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Explanation: Step 1: Identify the variablesIn this problem, we are given the mass of the water (20 mL), the initial temperature (7°C), and the final temperature (98°C). We are asked to find the energy content of the water. Step 2: Use the formula for heatThe formula to calculate the heat (Q) absorbed or released by a substance is given by: **Q = mLΔT**where:- m is the mass of the substance,- L is the specific heat capacity of the substance, and- ΔT is the change in temperature. Step 3: Convert the volume of water to massSince the density of water is approximately 1 g/mL, the mass of 20 mL of water is approximately 20 g. Step 4: Calculate the change in temperatureThe change in temperature (ΔT) is the final temperature minus the initial temperature. In this case, ΔT = 98°C - 7°C = 91°C. Step 5: Use the specific heat capacity of waterThe specific heat capacity (L) of water is 4.184 J/g°C. Step 6: Substitute the values into the formulaSubstitute the values of m, L, and ΔT into the formula to calculate Q: **Q = 20 g * 4.184 J/g°C * 91°C** Answer: After performing the calculation, we find that the energy content of the water is approximately 7625.44 J.

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