How many ml of c16h34 are needed to react with 0.050 mol o2, assuming complete combustion occurs? the density of c16h34 is 0.80 g/ml.

0.56 mL

Explanation:

Let's consider the combustion of C₁₆H₃₄.

C₁₆H₃₄ + 24.5 O₂ → 16 CO₂ + 17 H₂O

The molar ratio of C₁₆H₃₄ to O₂ is 1:24.5. The moles of C₁₆H₃₄ that react with 0.050 mol of O₂ are:

0.050 mol O₂ × (1 mol C₁₆H₃₄ / 24.5 mol O₂) = 0.0020 mol C₁₆H₃₄

The molar mass of C₁₆H₃₄ is 226.44 g/mol. The mass of C₁₆H₃₄ is:

0.0020 mol × (226.44 g/mol) = 0.45 g

The density of C₁₆H₃₄ is 0.80 g/mL. The volume of C₁₆H₃₄ is:

0.45 g × (1 mL / 0.80 g) = 0.56 mL

answer: enthalpy

explanation:

for a exothermic reaction, the energy is released i.e. the energy of the products is lower than the energy of the reactants.

= enthaply

= energy of products

= energy of reactants

as , thus comes out to be negative. negative value of enthalpy shows that the reaction is exothermic.