Consider the reaction: C₃H₈(g)+ 5 O₂(g)$\rightarrow$3 CO₂(g)+ 4 H₂O(g), where $\Delta$H = -531 kcal/mol. How much heat is released when 3.40 × 10²⁰ molecules of C₃H₈(g)is burned?

Question

Quizplus · Accepted Answer

The reaction releases -531 kcal/mol for one mole of C3H8. First, convert molecules to moles: 3.40 × 10^20 molecules / 6.022 × 10^23 molecules/mol = 5.65 × 10^-4 moles. Then, calculate the heat released: 5.65 × 10^-4 moles × 531 kcal/mol = 0.300 kcal.

Consider the Reaction: C3H8(g)+ 5 O2(g) →\rightarrow→ 3 CO2(g)+ 4 H2O(g), Where

Consider the Reaction: C₃H₈(g)+ 5 O₂(g) $\rightarrow$ 3 CO₂(g)+ 4 H₂O(g), Where