PLZ help me understand the way of solving this equation quick
A 0.07 mol sample of octane C8H18 absorbed 3.5*10^3 j of energy. calculate the temperature increase of octane if the molar heat capacity of octane is 254.0 j/k*mol
q = mass x specific heat x dT
3.5E3 = 0.07mol x 254 J/k*mol x dT
Solve for dT.
Check your problem and make sure that is J and not kJ (both places where you have J).
To solve this equation, we will use the formula:
q = n * C * ΔT
Where:
- q represents the energy absorbed by the substance (in joules),
- n is the number of moles of the substance,
- C is the molar heat capacity of the substance (in joules per kelvin per mole), and
- ΔT is the change in temperature of the substance (in kelvin).
In this case, you are given:
- q = 3.5 * 10^3 J
- n = 0.07 mol
- C = 254.0 J/K*mol (molar heat capacity of octane)
We need to solve for ΔT, the change in temperature of octane.
Rearranging the formula, we get:
ΔT = q / (n * C)
Substituting the known values:
ΔT = (3.5 * 10^3 J) / (0.07 mol * 254.0 J/K*mol)
Now, let's calculate the value:
ΔT = (3.5 * 10^3 J) / (17.78 J/K)
ΔT ≈ 196.4 K
So, the temperature increase of octane (ΔT) is approximately 196.4 Kelvin.