The calculation involves three steps:
1. Determine the temperature difference: ΔT = final temperature - initial temperature = 99°C - 25°C = 74°C
2. Calculate the heat energy required to raise the temperature of the water: Q = mass of water x specific heat capacity x ΔT = 500 g x 4.18 J/g-K x 74°C = 154,440 J
3. Convert the result to the appropriate units: 154,440 J = 1.54 x 10^5 J.
Therefore, the answer is: 1.54 x 10^5 J (option C).
How much of heat is needed to warm 500 g of water from 25 °C near to its boiling point of 99°C? The specific heat of capacity is 4.18J/g-k.
67.9 J
52.3 J
1.54 X 10 squared J
2.10 X10 squared J
1 answer
2 answers