The reaction through which carbon changes from graphite to diamond form is represented by the equation
C(graphite) ---> C(diamond) delta H: ?
Using the reactions below, determine the amount of heat absorbed in the change of one mole of graphite to one mole of diamond
C(graphite) + O2 ---> CO2(g) delta H is -393.5 kJ/mol
C(diamond) + O2(g) ---> CO2(g) Delta H is -395.4 kJ/mol
How much energy is absorbed in the manufacture of one kilogram of diamond?
If this reaction were to take place in water, how many grams of water could be cooled by 5 degrees Celsius by the formation of 1 mol of diamond