How much energy is needed to change the temperature of 25.00 mL of water from 10.0°C to 95.0°C? [C_p = 75.38 J/(mol.°C),d = 1.00 g/mL]

Question

Quizplus · Accepted Answer

To calculate the energy needed, use the formula q = m × C × ΔT. The mass (m) of water is 25.00 g (since density is 1.00 g/mL). The specific heat capacity (C) is 4.184 J/g°C (converted from 75.38 J/mol°C using the molar mass of water, 18.015 g/mol). The temperature change (ΔT) is 85.0°C (95.0°C - 10.0°C). Plugging in these values gives q = 25.00 g × 4.184 J/g°C × 85.0°C = 8,890 J, which is 8.89 kJ.

How Much Energy Is Needed to Change the Temperature of 25.00