Final answer:
The amount of energy required to heat 474g of water from 5.4°C to 98.6°C is 2.93 × 10^4 J.
Step-by-step explanation:
To calculate the amount of energy required to heat the water, we can use the equation Q = mcΔT, where Q is the energy in joules, m is the mass of the water in grams, c is the specific heat of water in J/g °C, and ΔT is the change in temperature.
Substituting the given values into the equation:
Q = (474g) × (4.184 J/g °C) × (98.6°C - 5.4°C)
Solving this equation:
Q = 2.93 × 104 J
Therefore, the amount of energy required to heat 474g of water from 5.4°C to 98.6°C is 2.93 × 104 J.