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Use Table 9.4 to calculate an approximate enthalpy or heat of reaction for the combustion of one mole of methane gas (CH4) to form gaseous H₂O and CO₂. What Volume (in L) of methane is needed to produce 2715 kJ of heat for methane gas at 33 °C and 9.50 atm pressure? Hint given in feedback

Use Table 9.4 to calculate an approximate enthalpy or heat of reaction for the combustion of one mole of methane gas (CH4) to form gaseous H₂O and CO₂. What Volume (in L) of methane is needed to produce 2715 kJ of heat for methane gas at 33 °C and 9.50 atm pressure? Hint given in feedback

Chemistry by OpenStax (2015-05-04)
Chemistry by OpenStax (2015-05-04)
1st Edition
ISBN:9781938168390
Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Chapter5: Thermochemistry
Section: Chapter Questions
Problem 44E: Although the gas used in an oxyacetylene torch (Figure 5.7) is essentially pure acetylene, the heat...
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Use Table 9.4 to calculate an approximate enthalpy or heat of reaction for the combustion of one mole of methane gas (CH4) to form gaseous H₂O and CO₂. What Volume (in L) of methane is needed to produce 2715 kJ of heat for methane gas at 33 °C and 9.50 atm pressure? Hint given in feedback
Transcribed Image Text:Use Table 9.4 to calculate an approximate enthalpy or heat of reaction for the combustion of one mole of methane gas (CH4) to form gaseous H₂O and CO₂. What Volume (in L) of methane is needed to produce 2715 kJ of heat for methane gas at 33 °C and 9.50 atm pressure? Hint given in feedback
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