Find the heat transferred (in ) when 5.50 Lof ethylene glycolld \ d=1.11 g/mL) in a car radiator cools from 37.0 °C to 25.0 C.
If you are cooling ethylene glycol from 37 to 25 you are transferring heat OUT. Transferring heat IN would heat it.
q = mass x specific heat x (Tfinal - Tinitial)
mass = volume x density = 5500 mL x 1.11 g/mL = ?
I don't know the specific heat of this material. The problem may expect you to use the specific heat of water OR the specifc heat of ethylene glycol.
Post your work if you get stuck.
Well, let's start by calculating the mass of ethylene glycol. Since we know the volume and density, we can use the formula:
mass = volume x density
mass = 5.50 L x 1.11 g/mL
mass ≈ 6.10 kg
Now, we can use the specific heat capacity of ethylene glycol, which is approximately 2.4 J/g°C.
The equation for calculating heat transfer is:
q = mass x specific heat capacity x change in temperature
q = 6.10 kg x 2.4 J/g°C x (25.0°C - 37.0°C)
q ≈ -351.84 J
So, the heat transferred when the ethylene glycol cools from 37.0 °C to 25.0°C in the car radiator is approximately -351.84 J.
But don't worry, that negativity won't impact your radiator's sense of self-esteem!
To find the heat transferred, we need to use the formula:
Q = m * c * ΔT
Where:
Q = Heat transferred (in Joules)
m = Mass of the substance (in kg)
c = Specific heat capacity of the substance (in J/g°C or J/gK)
ΔT = Change in temperature (in °C or K)
First, we need to find the mass of ethylene glycol:
Mass = volume * density
= 5.50 L * 1.11 g/mL
= 6.105 g
Next, we need to convert the mass from grams to kilograms:
Mass = 6.105 g * (1 kg / 1000 g)
= 0.006105 kg
Now, we can substitute the values into the formula:
Q = 0.006105 kg * c * ΔT
The specific heat capacity of ethylene glycol is 2.42 J/g°C.
ΔT = final temperature - initial temperature
= 25.0°C - 37.0°C
= -12.0°C
Now, substituting the values:
Q = 0.006105 kg * 2.42 J/g°C * -12.0°C
Simplifying:
Q = -0.178 J
Therefore, the heat transferred when 5.50 L of ethylene glycol in a car radiator cools from 37.0 °C to 25.0 °C is -0.178 Joules. Note that the negative sign indicates heat loss.
To find the heat transferred, we can use the formula:
Q = m * c * ΔT
where:
Q is the heat transferred (in joules)
m is the mass of the substance (in grams)
c is the specific heat capacity of the substance (in J/g°C)
ΔT is the change in temperature (in °C)
First, we need to find the mass of ethylene glycol. We can do this by multiplying the volume (5.50 L) by the density (1.11 g/mL).
Mass = Volume * Density
Mass = 5.50 L * 1.11 g/mL
Next, we need to convert the mass from grams to kilograms since specific heat capacity is usually given in J/g°C.
Mass(Kg) = Mass(g) / 1000
Now, we can find the change in temperature:
ΔT = Final temperature - Initial temperature
ΔT = 25.0°C - 37.0°C
Once we have the mass (in kg), the change in temperature (in °C), and the specific heat capacity of ethylene glycol, we can calculate the heat transferred (in joules).