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guymcguyson4573
05.05.2020 •
Chemistry
Calculate the enthalpy of the formation of butane, C4H10, using the balanced chemical equation and the standard value below:
4C(s) + 5H2(g) => C4H10(g)
Standard enthalpy of formation values:
(Delta Triangle)H^0 of C(s)= -393.5kJ/mol
(Delta triangle)H^0f of H2(g)=-285.8 kJ/mol
(Delta triangle)H^0f of C4H10(g)=-2877.6kJ/mol
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Ответ:
+125.4 KJmol-1
Explanation:
∆H C4H10(g) = -2877.6kJ/mol
∆H C(s)=-393.5kJ/mol
∆H H2(g) = -285.8
∆H reaction= ∆Hproducts - ∆H reactants
∆H reaction= (-2877.6kJ/mol) - [4(-393.5kJ/mol) +5(-285.8)]
∆H reaction= +125.4 KJmol-1
Ответ:
2(H2) + 1(O2) = 2 (H2O) is the balanced equation