How much heat energy is required to raise the temperature of 4.50 liters of water from 36 degrees celcius to 44.6 degrees celcius?
Note the correct spelling of celsius.
q = mass x specific heat x (Tfinal-Tinitial)
4.50L H2O = 4,500 mL and the density of water is approximately 1.00 g/mL so the mass of the water will be approximately 4,500g.
1620 J
To calculate the amount of heat energy required to raise the temperature of water, you can use the equation:
Q = m * c * ΔT
Where:
Q is the amount of heat energy (in joules),
m is the mass of the water (in kilograms),
c is the specific heat capacity of water (4.186 J/g°C or 4186 J/kg°C), and
ΔT is the change in temperature (in degrees Celsius).
First, you need to convert the volume of water (4.50 liters) to its mass using the density of water:
1 liter of water = 1 kilogram
So, 4.50 liters of water = 4.50 kilograms
Next, you can substitute the values into the formula:
Q = m * c * ΔT
Q = 4.50 kg * 4186 J/kg°C * (44.6°C - 36°C)
Simplifying the equation:
Q = 4.50 * 4186 * 8.6
Using a calculator:
Q ≈ 163,530 joules
Therefore, approximately 163,530 joules of heat energy is required to raise the temperature of 4.50 liters (or 4.50 kilograms) of water from 36°C to 44.6°C.