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 to 100 ? The density and specific heat capacity of ethylene glycol are 1.11 g/mL and 2.42 J/(g . ), respectively.

Question

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  to 100  ? The density and specific heat capacity of ethylene glycol are 1.11 g/mL and 2.42 J/(g . ), respectively.

Quizplus · Accepted Answer

First, we need to calculate the mass of the ethylene glycol:

density = mass/volume

mass = density x volume

mass = 1.11 g/mL x 10.0 L x 1000 mL/L

mass = 11,100 g

Next, we need to calculate the change in temperature:

ΔT = T_final - T_initial

ΔT = 100°F - 20°F

ΔT = 80°F

Finally, we can calculate the energy absorbed:

q = mcΔT

q = 11,100 g x 2.42 J/(g°F) x 80°F

q = 2,150,080 J = 2,150 kJ

So the answer is (B) 2,150 kJ.

The Cooling System in an Automobile Holds 10