Calculate ΔHrxn for the following reaction:
5C(s)+6H2(g)→C5H12(l)
Use the following reactions and given ΔH′s.
C5H12(l)+8O2(g)→5CO2(g)+6H2O(g),
ΔH= -3244.8 kJ
C(s)+O2(g)→CO2(g), ΔH= -393.5
kJ
2H2(g)+O2(g)→2H2O(g), ΔH=
-483.5 kJ
Express your answer to for significant figures.
5CO2(g) + 6H2O(g) ------> C5H12(l) + 8O2(g) ΔH= +3244.8 kJ take the first reaction and reverse it
5C(s) + 5O2(g) -------> 5CO2(g), ΔH= -1967.5 kJ secon reaction multiplayed with 5
6H2(g) +3O2(g) --------> 6H2O(g), ΔH= -1450.5 kJ third reaction multiplayed with 3 add all together
5C(s) + 6H2(g) --------> C5H12(l) ΔH = 3244.8 - 1967.5 - 1450.5 = -173.2 kj
Calculate ΔHrxn for the following reaction: 5C(s)+6H2(g)→C5H12(l) Use the following reactions and given ΔH′s. C5H12(l...
Calculate ΔHrxn for the following reaction: 5C(s)+6H2(g)→C5H12(l) Use the following reactions and given ΔH values: C5H12(l)+8O2(g)→5CO2(g)+6H2O(g), ΔH= -3244.8 kJ C(s)+O2(g)→CO2(g), ΔH= -393.5 kJ 2H2(g)+O2(g)→2H2O(g), ΔH= -483.5 kJ
Calculate ΔHrxn for the following reaction: 5C(s)+6H2(g)→C5H12(l) Use the following reactions and given ΔH values: C5H12(l)+8O2(g)→5CO2(g)+6H2O(g),ΔHC(s)+O2(g)→CO2(g),ΔH2H2(g)+O2(g)→2H2O(g),ΔH===−3244.8kJ−393.5kJ−483.5kJ Express your answer to four significant figures in kilojoules.
Calculate delta Hrxn for the following reaction: 5C(s)+6H2(g)--->C5H12(l) use the following reactions and given delta H's: C5H12(l)+8O2(g)---> 5CO2(g)+6H2O(g) delta H= -3505.8 kJ C(s)+O2(g)--->CO2(g) delta H= -393.5 kJ 2H2(g)+O2(g)---> 2H2O(g) delta H= -483.5 kJ The steps to solving this problem would be greatly appreciated! Thanks so much!
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the combustion of pentane produces heat according to theequation: C5H12(l) + 8O2(g) -->5CO2(g) + 6H2O(l) ΔHrxn = -3,510kJ How many grams of CO2 are produced per 2,500 kJ ofheat released?
The standard heat of formation, ΔH∘f, is defined as the enthalpy change for the formation of one mole of substance from its constituent elements in their standard states. Thus, elements in their standard states have ΔH∘f=0. Heat of formation values can be used to calculate the enthalpy change of any reaction. Consider, for example, the reaction 2NO(g)+O2(g)⇌2NO2(g) with heat of formation values given by the following table: Substance ΔH∘f (kJ/mol) NO(g) 90.2 O2(g) 0 NO2(g) 33.2 Then the standard heat...