Question

disposable lighters contain liquid butane (c4h10) that is vaporized and then burned to produce co2 and h2o. Balance the chemical equation for this combustion reaction.

Answer 1

The balanced chemical equation of combustion reaction is as follows:

$\boxed{{\mathbf{2}}{{\mathbf{C}}_{\mathbf{4}}}{{\mathbf{H}}_{{\mathbf{10}}}}\left(g\right)+{\mathbf{13}}{{\mathbf{O}}_{\mathbf{2}}}\left(g\right)\to{\mathbf{8C}}{{\mathbf{O}}_{\mathbf{2}}}\left(g\right)+{\mathbf{10}}{{\mathbf{H}}_{\mathbf{2}}}{\mathbf{O}}\left(g\right)}$

Further Explanation:

The chemical reaction that contains equal number of atoms of the different elements in the reactant as well as in the product side is known as balanced chemical reaction. The chemical equation is required to be balanced to follow the Law of the conservation of mass.

Combustion reaction is the reaction in which the reactant reacts with molecular oxygen to form carbon dioxide and water molecule. Molecular oxygen acts as the oxidizing agent in these reactions. The large amount of heat is released and therefore combustion reactions are exothermic reaction.

The steps to balance a chemical reaction are as follows:

Step 1: Complete the reaction and write the unbalanced symbol equation.

In the combustion reaction, ${{\text{C}}_4}{{\text{H}}_{10}}$ reacts with ${{\text{O}}_2}$ to form ${\text{C}}{{\text{O}}_{\text{2}}}$ and ${{\text{H}}_{\text{2}}}{\text{O}}$. The physical state of ${{\text{C}}_{\text{4}}}{{\text{H}}_{{\text{10}}}}$ is gas, ${{\text{O}}_2}$ is gas, ${\text{C}}{{\text{O}}_{\text{2}}}$ is gas and ${{\text{H}}_{\text{2}}}{\text{O}}$ is gas. The unbalanced chemical equation is as follows:

 ${{\text{C}}_{\text{4}}}{{\text{H}}_{{\text{10}}}}\left(g\right)+{{\text{O}}_2}\left(g\right)\to{\text{C}}{{\text{O}}_{\text{2}}}\left(g\right)+{{\text{H}}_{\text{2}}}{\text{O}}\left(g\right)$

Step 2: Then we write the number of atoms of all the different elements that are present in a chemical reaction in the reactant side and product side separately.  

• On reactant side,

Number of carbon atoms is 4.

Number of hydrogen atoms is 10.

Number of oxygen atoms is 2.

• On product side,

Number of carbon atoms is 1.

Number of hydrogen atoms is 2.

Number of oxygen atoms is 3.

Step 3: Initially, we try to balance the number of other atoms of elements except for carbon, oxygen, and hydrogen by multiplying with some number on any side but in the combustion reaction there is only carbon, hydrogen, and oxygen atom.

Step 4: After this, we balance the number of atoms of carbon and then hydrogen atom followed by oxygen atoms. To balance the number of atoms of carbon we have to multiply   by 4 to make 4 carbon atoms on both sides of the reaction. This gives,

 ${{\text{C}}_{\text{4}}}{{\text{H}}_{{\text{10}}}}\left(g\right)+{{\text{O}}_2}\left(g\right)\to4{\text{C}}{{\text{O}}_{\text{2}}}\left(g\right)+{{\text{H}}_{\text{2}}}{\text{O}}\left(g\right)$

The number of carbon, hydrogen and oxygen atoms on the reactant side is 4, 10 and 2 respectively. The number of carbon, hydrogen and oxygen atoms on the product side is 4, 2 and 9 respectively.

Step 5: After this,we have to balance the hydrogen atom by multiplying   by 4 to make 10 hydrogen atoms on both sides of the reaction. This gives,

 ${{\text{C}}_{\text{4}}}{{\text{H}}_{{\text{10}}}}\left(g\right)+{{\text{O}}_2}\left(g\right)\to 4{\text{C}}{{\text{O}}_{\text{2}}}\left(g\right)+5{{\text{H}}_{\text{2}}}{\text{O}}\left( g\right)$

The number of carbon, hydrogen and oxygen atoms on the reactant side is 4, 10 and 2 respectively. The number of carbon, hydrogen and oxygen atoms on the product side is 4, 10 and 13 respectively.

Step 6: After this,we have to balance the oxygen atom by multiplying   by   to make 13 oxygen on both side of the reaction. This gives,

 ${{\text{C}}_{\text{4}}}{{\text{H}}_{{\text{10}}}}\left(g\right)+\frac{{13}}{2}{{\text{O}}_2}\left(g\right)\to4{\text{C}}{{\text{O}}_{\text{2}}}\left(g\right)+5{{\text{H}}_{\text{2}}}{\text{O}}\left(g\right)$

The number of carbon, hydrogen and oxygen atoms on the reactant side is 4, 10 and 13 respectively. The number of carbon, hydrogen and oxygen atoms on the product side is 4, 10 and 13 respectively.

Step 7: Since the balanced reaction must contain coefficients as a whole number. To make all the coefficients whole number we have to multiply whole equation by 2. This gives the balanced chemical equation as follows:

 ${\text{2}}{{\text{C}}_{\text{4}}}{{\text{H}}_{{\text{10}}}}\left(g\right)+13{{\text{O}}_2}\left(g\right)\to 8{\text{C}}{{\text{O}}_{\text{2}}}\left(g\right)+10{{\text{H}}_{\text{2}}}{\text{O}}\left(g\right)$

Learn more:

1. Balanced chemical equation: brainly.com/question/1405182

2. Identification of all of the phases of the reaction: brainly.com/question/8926688

Answer details:  

Grade: High School

Subject: Chemistry

Chapter: Chemical reaction and equation

Keywords: Balancing, C4H10, O2, CO2, H2O, 2C4H10, 13O2, 8CO2, 10H2O, phases, physical state, solid, liquid, gas, aqueous, coefficients, and combustion reactions.

Answer 2

Butane ($C_4H_{10}$) is a hydrocarbon used in disposable lighters. It undergoes a combustion reaction to produce a flammable gas.

Combustion reaction: This reaction occurs when a hydrocarbon reacts with oxygen to produce water$(H_2O)$ and carbondioxide ($CO_2$). It is a exothermic reaction which means that heat is released during this reaction.

Now, we need to write a balanced equation for Combustion of butane.

Balancing a Chemical equation: For a chemical equation, a balanced equation is a equation in which the number of atoms for each element and the total charge are same for both reactants and products.

Balanced Equation,

$2C_4H_{10}+ 13O_2\rightarrow 10H_2O+8CO_2$