How do you calculate the energy required to produce 7.00 mol #Cl_2O_7# on the basis of the following balanced equation: #2Cl_2(g) + 7O_2(g) + 130 kcal -> 2Cl_2O_7(g)#?

1 Answer
Mar 29, 2018

Answer:

Approx. #450*kcal#...

Explanation:

You gots...

#2Cl_2(g) + 7O_2(g) + 130*kcal rarr 2Cl_2O_7(g)#

Another way of writing this is as...

#2Cl_2(g) + 7O_2(g) rarr 2Cl_2O_7(g)# #DeltaH_"rxn"^@=+130*kcal*mol^-1#

And when we write #mol^-1# we mean per mole of reaction as written...and so to get #7*mol# of the the product...we need #7/2# moles of reaction as written, with the associated enthalpy change....