Balance the following equations for combustion reactions....

Balance the following equations for combustion reactions. Circle the fuel for each reaction. a. $\mathrm{C}_{2} \mathrm{H}_{6}(g)+\mathrm{O}_{2}(g) \longrightarrow \mathrm{CO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(l)$ b. $\mathrm{C}_{6} \mathrm{H}_{6} \mathrm{O}_{6}(s)+\mathrm{O}_{2}(g) \longrightarrow \mathrm{CO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(l)$ c. $\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}(l)+\mathrm{O}_{2}(g) \longrightarrow \mathrm{CO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(l)$ d. $\mathrm{C}_{21} \mathrm{H}_{24} \mathrm{N}_{2} \mathrm{O}_{4}(s)+\mathrm{O}_{2}(g) \longrightarrow \mathrm{CO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(l)+\mathrm{NO}_{2}(g)$ e. $\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{SH}(l)+\mathrm{O}_{2}(g) \longrightarrow \mathrm{CO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(l)+\mathrm{SO}_{2}(g)$

Balance the following equations for combustion reactions. Circle the fuel for each reaction.
a. $\mathrm{C}_{2} \mathrm{H}_{6}(g)+\mathrm{O}_{2}(g) \longrightarrow \mathrm{CO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(l)$
b. $\mathrm{C}_{6} \mathrm{H}_{6} \mathrm{O}_{6}(s)+\mathrm{O}_{2}(g) \longrightarrow \mathrm{CO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(l)$
c. $\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}(l)+\mathrm{O}_{2}(g) \longrightarrow \mathrm{CO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(l)$
d. $\mathrm{C}_{21} \mathrm{H}_{24} \mathrm{N}_{2} \mathrm{O}_{4}(s)+\mathrm{O}_{2}(g) \longrightarrow \mathrm{CO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(l)+\mathrm{NO}_{2}(g)$
e. $\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{SH}(l)+\mathrm{O}_{2}(g) \longrightarrow \mathrm{CO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(l)+\mathrm{SO}_{2}(g)$

Key Concepts

Combustion Reactions

These are exothermic oxidation processes in which a fuel reacts with an oxidizing agent, typically oxygen, to produce combustion products such as carbon dioxide and water. This concept underpins many reactions occurring in energy production, engine operation, and various industrial chemical processes.

Balancing Chemical Equations

This refers to the process of ensuring that the number of atoms for each element is the same on both the reactant and product sides of a chemical equation. It is a practical application of the law of conservation of mass and is crucial for accurate stoichiometric calculations in chemical reactions.

Stoichiometry

This concept involves the quantitative relationships among the reactants and products in a chemical reaction. It allows chemists to calculate the necessary amounts of reactants required for a reaction and predict the yields of the products based on a balanced chemical equation.

Fuel Identification

This involves determining which substance in a reaction serves as the fuel—the main compound that undergoes combustion. Identifying the fuel is key to understanding the reaction dynamics as it is the component that primarily provides the energy upon oxidation.

Transcript

00:01 In problem for balance the each equation and circle the fuel for each reaction.

00:06 So first equation is c2h6 plus o2 gas that will form carbon dioxide plus h2o.

00:19 So that means when ethane reacts with the oxygen, then it will produce carbon dioxide and water.

00:25 So we can balance this equation.

00:27 So this is the balance equation.

00:32 Now we can multiply this equation by 2.

00:36 So multiply by, so we get, if we multiply this equation by 2, then we get this, this is c2h6 plus o2 gas that will form co2 plus h2o liquid.

00:59 So now on multiply equation this by 2, so we get 2c2h6 and this is 7o2 and this is 4 co2 and this is 6h2.

01:09 So both the equation are balanced equation and the fuel for this reaction is this c2h6 or we can say that this all right so in the second equation so in the second equation that is c6 h12.

01:34 So when this reactant reacts with the oxygen then it will produce carbon dioxide and water.

01:44 Now on balancing this equation we get this 6 co2 and this 6 h2 and then here we use 6 .o2.

01:55 So now this is the balance equation and fuel for this reaction is the c6h12.

02:02 So now in the third part of the equation that is the c2h5 -oh and the 3rd.

02:11 So this is the alcohol, which is known as ethyl alcohol.

02:15 So when this reacts with the oxygen gas, then it will produce carbon dioxide and water.

02:25 And water.

02:26 So on balancing this equation, we get.

02:29 So here we use two carbon dioxide and this is the 3h2o and this is the 302.

02:36 So now this is the balanced equation.

02:38 And fuel for this reaction is this c2h5oh that means we can say ethyl alcohol.

02:48 So in the part d of the equation, that is c -21h -24, n2o4.

02:58 So this when reacts with the oxygen gas, then it will produce carbon dioxide, water, carbon dioxide, plus water along with no2 gas.

03:16 So on balancing this equation we get here 21 co2 and total hydrogen on the left hand side is 24.

03:29 So we can multiply this by 12 and now we can count the so nitrogen on the left hand side is 2 so we can multiply this by 2...

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