How much heat must be absorbed by a 500 g pot of water in order to raise the temperature from 20„aC to 30„aC?
1*500*80+500*540= 310,000 J
To find the amount of heat required to raise the temperature of a substance, you can use the equation:
Q = mcΔT
Where:
Q = heat (in joules)
m = mass of the substance (in grams)
c = specific heat capacity of the substance (in J/g°C)
ΔT = change in temperature (in °C)
In this case, the mass of the water (m) is 500 g, the specific heat capacity of water (c) is approximately 4.18 J/g°C, and the change in temperature (ΔT) is 30°C - 20°C = 10°C.
Plugging these values into the equation, we have:
Q = (500 g) * (4.18 J/g°C) * (10°C)
Q = 20,900 J
Therefore, the amount of heat that must be absorbed by a 500 g pot of water to raise its temperature from 20°C to 30°C is 20,900 joules.
To calculate the amount of heat required to raise the temperature of a substance, you can use the equation:
Q = mcΔT
Where:
Q = Heat energy
m = Mass of the substance
c = Specific heat capacity of the substance
ΔT = Change in temperature
In this case, the substance is water with a mass of 500 g, the specific heat capacity of water is approximately 4.18 J/g°C, and the change in temperature is 10°C (30°C - 20°C).
Now, let's substitute these values into the equation:
Q = (500 g) * (4.18 J/g°C) * (10°C)
Q = 20,900 J
Therefore, approximately 20,900 Joules of heat must be absorbed by the 500 g pot of water in order to raise its temperature from 20°C to 30°C.