Question

For each molecule of C4H8 that reacts, how many molecules of carbon dioxide and water are produced?

Answer 1

So in this case, we are talking about a combustion reaction. The equation would be as follows:

`C_(4)H_(8)+6O_(2)` →
`4CO_(2)+4H_(2)O`

Now that we have a balanced equation, we can then say that for each molecule of
`C_(4)H_(8)` 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
`C_(4)H_(8):CO_(2):H_(2)O` respectively.

Answer 2

Answer : The number of molecules of
`CO_2` and
`H_2O` are,
`4* 6.022* 10^(23)` and
`4* 6.022* 10^(23)` 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,
`C_4H_8`

The balanced combustion reaction will be,

`C_4H_8+5O_2\rightarrow 4CO_2+4H_2O`

In this reaction,
`C_4H_8` and
`O_2` are the reactants and
`CO_2` and
`H_2O` are the products.

By the stoichiometry we can say that, 1 mole of
`C_4H_8` react with 5 moles of
`O_2` to give 4 moles of
`CO_2` and 4 moles of
`H_2O`.

In terms of molecules we can say that, 1 mole contains
`6.022* 10^(23)` number of molecules.

In the given reaction, there are
`6.022* 10^(23)` number of molecules of
`C_4H_8`,
`5* 6.022* 10^(23)` number of molecules of
`O_2`,
`4* 6.022* 10^(23)` number of molecules of
`CO_2`,
`4* 6.022* 10^(23)` number of molecules of
`H_2O`.

Therefore, the number of molecules of
`CO_2` and
`H_2O` are,
`4* 6.022* 10^(23)` and
`4* 6.022* 10^(23)` respectively.