The standard molar entropy of C2H6 gas is -232.7 J/mol∙K.
The standard free-energy change, ∆Gº, for the reaction is -112.4 kJ/mol. The sign of ∆Gº indicates that the reaction is exothermic.
The equilibrium constant for the reaction at 298 K is 0.0014.
The C C (triple bond) bond energy in C2H2 is 822 kJ/mol.
C2H2(g) + 2 H2(g)--> C2H6(g)
Substance So (J/mol∙K) ∆Hºf (kJ/mol)
C2H2(g 200.9 226.7
H2(g) 130.7 0
C2H6(g) -- -84.7
Bond Bond Energy (kJ/mol)
C-C 347
C=C 611
C-H 414
H-H 436
If the value of the standard entropy change, ∆Sº for the reaction is -232.7 joules per mole∙Kelvin, calculate the standard molar entropy, Sº, of C2H6
gas.
Calculate the value of the standard free-energy change, ∆Gº, for the reaction. What does the sign of ∆Gº indicate about the reaction above?
Calculate the value of the equilibrium constant for the reaction at 298 K.
Calculate the value of the C C (triple bond) bond energy in C2H2 in kJ/mole.
1 answer