Consider the reaction: C3H2828. Consider the reaction: C3H8(g) + 5 O2(g)  3 CO2(g) + 4 H2O(g), where H = – 531 kcal/mol. How much heat is released when 3.40 x 1020 molecules of C3H8(g) is burned?. Consider the reaction: C3H8(g) + 5 O2(g)  3 CO2(g) + 4 H2O(g), where H = – 531 kcal/mol. How much heat is released when 3.40 x 1020 molecules of C3H8(g) is burned?8(g) + 5 O2(g)  3 CO2(g) + 4 H2O(g), where H = – 531 kcal/mol. How much heat is released when 3.40 x 1020 molecules of C3H8(g) is burned?

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catalina151222 catalina151222 · Answer 1 · 2019-11-08T00:20:47+01:00

Answer: Energy released during the reaction is 0,299 kcal

Explanation: ΔH is the amount of energy released when 1 mol of C3H8 reacts, but there is no 1 mol but less, 3.40 x 10^20 molecules

Using Avogadro's number is possible to calculate the number of moles

[tex]n= 3,4x10^{20} molecules . \frac{1 mol}{6,0022x10^{23} molecules } = 5,64x10^{-4} mol[/tex]

The product of the mol number and ΔH is the energy released during the reaction

[tex]H = -531 kcal/mol . 5,64x10^{-4} mol = 0,299 kcal[/tex]