Synthetic natural gas (SNG) is a methane-containing mixture produced from the gasification of coal or oil shale directly at the site of the mine or oil field. One reaction for the production of SNG is: 4 CO (g) + 8 H2 (g) → 3 CH4 (g) + CO2 (g) + 2 H2O (g)Use the following thermochemical equations to determine ΔHo for the reaction as written. C(graphite) + 2 H2 (g) → CH4 (g) H2 (g) + 1/2 O2 (g) → H2O (g) C(graphite) + 1/2 O2 (g) → CO (g) CO(g) + 1/2 O2 (g) → CO2 (g) ΔHo = -74.8 kJ ΔHo = -285.8 kJ ΔHo = -110.5 kJ ΔHo = -283.0 kJ 5b. For the previous SNG reaction, how much energy would be released/gained if 200.0 g of CO were allowed to react with 400.0 g of H2?
Synthetic natural gas (SNG) is a methane-containing mixture produced from the gasification of coal or oil shale directly at the site of the mine or oil field. One reaction for the production of SNG is: 4 CO (g) + 8 H2 (g) → 3 CH4 (g) + CO2 (g) + 2 H2O (g)Use the following thermochemical equations to determine ΔHo for the reaction as written. C(graphite) + 2 H2 (g) → CH4 (g) H2 (g) + 1/2 O2 (g) → H2O (g) C(graphite) + 1/2 O2 (g) → CO (g) CO(g) + 1/2 O2 (g) → CO2 (g) ΔHo = -74.8 kJ ΔHo = -285.8 kJ ΔHo = -110.5 kJ ΔHo = -283.0 kJ 5b. For the previous SNG reaction, how much energy would be released/gained if 200.0 g of CO were allowed to react with 400.0 g of H2?
Chemistry: Principles and Reactions
8th Edition
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:William L. Masterton, Cecile N. Hurley
Chapter8: Thermochemistry
Section: Chapter Questions
Problem 36QAP: Given the following thermochemical equations: 4B(s)+3O2(g)2B2O3(s)H=2543.8kJ H2(g)+12...
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Synthetic natural gas (SNG) is a methane-containing mixture produced from the gasification of coal or oil shale directly at the site of the mine or oil field. One reaction for the production of SNG is:
4 CO (g) + 8 H2 (g) → 3 CH4 (g) + CO2 (g) + 2 H2O (g)
Use the following thermochemical equations to determine ΔHo for the reaction as written.
C(graphite) + 2 H2 (g) → CH4 (g) H2 (g) + 1/2 O2 (g) → H2O (g) C(graphite) + 1/2 O2 (g) → CO (g) CO(g) + 1/2 O2 (g) → CO2 (g)
ΔHo = -74.8 kJ ΔHo = -285.8 kJ ΔHo = -110.5 kJ ΔHo = -283.0 kJ
5b. For the previous SNG reaction, how much energy would be released/gained if 200.0 g of CO were allowed to react with 400.0 g of H2?
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