Question

Determine the number of grams of C4H10 that are required to completely react to produce 8.70 mol of CO2 according to the following combustion reaction: 2C4H10 13O2 --> 8CO2 10H2O

Answer 1

126.4 g of
`C_(4)H_(10)` are required

Step-by-step explanation:

Balanced reaction:
`2C_(4)H_(10)+13O_(2)\rightarrow 8CO_(2)+10H_(2)O`

According to balanced reaction-

8 moles of
`CO_(2)` are produced from 2 moles of
`C_(4)H_(10)`

So, 8.70 moles of
`CO_(2)` are produced from
`((2)/(8)* 8.70)` moles of
`C_(4)H_(10)` or 2.175 moles of
`C_(4)H_(10)`

Molar mass of
`C_(4)H_(10)` = 58.12 g/mol

So, mass of
`C_(4)H_(10)` required =
`(2.175* 58.12)g` = 126.4 g

Hence 126.4 g of
`C_(4)H_(10)` are required