Given the thermochemical equation: SO2 (g) + ½ O2 (g) ? SO3 (g) ?H = -99.0 kJ How much heat is evolved when 75.0 g of SO2 undergoes combustion?
Added by Larry S.
Close
Step 1
First, we need to find the moles of SO2. We know that the molar mass of SO2 is 32.07 g/mol (S) + 2 * 16.00 g/mol (O) = 64.07 g/mol. Show more…
Show all steps
Your feedback will help us improve your experience
Chareen Guzman and 71 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
Calculate heat for the following reaction to produce sulfur dioxide, S(s) + O2(g) = SO2(g) given the thermochemical equations below. 2 S(s) + 3 O2(g) = 2 SO3(g) ΔH° = -791.5 kJ 2 SO2(g) + O2(g) = 2 SO3(g) ΔH° = -197.9 kJ
Ronald P.
Given the thermochemical equation, calculate the heat evolved (in kJ) when 78.9 g of SO2 (molar mass = 64.1 g/mol) is converted to SO3: 2 SO2 + O2 → 2 SO3 ΔH = -198 kJ/mol a. 0 b. -182 c. -244 d. -61.0 e. -122
Madhur L.
S8(s) + 8O2(g) → 8SO2(g) ΔH = –2368 kJ How much heat is evolved when 25.0 moles of sulfur is burned in excess oxygen? How much heat is evolved when 275 grams of sulfur is burned in excess oxygen?
Nicole S.
Recommended Textbooks
Chemistry: Structure and Properties
Chemistry The Central Science
Chemistry
Transcript
Watch the video solution with this free unlock.
EMAIL
PASSWORD