Answer:
644.2918 g of turpentine are consumed.
Explanation:
Calculation of the moles of [tex]C[/tex] as:-
Mass = 569 g
Molar mass of carbon = 12.0107 g/mol
The formula for the calculation of moles is shown below:
[tex]moles = \frac{Mass\ taken}{Molar\ mass}[/tex]
Thus,
[tex]Moles= \frac{569\ g}{12.0107\ g/mol}[/tex]
[tex]Moles_{C}= 47.3744\ mol[/tex]
According to the given reaction:-
[tex]C_{10}H_{16}+8Cl_2\rightarrow 10C+16HCl[/tex]
10 moles of C are produced when 1 mole of turpentine undergoes reaction
1 mole of C are produced when [tex]\frac{1}{10}[/tex] mole of turpentine undergoes reaction
47.3744 moles of C are produced when [tex]\frac{1}{10}\times 47.3744[/tex] moles of turpentine undergoes reaction
Moles of turpentine = 4.73744 moles
Molar mass of turpentine = 136 g/mol
[tex]Mass=Moles\times Molar\ mass=4.73744\ moles\times 136\ g/mol=644.2918\ g[/tex]
644.2918 g of turpentine are consumed.
