Question

How many grams of turpentine are consumed to produce 569g of carbon with C10H16+_8Cl=10C+16HCl

Answer 1

644.2918 g of turpentine are consumed.

Step-by-step explanation:

Calculation of the moles of
`C` as:-

Mass = 569 g

Molar mass of carbon = 12.0107 g/mol

The formula for the calculation of moles is shown below:

`moles = (Mass\ taken)/(Molar\ mass)`

Thus,

`Moles= (569\ g)/(12.0107\ g/mol)`

`Moles_(C)= 47.3744\ mol`

According to the given reaction:-

`C_(10)H_(16)+8Cl_2\rightarrow 10C+16HCl`

10 moles of C are produced when 1 mole of turpentine undergoes reaction

1 mole of C are produced when
`(1)/(10)` mole of turpentine undergoes reaction

47.3744 moles of C are produced when
`(1)/(10)* 47.3744` moles of turpentine undergoes reaction

Moles of turpentine = 4.73744 moles

Molar mass of turpentine = 136 g/mol

`Mass=Moles* Molar\ mass=4.73744\ moles* 136\ g/mol=644.2918\ g`

644.2918 g of turpentine are consumed.