Flask A contains 500 mL of water at 25 degrees Celsius and flask B contains 250 mL of water at 50 degrees Celsius. Which flask has a higher heat content? Explain your choice.
change temp to kelvins, and you immediatly know the answer:
Heat available: mass*tempinKelvins
to get kelvins, add 297 to degrees C.
to get Kelvins you add 273 to C NOT 297
To determine which flask has a higher heat content, we need to consider the principle of heat transfer.
The heat content of an object, in this case, a flask of water, can be calculated using the formula:
Q = mcΔT
Where:
Q (heat content) is measured in joules (J)
m (mass) is measured in grams (g)
c (specific heat capacity) is measured in joules per gram per degree Celsius (J/g°C)
ΔT (change in temperature) is measured in degrees Celsius (°C)
In this scenario, flask A contains 500 mL of water at 25 degrees Celsius, and flask B contains 250 mL of water at 50 degrees Celsius.
To compare their heat contents, we need to calculate the heat content for each flask using the given values and the specific heat capacity of water, which is approximately 4.18 J/g°C.
For flask A:
m = mass = volume × density
= 500 mL × 1 g/mL (since the density of water is approximately 1 g/mL)
= 500 g
ΔT = final temperature - initial temperature
= 25°C - 0°C (initial temperature is given as 0°C)
= 25°C
Q (flask A) = mcΔT
= 500 g × 4.18 J/g°C × 25°C
= 52,250 J
For flask B:
m = mass = volume × density
= 250 mL × 1 g/mL (since the density of water is approximately 1 g/mL)
= 250 g
ΔT = final temperature - initial temperature
= 50°C - 0°C (initial temperature is given as 0°C)
= 50°C
Q (flask B) = mcΔT
= 250 g × 4.18 J/g°C × 50°C
= 52,500 J
Now, comparing the heat contents, we can see that the heat content of flask B is higher (52,500 J) compared to flask A (52,250 J). Therefore, flask B has a higher heat content.