To calculate the amount of heat required to heat 250.0 g of water from 22.0 degrees C to 75.0 degrees C, we can use the formula:
Q = m × c × ΔT
where Q is the amount of heat, m is the mass of the water, c is the specific heat capacity of water, and ΔT is the change in temperature of the water.
The specific heat capacity of water is 4.184 J/(g·°C), which means that it takes 4.184 joules of energy to raise the temperature of 1 gram of water by 1 degree Celsius.
Substituting the given values, we get:
Q = 250.0 g × 4.184 J/(g·°C) × (75.0°C - 22.0°C)
Q = 250.0 g × 4.184 J/(g·°C) × 53.0°C
Q = 55,317.2 J or 55.32 kJ (to two decimal places)
Therefore, it requires 55.32 kJ of heat to raise the temperature of 250.0 g of water from 22.0°C to 75.0°C.