The complete combustion of propane, C3H8(g), is represented by the equation: C3H8(g) + 5O2(g) → 3CO2(g) + 4H2O(l) ΔH° = -1,930 kJ How much heat is evolved in the complete combustion of 172 g of O2(g) (Mw = 32 g/mol)?
Added by Jacqueline H.
Step 1
Moles of O2 = mass / molar mass = 172 g / 32 g/mol = 5.375 mol From the balanced chemical equation, we know that 5 moles of O2 produce -1930 kJ of heat. Show more…
Show all steps
Your feedback will help us improve your experience
Sri K and 82 other Chemistry 101 educators are ready to help you.
Ask a new question
Labs
Want to see this concept in action?
Explore this concept interactively to see how it behaves as you change inputs.
Key Concepts
Recommended Videos
The complete combustion of propane, C3H8(g), is represented by the following unbalanced equation C3H8 (g) + O2 (g) -> CO2 (g) + H2O (l) DH = -2220 kJ How much heat, in kJ, is evolved by the complete combustion of 1.100g C3H8, (g)?
Chareen G.
How much heat is produced by the combustion of 212 g of propane (C3H8)? C3H8(g) + 5O2(g) ⟶ 3CO2(g) + 4H2O(l) ΔH° = -2220 kJ/mol
Sima S.
The combustion of propane is given by the following reaction: C3H8 + 5 O2 → 3 CO2 + 4 H2O The enthalpy of reaction is -2202.0 kJ/mol. How much energy (in joules) will be released if 72.12 grams of propane is burned? (Molar mass of propane = 44.11 g/mol).
Ronald P.
Recommended Textbooks
Chemistry: Structure and Properties
Chemistry The Central Science
Chemistry
Transcript
18,000,000+
Students on Numerade
Trusted by students at 8,000+ universities
Watch the video solution with this free unlock.
EMAIL
PASSWORD