So in this case, we are talking about a combustion reaction. The equation would be as follows:
[tex] C_{4}H_{8}+6O_{2} [/tex] → [tex] 4CO_{2}+4H_{2}O [/tex]
Now that we have a balanced equation, we can then say that for each molecule of [tex] C_{4}H_{8} [/tex] that reacts, there will be one four molecules of carbon dioxide produced and 4 molecules of water produced, as there is a 1:4:4 ratio between [tex] C_{4}H_{8}:CO_{2}:H_{2}O [/tex] respectively.
Answer : The number of molecules of [tex]CO_2[/tex] and [tex]H_2O[/tex] are, [tex]4\times 6.022\times 10^{23}[/tex] and [tex]4\times 6.022\times 10^{23}[/tex] respectively.
Explanation :
Combustion reaction : It is defined as the reaction in which the hydrocarbon react with oxygen to give carbon dioxide and water as a product.
The given hydrocarbon is, [tex]C_4H_8[/tex]
The balanced combustion reaction will be,
[tex]C_4H_8+5O_2\rightarrow 4CO_2+4H_2O[/tex]
In this reaction, [tex]C_4H_8[/tex] and [tex]O_2[/tex] are the reactants and [tex]CO_2[/tex] and [tex]H_2O[/tex] are the products.
By the stoichiometry we can say that, 1 mole of [tex]C_4H_8[/tex] react with 5 moles of [tex]O_2[/tex] to give 4 moles of [tex]CO_2[/tex] and 4 moles of [tex]H_2O[/tex].
In terms of molecules we can say that, 1 mole contains [tex]6.022\times 10^{23}[/tex] number of molecules.
In the given reaction, there are [tex]6.022\times 10^{23}[/tex] number of molecules of [tex]C_4H_8[/tex], [tex]5\times 6.022\times 10^{23}[/tex] number of molecules of [tex]O_2[/tex], [tex]4\times 6.022\times 10^{23}[/tex] number of molecules of [tex]CO_2[/tex], [tex]4\times 6.022\times 10^{23}[/tex] number of molecules of [tex]H_2O[/tex].
Therefore, the number of molecules of [tex]CO_2[/tex] and [tex]H_2O[/tex] are, [tex]4\times 6.022\times 10^{23}[/tex] and [tex]4\times 6.022\times 10^{23}[/tex] respectively.
