First, we need to calculate the change in temperature:
ΔT = final temperature - initial temperature = 20°C - 100°C = -80°C
Note that the change in temperature is negative, indicating a cooling process.
Next, we can calculate the amount of heat lost using the formula:
Q = mcΔT
Where:
- Q is the amount of heat lost (in joules)
- m is the mass of the metal bar (in grams)
- c is the specific heat of the metal (in J/g°C)
- ΔT is the change in temperature (in °C)
Substituting the given values:
Q = (4110 g) x (0.2311 J/g°C) x (-80°C)
Q = -76,234.04 J
Note that the negative sign indicates that heat is lost (rather than gained). Therefore, the answer is 76,234.04 J of heat lost when the Fran metal bar cools from 100°C to 20°C.
How much heat is lost when 4110 Fran metal bar whose specific heat is 0.2311j/ gc cools from 100c to 20c
3 answers
How much heat is required to raise the temperature of 854 g of water from 23.5 c to 85 c
We can use the formula:
Q = mcΔT
Where:
- Q is the amount of heat needed (in joules)
- m is the mass of the water (in grams)
- c is the specific heat of water (4.184 J/g°C)
- ΔT is the change in temperature (in °C)
Substituting the given values:
Q = (854 g) x (4.184 J/g°C) x (85°C - 23.5°C)
Q = 251,704.72 J
Therefore, 251,704.72 J of heat is required to raise the temperature of 854 g of water from 23.5°C to 85°C.
Q = mcΔT
Where:
- Q is the amount of heat needed (in joules)
- m is the mass of the water (in grams)
- c is the specific heat of water (4.184 J/g°C)
- ΔT is the change in temperature (in °C)
Substituting the given values:
Q = (854 g) x (4.184 J/g°C) x (85°C - 23.5°C)
Q = 251,704.72 J
Therefore, 251,704.72 J of heat is required to raise the temperature of 854 g of water from 23.5°C to 85°C.