Final answer:
The balanced chemical equation for the reaction of C₁₀H₁₆ with Cl₂ is C₁₀H₁₆ + 8 Cl₂ -> 10 C + 16 HCl. The molar mass of C₁₀H₁₆ is 136.128 g/mol. The reaction is a halogenation and combustion type, producing Carbon (C) and Hydrogen chloride (HCl) as products.
Step-by-step explanation:
The balanced chemical equation for the reaction of C₁₀H₁₆ with Cl₂ is C₁₀H + 8 Cl₂ -> 10 C + 16 HCl. To balance the equation, you ensure that an equal number of atoms of each element is present on both sides of the reaction.
To calculate the molar mass of C₁₀H₁₆, add up the molar masses of carbon (C, approximately 12.01 g/mol) and hydrogen (H, approximately 1.008 g/mol). With 10 carbon atoms and 16 hydrogen atoms, the molar mass of C₁₀H₁₆ is (10 x 12.01) + (16 x 1.008) = 136.128 g/mol.
The products of the reaction are Carbon (C) and Hydrogen chloride (HCl).
This reaction is a type of halogenation reaction, as well as a combustion reaction since the hydrocarbon is being transformed into its respective elements.