What is the change in enthalpy of the first reaction below, given the enthalpies of the other two reactions?
2C(s) +0,(8) 200(g)
C(s) +0,(g) - CO2(g) AH°-394 kJ/mol
CO(s) +0,() CO2(g) AH° = -283 kJ/mol

pure substance: iron,copper

impure substance: water,charcoal

i think that the answer is c

consider the reaction below.

 no rx

at 500 k, the reaction is at equilibrium with the following concentrations.

[pci5]= 0.0095 m

[pci3] = 0.020

[ci2] = 0.020 m

what is the equilibrium constant for the given reaction?

0.042

0.42

2.4

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