0.07 mol sample of octane, c^6h^18 absorbed 3.5 x 10^3 j of energy. calculate the temp increase of octane if the molar heat capacity of octane is 254.0 j/k* mol

n = number of moles of sample of octane = 0.07 mol

Q = energy absorbed by a sample of octane = 3.5 x 10³ J

c = molar heat capacity of octane = 254.0 J/K* mol

ΔT = increase in temperature of octane = ?

Heat absorbed is given as

Q = n c ΔT

inserting the values

3.5 x 10³ J = (0.07 mol) (254.0 J/K* mol) ΔT

ΔT = (3.5 x 10³ )/((0.07) (254.0))

ΔT = 196.85 K

hence increase in temperature comes out to be 196.85 K

every chemical equation adheres to the law of conservation of mass, which states that matter cannot be created or destroyed. therefore, there must be the same number of atoms of each element on each side of a chemical equation.