1
answer
0
watching
235
views
11 Nov 2019
Please answer and explain!
The known reactions we will use for this particular example are called enthalpy of formation reactions. We define the ÎHo of formation as the enthalpy change when a compound is made directly from its elements in their natural state. The enthalpy of formation reactions we will use are: 6 C(s) + 6 H2(g) + 3 O2 â C6H 1206(s) 2 c(s) + 3 H2(g) + 1/2 02(g) â C2H5OH(I) c(s) + O2(g) â CO2(g) ì¨to-. 1273.3 k) ì¨+"--277.7 kJ The diagram below depicts the enthalpy change for making each of the species listed directly from their elements. Elements in their natural state C (s); H2 (g) ; 02 (g) 277.7 kJ -393.5 k Enthalpy CH,OH ) - 1273.3 kJ CO2 (g) C&H1206(s a) Rearrange and combine the ì¨to equations given above in order to determine the ì¨to for the overall fermentation reaction. This is the same method you have been using for other Hess's Law problems. kJ/mol
Please answer and explain!
The known reactions we will use for this particular example are called enthalpy of formation reactions. We define the ÎHo of formation as the enthalpy change when a compound is made directly from its elements in their natural state. The enthalpy of formation reactions we will use are: 6 C(s) + 6 H2(g) + 3 O2 â C6H 1206(s) 2 c(s) + 3 H2(g) + 1/2 02(g) â C2H5OH(I) c(s) + O2(g) â CO2(g) ì¨to-. 1273.3 k) ì¨+"--277.7 kJ The diagram below depicts the enthalpy change for making each of the species listed directly from their elements. Elements in their natural state C (s); H2 (g) ; 02 (g) 277.7 kJ -393.5 k Enthalpy CH,OH ) - 1273.3 kJ CO2 (g) C&H1206(s a) Rearrange and combine the ì¨to equations given above in order to determine the ì¨to for the overall fermentation reaction. This is the same method you have been using for other Hess's Law problems. kJ/mol
Lelia LubowitzLv2
28 Sep 2019