Question

How many moles of CO2 are produced when 45.0g of C6H6 react completely in the following equation? 2C6H6+ 15O2 → 12CO2 + 6H2O

Answer 1

The answer is in the photo

Answer 2

Answer : The moles of
`CO_2` produced are, 3.462 moles.

Explanation : given,

Mass of
`C_6H_6` = 45.0 g

Molar mass of
`C_6H_6` = 78 g/mole

First we have to calculate the moles of
`C_6H_6`.

`\text{Moles of }C_6H_6=\frac{\text{Mass of }C_6H_6}{\text{Molar mass of }C_6H_6}=(45.0g)/(78g/mole)=0.577moles`

Now we have to calculate the moles of
`CO_2`

The given balanced chemical reaction is,

`2C_6_H6+15O_2\rightarrow 12CO_2+6H_2O`

From the balanced chemical reaction, we conclude that

As, 2 moles of
`C_6H_6` react to give 12 moles of
`CO_2`.

So, 0.577 moles of
`C_6H_6` react to give
`(12)/(2)* 0.577=3.462` moles of
`CO_2`.

Therefore, the moles of
`CO_2` produced are, 3.462 moles.