C3H7OH is an alcohol, it reacts ( burns) with oxygen O2 to produce water and carbon dioxide.

C3H7OH is an alcohol, it reacts ( burns) with oxygen O2 to produce water and carbon dioxide. write a balance chemical reaction. Indicate how many miles of oxygen is used?

The Correct Answer and Explanation is:

Balanced Chemical Equation:

The combustion of C₃H₇OH (propanol) in oxygen produces CO₂ (carbon dioxide) and H₂O (water):C3H7OH+9/2O2→3CO2+4H2O\text{C}_3\text{H}_7\text{OH} + 9/2 \text{O}_2 \rightarrow 3 \text{CO}_2 + 4 \text{H}_2\text{O}C3​H7​OH+9/2O2​→3CO2​+4H2​O

To remove the fraction, multiply the entire equation by 2:2C3H7OH+9O2→6CO2+8H2O2 \text{C}_3\text{H}_7\text{OH} + 9 \text{O}_2 \rightarrow 6 \text{CO}_2 + 8 \text{H}_2\text{O}2C3​H7​OH+9O2​→6CO2​+8H2​O

Final Balanced Equation:

2C3H7OH+9O2→6CO2+8H2O\boxed{2 \text{C}_3\text{H}_7\text{OH} + 9 \text{O}_2 \rightarrow 6 \text{CO}_2 + 8 \text{H}_2\text{O}}2C3​H7​OH+9O2​→6CO2​+8H2​O​

Moles of Oxygen Used:

From the balanced equation, 9 moles of oxygen gas (O₂) are required to completely burn 2 moles of propanol (C₃H₇OH).

Explanation :

Propanol (C₃H₇OH) is a type of alcohol, and like all hydrocarbons and alcohols, it reacts with oxygen in a combustion reaction. Combustion is a chemical process that usually occurs when a substance reacts with oxygen and releases energy in the form of heat and light. In complete combustion, the products are always carbon dioxide and water.

To write a balanced chemical equation, start by writing the unbalanced reaction:C3H7OH+O2→CO2+H2O\text{C}_3\text{H}_7\text{OH} + \text{O}_2 \rightarrow \text{CO}_2 + \text{H}_2\text{O}C3​H7​OH+O2​→CO2​+H2​O

Then balance the carbon atoms. There are three carbon atoms in propanol, so you need three CO₂ molecules on the right.

Next, balance the hydrogen atoms. There are eight hydrogen atoms in two molecules of propanol (each has seven hydrogens plus one from the OH group), so you need four H₂O molecules.

Now count the oxygen atoms. On the right side, there are six oxygen atoms from CO₂ and four from H₂O, totaling ten oxygen atoms. On the left, each O₂ molecule has two atoms, so to get ten oxygen atoms, you need five O₂ molecules. Since the original equation had a fraction (9/2), we multiply the entire equation by 2 to eliminate fractions.

The final balanced reaction shows that 9 moles of oxygen gas are used for every 2 moles of propanol combusted. This type of stoichiometric ratio is crucial in chemistry when calculating the amount of reactants needed or the amount of products formed.