Answer to Question #286918 in General Chemistry for mia

Question #286918

the thermochemical equation for the incomplete combustion of carbon into carbon monoxide is represented as: 2C+O2(g) = 2CO(g)

Applying hess's law, compute for the ΔH of the reaction if overall process above can occur in two steps whose thermochemical equations are given below:

  1. C(s)+O2(g) = CO2(g) ΔH°= -393.5 kJ
  2. 2CO(g) +O2(g) = 2CO2(g) ΔH°= -566.0 kJ
1
Expert's answer
2022-01-14T11:28:02-0500

ROUTE 1

2C(s)+O2(g)2CO(g)  ΔH2°2C_{(s)}+O_{2(g)}\to2CO_{(g)}\>\>\Delta\>H_2^°


2CO(g)+O2(g)2CO2(g)  ΔH3°=566kJ2CO_{(g)}+O_{2(g)}\to2CO_{2(g)}\>\>\Delta\>H_3^°=-566kJ



ROUTE 2


2C(s)+2O2(g)2CO2(g)  ΔH1=(393.5×2)kJ2C_{(s)}+2O_{2(g)}\to2CO_{2(g)}\>\>\Delta\>H_1=(-393.5×2)kJ



Applying Hess's Law


ΔH1=ΔH2+ΔH3\Delta\>H_1=\Delta\>H_2+\Delta\>H_3

393.5×2=ΔH2+566-393.5×2=\Delta\>H_2+-566


ΔH2=221kJ\Delta\>H_2=-221kJ





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