The cooling system in an automobile holds 10.0 L of ethylene glycol antifreeze. How much energy
is absorbed when the temperature of the ethylene glycol goes from 20°C to 100°C? The density
and specific heat capacity of ethylene glycol are 1.11 g/mL and 2.42 J/(g • °C),
heatabsorbed=mass*c*deltaTemp
heatabsorbed=10L*1.11g/L*2.42J/gC*80C
2129600
To determine the energy absorbed by the ethylene glycol, we need to calculate the change in temperature and use the specific heat capacity.
Step 1: Convert the volume of ethylene glycol from liters to grams.
Given that the density of ethylene glycol is 1.11 g/mL, we can use the conversion factor:
10.0 L * 1.11 g/mL = 11.1 kg (since 1 L = 1,000 mL)
Step 2: Calculate the mass of the ethylene glycol.
The mass of the ethylene glycol is already given as 11.1 kg.
Step 3: Calculate the change in temperature.
The change in temperature is given as 100°C - 20°C = 80°C.
Step 4: Calculate the energy absorbed.
The formula to calculate the energy absorbed is:
Energy = mass * specific heat capacity * change in temperature
Using the given specific heat capacity of ethylene glycol (2.42 J/(g • °C)), we can calculate the energy absorbed:
Energy = 11.1 kg * 2.42 J/(g • °C) * 80°C
Calculating the energy:
Energy = 2134.32 J
Therefore, the energy absorbed when the temperature of the ethylene glycol goes from 20°C to 100°C is approximately 2134.32 Joules.
To calculate the amount of energy absorbed by the ethylene glycol when its temperature changes, we can use the formula:
Q = m * c * ΔT
Where:
Q is the energy absorbed (in Joules).
m is the mass of the ethylene glycol (in grams).
c is the specific heat capacity of ethylene glycol (in J/(g • °C)).
ΔT is the change in temperature (in °C).
First, we need to calculate the mass of the ethylene glycol from its volume. Given that the density of ethylene glycol is 1.11 g/mL, we can convert the volume of 10.0 L to grams:
mass = volume * density
mass = 10.0 L * 1.11 g/mL
Next, we can calculate the change in temperature (ΔT) by subtracting the initial temperature from the final temperature:
ΔT = final temperature - initial temperature
ΔT = (100°C - 20°C)
Now, we have all the values needed. Plug them into the formula:
Q = mass * c * ΔT
Calculate mass:
mass = 10.0 L * 1.11 g/mL = 11.1 kg
Calculate ΔT:
ΔT = 100°C - 20°C = 80°C
Now we can calculate Q:
Q = 11.1 kg * 2.42 J/(g • °C) * 80°C
Q = 2131.04 J
Therefore, the amount of energy absorbed when the temperature of the ethylene glycol goes from 20°C to 100°C is approximately 2131.04 Joules.