How much heat in kilojoules has to be removed from 225g of water to lower its temperature from 25.0 degrees celsius to 10.0 degrees celsius?
See your other post. Same formula.
-14.1 kJ
To calculate the heat that needs to be removed from the water, we can use the formula:
Q = m * c * ΔT
Where:
Q = heat (in kilojoules)
m = mass of the water (in grams)
c = specific heat capacity of water (4.18 J/g°C)
ΔT = change in temperature (in degrees Celsius)
First, let's convert the mass from grams to kilograms:
m = 225g ÷ 1000g/kg = 0.225kg
Now, let's calculate the change in temperature:
ΔT = 25.0°C - 10.0°C = 15.0°C
Now, we can substitute the values into the equation:
Q = 0.225kg * 4.18 J/g°C * 15.0°C
To convert the result to kilojoules, we need to divide by 1000:
Q = (0.225kg * 4.18 J/g°C * 15.0°C) ÷ 1000
Calculating this equation, we get:
Q ≈ 1.479 kilojoules
Therefore, approximately 1.479 kilojoules of heat needs to be removed from the water to lower its temperature from 25.0 degrees Celsius to 10.0 degrees Celsius.
To determine the amount of heat that needs to be removed from the water, you can use the formula:
Q = m * c * ΔT
Where:
Q is the amount of heat in joules
m is the mass of the water in grams
c is the specific heat capacity of water, which is approximately 4.18 J/g°C
ΔT is the change in temperature in degrees Celsius
First, let's convert the mass from grams to kilograms:
mass = 225g = 0.225kg
Next, calculate the change in temperature:
ΔT = final temperature - initial temperature
ΔT = 10.0°C - 25.0°C = -15.0°C
Now we can plug these values into the formula:
Q = 0.225kg * 4.18 J/g°C * -15.0°C
Note that the specific heat capacity of water is given in joules per gram per degree Celsius, so we need to multiply by the mass in grams and not kilograms.
To convert the answer to kilojoules, we need to divide by 1000:
Q = (0.225kg * 4.18 J/g°C * -15.0°C) / 1000
Calculating this expression will give us the amount of heat that needs to be removed from the water in kilojoules.