How much energy would be needed to warm 1.5 L of water from 0 °C to 25 °C? The specific heat capacity of water is 4186 J/kg/°C.
To calculate the amount of energy needed to warm the water, we can use the formula:
Q = m * c * ΔT
Where:
Q is the energy needed (in joules)
m is the mass of the water (in kilograms)
c is the specific heat capacity of water (in J/kg/°C)
ΔT is the change in temperature (in °C)
First, we need to convert the volume of water into mass by using its density. The density of water is approximately 1 kg/L, so the mass (m) of 1.5 L of water is 1.5 kg.
Next, we calculate the change in temperature (ΔT):
ΔT = final temperature - initial temperature
ΔT = 25 °C - 0 °C
ΔT = 25 °C
Now we can substitute these values into the formula:
Q = 1.5 kg * 4186 J/kg/°C * 25 °C
Calculating this gives us:
Q = 156,975 Joules
Therefore, approximately 156,975 Joules of energy would be needed to warm 1.5 L of water from 0 °C to 25 °C.