I thought Bob Pursley showed you how to do this.
Add equation to the reverse of equation 2. That gives you kJ/mol graphite to diamond. If you want 1 kg, then
kJ/mol from the above x (1000 g/12.01) = ? heat absorbed to make 1 kg.
For part b.
?kg from above = mass H2O x specific heat H2O x 5
Solve for grams H2O. I estimate the answer to be about 100 grams but check me out on that.
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
1 answer