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Chapter 15: 15-6Q (page 412)

(a) What happens if you remove the lid of a bottle containing chlorine gas? (b) Does the reverse process ever happen? Why or why not? (c) Can you think of two other examples of irreversibility?

Short Answer

Expert verified
  1. The chlorine gas will create a mixture of air-chlorine gas inside the room.
  2. No, the reverse process can never happen.
  3. Two examples can be if you break a plastic scale, it cannot be restored to its original shape, and if you open the lid of a perfume bottle, it cannot be reversed.

Step by step solution

01

Concepts

Diffusion is a property of gas.

The incident takes place in a way by which the entropy of the system increases.

02

Explanation for part (a) 

After removing the lid of a bottle containing chlorine gas, the gas comes out and forms a mixture of air-chlorine gas inside the room.

03

Explanation for part (b)

The reverse process can never happen because, according to the second law of thermodynamics, the universe's entropy increases when an incident happens. However, in the reverse process, the entropy should decrease, but that cannot happen. Hence, the reverse process is not possible.

04

Explanation for part (c)

Two other examples of this can be if you break a plastic scale, it cannot be restored to its original shape, and if you open the lid of a perfume bottle, it cannot be reversed.

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Most popular questions from this chapter

A particular car does work at the rate of about\({\bf{7}}{\bf{.0}}\;{\bf{kJ/s}}\)when traveling at a steady\({\bf{21}}{\bf{.8}}\;{\bf{m/s}}\)along a level road. This is the work done against friction. The car can travel 17 km on 1.0 L of gasoline at this speed (about 40 mi/gal). What is the minimum value for\({{\bf{T}}_{\bf{H}}}\)if\({{\bf{T}}_{\bf{L}}}\)is 25掳C? The energy available from 1.0 L of gas is\({\bf{3}}{\bf{.2 \times 1}}{{\bf{0}}{\bf{7}}}\;{\bf{J}}\).

Question: (I) What is the change in entropy of 320 g of steam at 100掳C when it is condensed to water at 100掳C?

A 鈥淐arnot鈥� refrigerator (the reverse of a Carnot engine) absorbs heat from the freezer compartment at a temperature of -17掳C and exhausts it into the room at 25掳C.

(a) How much work would the refrigerator do to change 0.65 kg of water at 25掳C into ice at -17掳C.

(b) If the compressor output is 105 W and runs 25% of the time, how long will this take?

Question: (III) The PV diagram in Fig. 15鈥�23 shows two possible states of a system containing 1.75 moles of a monatomic ideal gas. \(\left( {{P_1} = {P_2} = {\bf{425}}\;{{\bf{N}} \mathord{\left/{\vphantom {{\bf{N}} {{{\bf{m}}^{\bf{2}}}}}} \right.} {{{\bf{m}}^{\bf{2}}}}},\;{V_1} = {\bf{2}}{\bf{.00}}\;{{\bf{m}}^{\bf{3}}},\;{V_2} = {\bf{8}}{\bf{.00}}\;{{\bf{m}}^{\bf{3}}}.} \right)\) (a) Draw the process which depicts an isobaric expansion from state 1 to state 2, and label this process A. (b) Find the work done by the gas and the change in internal energy of the gas in process A. (c) Draw the two-step process which depicts an isothermal expansion from state 1 to the volume \({V_2}\), followed by an isovolumetric increase in temperature to state 2, and label this process B. (d) Find the change in internal energy of the gas for the two-step process B.

Question: An ideal gas undergoes an isobaric compression and then an isovolumetric process that brings it back to its initial temperature. Had the gas undergone one isothermal process instead,

(a) the work done on the gas would be the same.

(b) the work done on the gas would be less.

(c) the work done on the gas would be greater.

(d) Need to know the temperature of the isothermal process.
See all solutions

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