To calculate the amount of heat absorbed by water to increase its temperature, we need to use the specific heat capacity of water and the formula:
Q = m * c * ΔT
where Q is the amount of heat absorbed, m is the mass of the water, c is the specific heat capacity of water, and ΔT is the change in temperature.
The specific heat capacity of water is 4.184 J/(g*C), which means that 1 gram of water requires 4.184 joules of energy to raise its temperature by 1 degree Celsius.
Substituting the given values, we have:
m = 9448 g (mass of water)
c = 4.184 J/(g*C) (specific heat capacity of water)
ΔT = (32.50 C - 25.00 C) = 7.50 C (change in temperature)
Q = m * c * ΔT
Q = 9448 g * 4.184 J/(g*C) * 7.50 C
Q = 283,464.72 J
Therefore, the amount of heat absorbed by 9448 g of water in order for the temperature to increase from 25.00 C to 32.50 C is approximately 283,465 J (joules).