How to Calculate Heat Transfer in a Specific Scenario
How many kilocalories are required to increase the temperature of 15.6g of iron from 122°C to 355°C?
The specific heat of iron is 0.450 J/g°C.
Answer:
0.415 kilocalories are required to increase the temperature of 15.6g of iron from 122°C to 355°C.
To solve this problem, we used the quantity of heat formula Q = mcΔT. By plugging in the given values, we determined that 0.415 kilocalories are needed to increase the temperature as specified.
Explanation:
In order to calculate the heat transfer in this scenario, we utilized the formula Q = mcΔT. Here, Q represents the quantity of heat, m is the mass, c is the specific heat capacity, and ΔT is the difference in temperature. After calculating the result in joules, we converted it to kilocalories.
By plugging in the provided values, the heat required was determined to be: Q = 15.6 g * 0.450 J/g°C * (355°C - 122°C) = 1737.42 J. To convert this value to kilocalories, we used the conversion factor 1 Kcal = 4184 J. Therefore, Q = 1737.42 J * (1 Kcal/4184 J) = 0.415 Kcal.
Conclusion:
Hence, 0.415 kilocalories are essential to raise the temperature of 15.6g of iron from 122°C to 355°C.