Question

How many grams of CO2 would be formed from 53.8 g of C2H6 and unlimited O2 in the reaction 2C2H6+7O2–>6H2O+4CO2

Answer 1

157.52

Step-by-step explanation:

Answer 2

Answer : The mass of
`CO_2` formed will be, 157.52 grams.

Solution : Given,

Mass of
`C_2H_6` = 53.8 g

Molar mass of
`C_2H_6` = 30 g/mole

Molar mass of
`CO_2` = 44 g/mole

First we have to calculate the moles of
`C_2H_6`.

`\text{Moles of }C_2H_6=\frac{\text{Mass of }C_2H_6}{\text{Molar mass of }C_2H_6}=(53.8g)/(30g/mole)=1.79moles`

Now we have to calculate the moles of
`CO_2`.

The given balanced chemical reaction is,

`2C_2H_6+7O_2\rightarrow 6H_2O+4CO_2`

From the balanced reaction, we conclude that

As, 2 moles of
`C_2H_6` react to give 4 moles of
`CO_2`

So, 1.79 moles of
`C_2H_6` react to give
`(4)/(2)* 1.79=3.58` moles of
`CO_2`

Now we have to calculate the mass of
`CO_2`.

`\text{Mass of }CO_2=\text{Moles of }CO_2* \text{Molar mass of }CO_2`

`\text{Mass of }CO_2=(3.58mole)* (44g/mole)=157.52g`

Therefore, the mass of
`CO_2` formed will be, 157.52 grams.