Final answer:
A total of 7426.3 calories of heat are required to raise the temperature of 225g of water from 10.5°C to 43.7°C, calculated using the specific heat capacity of water and the formula q = m × c × ΔT.
Step-by-step explanation:
To calculate the calories of heat required to raise the temperature of 225g of water from 10.5°C to 43.7°C, we use the specific heat capacity of water, which is 4.184 J/g °C. The specific heat capacity is the amount of heat needed to raise the temperature of 1 gram of a substance by 1°C.
The formula to calculate heat (q) is q = mass (m) × specific heat capacity (c) × temperature change (ΔT).
The temperature increase we're looking at is 43.7°C - 10.5°C = 33.2°C.
Let's calculate the heat required in joules initially:
q = 225g × 4.184 J/g°C × 33.2°C = 31084.8 J.
Since 1 calorie is equal to 4.184 joules, we need to convert joules to calories.
Therefore, the heat required is 31084.8 J ÷ 4.184 J/cal = 7426.3 calories.
The answer is that 7426.3 calories of heat are required to raise the temperature of 225g of water from 10.5°C to 43.7°C.