How can an unknown H reaction be determined using Hess law
To use Hess Law, one simply uses the known equations and their
respective ∆H values, rearranges them as necessary to arrive at the
target equation (unknown ∆H) and then adds the ∆H values to obtain
the value for the target equation. This is possible because Hess
Law applies to state functions which are independent of the
path.
1: At which temperature would a reaction withΔH = -102 kJ/mol, ΔS = -0.188 kJ/(mol×K) be spontaneous2:At which temperature would a reaction withΔH = 132 kJ/mol, ΔS = 0.200 kJ/(mol×K) be spontaneous
Using the following thermochemical data, what is the change in enthalpy for the following reaction: 3H2(g) + 2C(s) + ½O2(g) → C2H5OH(l) C2H5OH(l)+3O2(g)→2CO2(g)+3H2O(l), ΔH = –1367 kJ/mol C(s)+O2(g)→CO2(g), ΔH = –393.5 kJ H2(g)+½O2(g)→H2O(l), ΔH = –285.8 kJ a. -277.6 kJ/mol b. -194.7 kJ/mol c. 194.7 kJ/mol d. 486 kJ/mol