Step-by-step explanation:
The molar mass of octane (C8H18) is approximately 114 g/mol.
To find the energy required to increase 1 mole of substance by 10°C, we can use the formula:
ΔE = n * C * ΔT
where ΔE is the energy required, n is the number of moles, C is the specific heat, and ΔT is the change in temperature.
For water, n = 1 mol, C = 4.184 J/gK, and ΔT = 10°C.
So, the energy required to increase 1 mole of water by 10°C is:
ΔE_water = n * C_water * ΔT
= 1 mol * 4.184 J/gK * 10 K
= 41.84 J
For octane, n = 1 mol, C = 2.22 J/gK, and ΔT = 10°C.
So, the energy required to increase 1 mole of octane by 10°C is:
ΔE_octane = n * C_octane * ΔT
= 1 mol * 2.22 J/gK * 10 K
= 22.2 J
Therefore, it takes more energy to increase 1 mole of water by 10°C than 1 mole of octane.