Consider 1.00 mole of an ideal gas that is expanded isothermally at 25°C from
Step 1: from
Step 2: from
Step 3: from
Calculate q, w,
Interpretation : The value of
Concept Introduction :
Work done can be calculated as follows:
The internal energy is sum of heat and work.
The change in entropy is calculated as follows:
Also, change in Gibbs free energy is related to change in enthalpy and entropy as follows:
w − work done
P − pressure
V − volume
n − number of moles
R − universal gas constant
T − temperature
ΔE − energy change
q − heat
ΔS − entropy change
ΔG − Gibbs free energy change
ΔH − enthalpy change
Answer to Problem 147CP
q | w | ΔE | ΔS | ΔH | ΔG | |
Step 1 | 1480 J | -1480 J | 0 | 7.56 J/K | 0 | -2250 J |
Step 2 | 1240 J | -1240 J | 0 | 5.77 J/K | 0 | -1720 J |
Step 3 | 1246 J | -1246 J | 0 | 5.81 J/K | 0 | -1730 J |
Total | 3966 J | -3966 J | 0 | 19.14 J/K | 0 | -5700 J |
Explanation of Solution
Given information :
1.00 mole of an ideal gas is isothermally expanded at 25 0C as follows.
Step 1:
Step 2:
Step 3:
Step 1:
Step 2:
Step 3:
q | w | ΔE | ΔS | ΔH | ΔG | |
Step 1 | 1480 J | -1480 J | 0 | 7.56 J/K | 0 | -2250 J |
Step 2 | 1240 J | -1240 J | 0 | 5.77 J/K | 0 | -1720 J |
Step 3 | 1246 J | -1246 J | 0 | 5.81 J/K | 0 | -1730 J |
Total | 3966 J | -3966 J | 0 | 19.14 J/K | 0 | -5700 J |
Thus,
q | w | ΔE | ΔS | ΔH | ΔG | |
Step 1 | 1480 J | -1480 J | 0 | 7.56 J/K | 0 | -2250 J |
Step 2 | 1240 J | -1240 J | 0 | 5.77 J/K | 0 | -1720 J |
Step 3 | 1246 J | -1246 J | 0 | 5.81 J/K | 0 | -1730 J |
Total | 3966 J | -3966 J | 0 | 19.14 J/K | 0 | -5700 J |
Want to see more full solutions like this?
Chapter 10 Solutions
Chemical Principles
- Calculate H when a 38-g sample of glucose, C6H12O6(s), burns in excess O2(g) to form CO2(g) and H2O() in a reaction at constant pressure and 298.15 K.arrow_forwardWhen vapors from hydrochloric acid and aqueous ammonia come in contact, they react, producing a white cloud of solid NH4C1 (Figure 18.9). HCI(g) + NH3(g) NH4Cl(s) Defining the reactants and products as the system under study: (a) Predict whether S(system), S(surroundings), S(universe), rH, and rG (at 298 K) are greater than zero, equal to zero, or less than zero; and explain your prediction. Verify your predictions by calculating values for each of these quantities. (b) Calculate the value of Kp for this reaction at 298 K.arrow_forward2. In which of the following reactions is there a significant transfer of energy as work from the system to the surroundings? This occurs if there is a change in the number of moles of gases. C(s) + O2(g) → CO2(g) CH4(g) + 2 O2(g) → CO2g) + 2 H2O(g) 2 C(s) + O2(g) → 2 CO(g) 2 Mg(s) + O2(g) → 2 MgO(s)arrow_forward
- What is the change in internal energy when a gas contracts from 377mL to 119mLundera pressure of 1550 torr, whileat the same time being cooled by removing 124.0J ofheat energy?arrow_forwardSuppose that you are studying kinetic energy of helium molecules: A helium weather balloon rises to an altitude of 40,000 ft; the temperature of the gas drops to 70 F. (a) Make an appropriate choice of system and surroundings and describe it unambiguously. (b) Explain why you chose the system and surroundings you did. (c) Identify transfers of energy and material into and out of the system that would be important for you to monitor in your study.arrow_forwardA volume of 1.50 L of argon gas is confined in a cylinder with a movable piston under a constant pressure of 1.22 105 Pa. When 1.25 kJ of energy in the form of heat is transferred from the surroundings to the gas, the internal energy of the gas increases by 1.11 kJ. What is the final volume of argon gas in the cylinder?arrow_forward
- Consider a mixture of air and gasoline vapor in a cylinder with a piston. The original volume is 40. cm3. If the combustion of this mixture releases 950. J of energy, to what volume will the gases expand against a constant pressure of 650. torr if all the energy of combustion is converted into work to push back the piston?arrow_forwardAn industrial process for manufacturing sulfuric acid, H2SO4, uses hydrogen sulfide, H2S, from the purification of natural gas. In the first step of this process, the hydrogen sulfide is burned to obtain sulfur dioxide, SO2. 2H2S(g)+3O2(g)2H2O(l)+2SO2(g);H=1124kJ The density of sulfur dioxide at 25C and 1.00 atm is 2.62 g/L, and the molar heat capacity is 30.2 J/(mol C). (a) How much heat would be evolved in producing 1.00 L of SO2 at 25C and 1.00 atm? (b) Suppose heat from this reaction is used to heat 1.00 L of the SO2 from 25C to 500C for its use in the next step of the process. What percentage of the heat evolved is required for this?arrow_forwardH₂(g) + I₂(g) → 2HI(g) AH = +52kJ 33. A colorless hydrogen gas is mixed with purple iodine vapor in a sealed flask. The chemical reaction produced a colorless hydrogen iodide as shown in the equation above. What can be done to temperature, concentration and pressure of any of the chemicals in the mixture to increase the formation of purple vapor? (B) (A) Decrease temperature and H₂ concentration, same pressure Decrease temperature and I₂ concentration, same pressure (C) Increase temperature and I₂ concentration, decrease pressure Increase the temperature, HI concentration, and pressure (D)arrow_forward
- Suppose you place 0.0400 g of magnesium chips in a coffee-cup calorimeter and then add 100.0 mL of 1.00 M HCl. The reaction that occurs is Mg(s) + 2 HCl(aq) → H2(g) + MgCl2(aq) The temperature of the solution increases from 21.66 °C (294.81 K) to 23.46 °C (296.61 K). What is the enthalpy change for the reaction per mole of Mg? Assume a specific heat capacity of the solution is 4.20 J/g∙K and the density of the HCl solution is 1.00 g/mL. kJ/molarrow_forwardSuppose you place 0.0300 g of magnesium chips in a coffee-cup calorimeter and then add 100.0 mL of 1.00 M HCl. The reaction that occurs is Mg(s) + 2 HCl(aq) → H2(g) + MgCl2(aq) The temperature of the solution increases from 23.49 °C (296.64 K) to 24.84 °C (297.99 K). What is the enthalpy change for the reaction per mole of Mg? Assume a specific heat capacity of the solution is 4.20 J/g∙K and the density of the HCl solution is 1.00 g/mLarrow_forwardThe enthalpy of vaporization of chlorine at the standard (1 atm) boiling point (284 K) is 20.41 kJ/mol. What is the change in internal energy when one mole of chlorine vaporizes under those conditions?arrow_forward
- ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage Learning
- Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage LearningChemistry for Engineering StudentsChemistryISBN:9781337398909Author:Lawrence S. Brown, Tom HolmePublisher:Cengage LearningChemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage Learning