Question

The enthalpy change for a chemical reaction is the sum of the energy consumed in breaking bonds and the energy released during bond formation. One way to determine the overall energy change for a chemical reaction is to apply Hess's law to add together a group of reactions which can be arranged such that the chemical equations, when combined, give the overall equation we are trying to characterize 3rd attempt See Hint Ad See Periodic Table Part 1 (1 point) Feedback Write a balanced chemical equation for the combustion of gaseous propane in gaseous oxygen to produce gaseous carbon dioxide and liquid water. х х (ag). He cHg(g)+ 5 02(g) 3 CO,()+ 4 H,0(g)

Answer 1

Answer: (part 3)

Step 1: Calculate the moles from mass

We know, moles = mass / molar mass

moles of propane = 17000 g / 44.1 g/mol = 385.4875283 mol [ note: 1 kg = 1000 g ]

Step 2: Calculation

(1) Write the equation

C₃H₈(g) + 5O₂(g)----> 3CO₂(g)+4H₂O(g) ; ΔH= −2219.9 kJ [ Enthapy change you calculated is correct ]

For 1 moles of propane enthaply released = 2219.9  kJ

so, for 385.4875283 mol of enthalpy enthapy released will be = ( 2219.9 kJ / 1 mol ) × 385.4875283 mol = 855743.8 kJ

[ negative sign we did not need because they already mention that calculate energy released but if require you may check by changing it]