Final answer:
The amount of heat lost by the water is -729.4 J.
Step-by-step explanation:
To calculate the amount of heat lost by the water, we can use the equation: Q = mcΔT, where Q is the heat lost, m is the mass of the water, c is the specific heat capacity of water, and ΔT is the change in temperature. Given that the sample has a volume of 7.00 mL, we can assume its mass is approximately 7.00 g (since the density of water is close to 1 g/mL). The specific heat capacity of water is 4.184 J/(g°C). The change in temperature is calculated as ΔT = Tfinal - Tinitial = 25.0°C - 50.0°C = -25.0°C. Plugging these values into the equation, we get: Q = (7.00 g)(4.184 J/(g°C))(-25.0°C) = -729.4 J.