Hydrogen gas for fuel can be made through the catalyzed reaction of methane gas and steam. Calculate the minimum temperature required for this reaction to achieve an equilibrium constant of unity (K = 1) using only the following information:
CH4+2H2O->4H2+CO2
A) âHËrxn - can be calculated from bond energy (bond enthalpy) values as given in the following table of data: Bond Bond Energy (kJ mol-1)
H-H 436
H-C 414
H-O 464
C=O 799
B) âSËrxn for this reaction can be calculated from the following âSË values (J K-1) at 298K:
C(s, graphite) + 2H2(g) -> CH4(g) âSË = -80.8
C(s, graphite) + O2(g) -> CO2(g) âSË = 2.9
H2(g) + 1/2O2(g) -> H2O(g) âSË = -44.5
C) Using the above two values, calculate âGË for this reaction, and the corresponding reaction equilibrium constant at 298K.
D) Assuming that âHËrxn and âSËrxn are independent of temperature, calculate the temperature (in K) required for this reaction to have K = 1.
Please show all work!
Hydrogen gas for fuel can be made through the catalyzed reaction of methane gas and steam. Calculate the minimum temperature required for this reaction to achieve an equilibrium constant of unity (K = 1) using only the following information:
CH4+2H2O->4H2+CO2
A) âHËrxn - can be calculated from bond energy (bond enthalpy) values as given in the following table of data: Bond Bond Energy (kJ mol-1)
H-H 436
H-C 414
H-O 464
C=O 799
B) âSËrxn for this reaction can be calculated from the following âSË values (J K-1) at 298K:
C(s, graphite) + 2H2(g) -> CH4(g) âSË = -80.8
C(s, graphite) + O2(g) -> CO2(g) âSË = 2.9
H2(g) + 1/2O2(g) -> H2O(g) âSË = -44.5
C) Using the above two values, calculate âGË for this reaction, and the corresponding reaction equilibrium constant at 298K.
D) Assuming that âHËrxn and âSËrxn are independent of temperature, calculate the temperature (in K) required for this reaction to have K = 1.
Please show all work!