1). From the following enthalpy changes, S (s) + 3/2 O2 (g) ? SO3 (g) ?H° = -395.2 kJ 2 SO2 (g) + O2 (g) ? 2 SO3 (g) ?H° = -198.2 kJ Calculate the value of ?H° for the reaction by using Hess's law of Heat Summation S (s) + O2 (g) ? SO2 (g). 2) Oxyacetylene torches are fueled by the combustion of acetylene, C2H2. 2 C2H2 + 5 O2 (g) ? 4 CO2 (g) + 2 H2O (g) If the enthalpy change for the reaction is -2511.14 kJ/mol, a) How much heat can be produced by the reaction of 10 g of C2H2? b) Is it an endothermic or exothermic reaction? Molar mass of acetylene is 26.04 g/mol.
Added by Charles R.
Close
Step 1
2 kJ b) 2 SO2(g) + O2(g) → 2 SO3(g) ΔH2 = -198.2 kJ We can manipulate these reactions to get the desired reaction: a) S(s) + 3/2 O2(g) → SO3(g) ΔH1 = -395.2 kJ b) 1/2 * (2 SO2(g) + O2(g) → 2 SO3(g)) ΔH2/2 = -99.1 kJ Now, subtract reaction b from reaction Show more…
Show all steps
Your feedback will help us improve your experience
Adi S and 93 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
Given the following reactions and their associated enthalpies: 1. S(s) + O2(g) -> SO2(g) ΔH = -296.8 kJ 2. 2S(s) + 3O2(g) -> 2SO3(g) ΔH = -792.0 kJ Calculate the enthalpy of the following reaction: 2SO2(g) + O2(g) -> 2SO3(g)
Ronald P.
Determine the enthalpy for the reaction represented by the equation: SO2(g) + 1/2 O2(g) -> SO3(g) Use Hess's law along with the following equations: S(s) + O2(g) -> SO2(g) ΔH = -296.8 kJ 2S(s) + 3O2(g) -> 2SO3(g) ΔH = -795.45 kJ
Chareen G.
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