Three moles of an ideal gas undergo a reversible isothermal compression at 22.0°c. during this compression, 1700 j of work is done on the gas. what is the change in entropy of the gas? (j/k)

change in entropy is - 5.7627 J/K

Explanation:

Given data

temperature = 22.0°C = 22 + 273 = 295 K

work is done = 1700 J

to find out

change in entropy

solution

we know that change in entropy = Q /T  1

from 1st law of thermodynamic we know

Q =W for change in internal energy = 0

Q = -1700 J

so from equation 1

change in entropy = - 1700 / 295

change in entropy = - 5.7627

so change in entropy is - 5.7627 J/K

1/0.14nm = 10^10/1.4 a lot

note: the given question is incomplete.

complete question is given below.

which is an example of kinetic energy?

a. the energy stored in ethanol  

b. a hockey puck sliding across the ice  

c. a compressed spring  

d. a ball sitting at the top of a ramp

solution: the kinetic energy is the energy posses by the virtue of the motion of the object.

in the given options, a, c and d are the example of potential energy because it is the energy posses by the virtue of the rest of the object. but option b has the kinetic energy as the object is in motion.

hence, a hockey puck sliding across the ice   is the apex example of kinetic energy.

so, the option (b) a hockey puck sliding across the ice   is the correct option.