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calculate the enthalpy change for the following reaction:
C (s) + 2 H2 (g) --> CH4 (g)
(bond dissociation energy of H-H and C-H bonds are 436 KJ/mol and 415 KJ/mol, respectively. dHf of C (g) = 715 KJ/mol)
My solution:
CH4 - 2*H2 - C =
4*C-H - 2*H-H - C =
4*(415) - (715) - 2*2*(436) =
Am I doing it right?
C (s) + 2 H2 (g) --> CH4 (g)
(bond dissociation energy of H-H and C-H bonds are 436 KJ/mol and 415 KJ/mol, respectively. dHf of C (g) = 715 KJ/mol)
My solution:
CH4 - 2*H2 - C =
4*C-H - 2*H-H - C =
4*(415) - (715) - 2*2*(436) =
Am I doing it right?