Final answer:
The total heat required to raise the temperature of 93.0 g of water from its melting point to its boiling point is 38,898 J, and the total heat required to melt 10 g of ice is 51,864 J.
Step-by-step explanation:
To calculate the heat required to raise the temperature of water from its melting point to its boiling point, we need to consider the three phases of water and the heat required for each phase transition.
First, we calculate the heat required to raise the temperature of the 93.0 g of water from its melting point (0°C) to its boiling point (100°C) using the specific heat capacity of water, which is 4.18 J/g°C.
Q1 = m x C x ΔT
= (93.0 g) x (4.18 J/g°C) x (100 - 0)
= 38,898 J
Then, we calculate the heat required to melt the same mass of ice using the observation in the 18th century mentioned in the question, which states that this heat is equal to four-thirds of the heat required to raise the temperature. Therefore, the heat required to melt 10 g of ice is (4/3) x 38,898 J = 51,864 J.
In summary, the total heat required to raise the temperature of 93.0 g of water from its melting point to its boiling point is 38,898 J and the total heat required to melt 10 g of ice is 51,864 J.