6536 kJ x (16.0/2*molar mass C6H6
dH is -that number. Or it is correct to say that numberr of kJ is released as heat.
The value of delta H for the reaction below is -6536 kJ. ____kJ of heat released in the combutsion of 16.0g of C6H6.
2C6H6(l) + 15O2(g) yield 12CO2(g) + 6H2O
2 answers
First, Determine the number of moles you have of C6H6 (16 g / molar mass (78)) = .206 Moles C6H6
Now its good ol stoichiometry
Using the formula given
2 moles of C6H6 produce the -6536 kJ
.206 C6H6 * -6536kJ / 2 moles C6H6 = -673.208 (or so)
Now its good ol stoichiometry
Using the formula given
2 moles of C6H6 produce the -6536 kJ
.206 C6H6 * -6536kJ / 2 moles C6H6 = -673.208 (or so)
2 answers