Natural gas burns in air to form carbon dioxide and water, releasing heat. CH4(g) + O2(g) → CO2(g) + H2O(g) ΔHorxn = -802.3 kJ What minimum mass of CH4 is required to heat 23g of water by 32oC? (Assume 100% heating efficiency.) Natural gas burns in air to form carbon dioxide and water, releasing heat. CH4(g) + O2(g) → CO2(g) + H2O(g) ΔHorxn = -802.3 kJ
Natural gas burns in air to form carbon dioxide and water, releasing heat. CH4(g) + O2(g) → CO2(g) + H2O(g) ΔHorxn = -802.3 kJ What minimum mass of CH4 is required to heat 23g of water by 32oC? (Assume 100% heating efficiency.) Natural gas burns in air to form carbon dioxide and water, releasing heat. CH4(g) + O2(g) → CO2(g) + H2O(g) ΔHorxn = -802.3 kJ
Chemistry by OpenStax (2015-05-04)
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Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
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Chapter5: Thermochemistry
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Natural gas burns in air to form carbon dioxide and water, releasing heat.
CH4(g) + O2(g) → CO2(g) + H2O(g) ΔHorxn = -802.3 kJ
What minimum mass of CH4 is required to heat 23g of water by 32oC? (Assume 100% heating efficiency.)
Natural gas burns in air to form carbon dioxide and water, releasing heat.
CH4(g) + O2(g) → CO2(g) + H2O(g) ΔHorxn = -802.3 kJ
What minimum mass of CH4 is required to heat 23g of water by 32oC? (Assume 100% heating efficiency.)
62 g
22.5 g
7.80 mg
61 mg
118 mg
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