrm{O}$) reacts with oxygen ($\mathrm{O}_2$) to form carbon dioxide ($\mathrm{CO}_2$) and water vapor ($\mathrm{H}_2\mathrm{O}$).

\[ \mathrm{CH}_4\mathrm{O} + \mathrm{O}_2 \rightarrow \mathrm{CO}_2 + \mathrm{H}_2\mathrm{O} \]

Step 2: Identify the Physical States of Reactants and Products

Next, we identify the physical states of each substance involved in the reaction. Methanol is a liquid ($\ell$), oxygen is a gas ($g$), carbon dioxide is a gas ($g$), and water vapor is a gas ($g$).

\[ \mathrm{CH}_4\mathrm{O}(\ell) + \mathrm{O}_2(g) \rightarrow \mathrm{CO}_2(g) + \mathrm{H}_2\mathrm{O}(g) \]

Step 3: Balance the Chemical Equation

Now, we balance the chemical equation by ensuring that the number of atoms of each element is the same on both sides of the equation.

Carbon (C): There is 1 carbon atom on both sides.
Hydrogen (H): There are 4 hydrogen atoms in methanol and 2 in water vapor. We need 2 water molecules to balance hydrogen.
Oxygen (O): There are 2 oxygen atoms in methanol and 2 in each water molecule, totaling 4 oxygen atoms on the product side. We need 3 oxygen molecules to balance oxygen.

The balanced equation is:

\[ 2\mathrm{CH}_4\mathrm{O}(\ell) + 3\mathrm{O}_2(g) \rightarrow 2\mathrm{CO}_2(g) + 4\mathrm{H}_2\mathrm{O}(g) \]