Can someone help me check if my answer is correct for the thermochemical equation for the complete combustion of anthracene is:
2C14H10 (s) + 33O2 (g) --- 28CO2 (g) + 10H2O (l) + 6840 kj
or
2C14H10 (s) + 33O2 (g) --- 28CO2 (g) + 10H2O (l), ∆H=-6840 kj

Question

Can someone help me check if my answer is correct for the thermochemical equation for the complete combustion of anthracene is:
2C14H10 (s) + 33O2 (g) ---> 28CO2 (g) + 10H2O (l) + 6840 kj
or
2C14H10 (s) + 33O2 (g) ---> 28CO2 (g) + 10H2O (l),    ∆H=-6840 kj

chmvijay · Answer

what is ur question? and answer ?

anonymous · Answer

A 2.56 g sample of anthracene, C14H10, was burned to heat an aluminum calorimeter (mass = 948 g). The calorimeter contained 1.50 L of water with an initial temperature of 20.5oC and a final temperature of 34.3oC. The molar heat for the combustion of anthracene is -6840 kJ/mol. What is the thermochemical equation, in two ways, for the complete combustion of anthracene?