Final answer:
The heat absorbed by a 10-g sample of water when its temperature is increased from 23°C to 32°C is 376.56 joules, calculated using the specific heat capacity of water (4.184 J/(g°C)) and the temperature change of 9°C. Thus, the heat absorbed by the 10-g sample of water as it is heated from 23°C to 32°C is 376.56 joules.
Step-by-step explanation:
To determine how much heat is absorbed when a 10-g sample of water changes its temperature from 23°C to 32°C, we need to use the specific heat capacity of water and the formula q = mcΔT, where q is the heat absorbed, m is the mass in grams, c is the specific heat capacity, and ΔT is the change in temperature.
The specific heat capacity of water is 4.184 J/(g°C). The change in temperature (ΔT) is 32°C - 23°C = 9°C.
Using the formula, we calculate the heat absorbed as follows:
q = (10 g)(4.184 J/(g°C))(9°C) = 376.56 J
Thus, the heat absorbed by the 10-g sample of water as it is heated from 23°C to 32°C is 376.56 joules.