The formula for calculating heat capacity is: Q = m x c x ∆T, where Q is the amount of heat absorbed or released, m is the mass of the substance, c is the specific heat capacity, and ∆T is the change in temperature.
In a heat capacity question, the mass of water is typically given or can be measured using a balance. In this case, the mass of water is 12kg.
The specific heat capacity of water is 4.186 joules per gram per degree Celsius (J/g°C). This means that it takes 4.186 joules of energy to raise the temperature of 1 gram of water by 1 degree Celsius.
To convert Celsius to Kelvin, you add 273.15 to the Celsius temperature. In this question, the initial temperature of 15.4°C would be converted to 288.55K.
The final temperature of the water can be calculated by rearranging the heat capacity formula, Q = m x c x ∆T, to solve for ∆T. In this case, ∆T = Q / (m x c) = (93°C - 15.4°C) = 77.6°C. Therefore, the final temperature of the water is 93°C.