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
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).
To calculate the amount of heat needed to warm the water, you can use the formula:
Q = m * c * ΔT
where:
Q = heat energy (in joules)
m = mass of the water (in grams)
c = specific heat capacity of water (in J/g-°C)
ΔT = change in temperature (in °C)
Given:
m = 500 g
c = 4.18 J/g-°C
ΔT = (99 °C - 25 °C) = 74 °C
Plugging in these values into the formula:
Q = 500 g * 4.18 J/g-°C * 74 °C
Q = 155,380 J
Therefore, the amount of heat needed to warm 500 g of water from 25 °C to 99 °C is approximately 155,380 J.
None of the given options match the correct answer.