On a hot summer day, 3.50 ✕ 106 J of heat transfer into a parked car takes place, increasing its temperature from 36.5°C to 44.4°C. What is the increase in entropy (in J/K) of the car due to this heat transfer alone?

On a winter day, a certain house loses 5.80 ✕ 108 J of heat to the outside (about 550,000 Btu). What is the total change in entropy (in J/K) due to this heat transfer alone, assuming an average indoor temperature of 23.5°C and an average outdoor temperature of 5.30°C?

a)

b)

Explanation:

a)

Given:

amount of heat transfer occurred,

initial temperature of car,

final temperature of car,

We know that the change in entropy is given by:

(heat is transferred into the system of car)

b)

amount of heat transfer form the system of house,

initial temperature of house,

final temperature of house,

answer:   you might love summer weather, but you don’t want it to feel like the sun is inside your car. but a hot car that just won’t seem to cool down might be a bigger of a problem than you think. your car relies on being at the right temperature.

explanation:

f is prop to m1xm2 double m1 double force