Final answer:
The specific heat of the unknown substance is 0.45 J/g°C. Without a reference table, the substance cannot be identified, but it is not water due to the substantially lower specific heat.
Step-by-step explanation:
To determine the specific heat of the substance, we can use the formula:
Q = mcΔT, where Q is the energy in joules, m is the mass in grams, c is the specific heat capacity in J/g°C, and ΔT is the change in temperature in degrees Celsius.
Given that the substance absorbs 1.305x10² J of heat to raise its temperature from 25.0°C to 45.0°C and that the mass of the substance is 14.5 g, we can rearrange the formula to solve for c:
c = Q / (mΔT).
The change in temperature (ΔT) is 45.0°C - 25.0°C = 20.0°C.
Therefore, c = 1.305x10² J / (14.5 g * 20.0°C) = 0.45 J/g°C.
Without Table 9.1, we can't definitively identify the substance; however, with the specific heat close to that of water (4.18 J/g°C), it is likely not water because the calculated specific heat is much lower. We can compare it to known specific heat values of common substances to make an educated guess.