Final answer:
The amount of heat required to heat 22.0g of water from 25.0°C to 100°C is 19,520 J.
Step-by-step explanation:
The specific heat capacity of water is 4.184 J/g °C. To find the amount of heat required to heat the water, we can use the equation q = m * c * ΔT, where q is the heat, m is the mass of the water, c is the specific heat capacity, and ΔT is the change in temperature. Given that the mass of water is 22.0 g, the initial temperature is 25.0 °C, and the final temperature is 100 °C, we can calculate q as follows:
q = (22.0 g) * (4.184 J/g °C) * (100 °C - 25.0 °C) = 19,520 J
Therefore, the amount of heat required to heat 22.0 g of water from 25.0 °C to 100 °C is 19,520 J.