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

The change in enthalpy for the formation of ethanol is -276.5 kJ/mol

Explanation:

The given reactions are:

The required reaction involves the formation of C2H5OH from C, H2 and O2:

This can be obtained by reversing reaction (1), multiplying equation (2) by 2, multiplying equation (3) by 3 and then adding the corresponding ΔH values

explanation: no but i do not usually comment