Useful info 1 bar = 10° Pa 1 atm = 1.013bar R = 8.314 J/K-mol NA = 6.022x1023 mol = 8.206x10 L-atm/K-mol 3 = 8.206x10° m²-atm/K-mol 8 = 9.807 m/s? Pm[H2O] = 1.00 g/mL = 760 Torr = 62.36 L-Torr/K-mol 1 mbar = 10 bar 1J = 10² L-bar = 9.870×10³ L-atm= 0.2390 cal = 10² cm= 10° mm= 10° µm = 10° nm=101º A 1J = 1 Pa-m³ 1 L-atm = 101.3 J 1 m³ = 10³ L = 106 cm³ At 298 K (only): %3D RT = 2.478 kJ/mol (= 24.46 L-atm/mol) Physical Properties of Selected Substances mol. wt. ΔΗ Sm J/(mol·K) J/(mol·K) Cp,m AHus melting temp AHap boiling temp kJ/mol g/mol 39.9 kJ/mol K kJ/mol K 154.84 Ar(g) C(s,grpht.) CH;OH(1) CH;OH(g) CH4(g) CO(g) CO,(g) H,(g) H,O(1) H,O(g) NH;(g) O2(g) Properties of pure phases are for standard conditions of 298 K and 1 atm. Phase transition enthalpies are valid at the indicated phase transition temperature, at 1 atm. 20.786 12.01 8.53 32.04 -238.66 81.6 3.16 175.2 35.29 337.2 32.04 -200.66 43.9 16.04 -74.8 35.3 0.94 91 8.2 112 28.0 -110.53 29.14 44.0 -393.5 213.74 37.11 2.0 116.1 28.8 18.0 -285.8 69.9 75.3 6.0 273 40.6 373 18.0 -241.8 188.8 33.6 18.0 -46.1 192.4 35.1 5.7 195 23.3 240 32.0 205.1 29.4 Integrals Equations of state xn+1 x" dx ;n + -1 RT a ; van der Waals V2 n + 1 Vm In x В RT 1 + Vm + ... ; virial Vm 1 dx 1 - In (аx — b) ax a Nomenclature – but, when in doubt, write it out! AH Change in enthalpy for an arbitrary process (units of energy) AHm Change in enthalpy for an arbitrary process, per mole (energy/mole) AH, or AHn Standard molar enthalpy of reaction, per mole, between separated products and reactants, each in the standard states for the phases specified and at the specified temperature. (energy/mole) rxn 10

Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
icon
Related questions
icon
Concept explainers
Question

The oxidation of carbon monoxide is important in reducing ground-level pollution from cars:

CO(g) + 1/2 O2 (g) −−→ CO2 (g)                                   (1)

Use the information you have available to answer the following questions.

3a. What is the molar enthalpy of reaction (∆H◦ rxn) for Equation 1 at a temperature of 298 K? 

3b. This reaction is typically run using a catalyst at elevated temperature. What is the value of ∆H◦ rxn for Equation 1 at a temperature of 700 K?

3c. Give the molar internal energy of reaction (∆U ◦ rxn) at 700 K for Equation 1

Useful info
1 bar = 10° Pa
1 atm = 1.013bar
R = 8.314 J/K-mol
NA
= 6.022x1023 mol
= 8.206x10 L-atm/K-mol
3
= 8.206x10° m²-atm/K-mol
8 = 9.807 m/s?
Pm[H2O] = 1.00 g/mL
= 760 Torr
= 62.36 L-Torr/K-mol
1 mbar = 10 bar
1J = 10² L-bar = 9.870×10³ L-atm= 0.2390 cal
= 10² cm= 10° mm= 10° µm = 10° nm=101º A
1J = 1 Pa-m³ 1 L-atm = 101.3 J
1 m³ = 10³ L = 106 cm³
At 298 K (only):
%3D
RT = 2.478 kJ/mol (= 24.46 L-atm/mol)
Physical Properties of Selected Substances
mol. wt.
ΔΗ
Sm
J/(mol·K) J/(mol·K)
Cp,m
AHus melting temp
AHap boiling temp
kJ/mol
g/mol
39.9
kJ/mol
K
kJ/mol
K
154.84
Ar(g)
C(s,grpht.)
CH;OH(1)
CH;OH(g)
CH4(g)
CO(g)
CO,(g)
H,(g)
H,O(1)
H,O(g)
NH;(g)
O2(g)
Properties of pure phases are for standard conditions of 298 K and 1 atm.
Phase transition enthalpies are valid at the indicated phase transition temperature, at 1 atm.
20.786
12.01
8.53
32.04
-238.66
81.6
3.16
175.2
35.29
337.2
32.04
-200.66
43.9
16.04
-74.8
35.3
0.94
91
8.2
112
28.0
-110.53
29.14
44.0
-393.5
213.74
37.11
2.0
116.1
28.8
18.0
-285.8
69.9
75.3
6.0
273
40.6
373
18.0
-241.8
188.8
33.6
18.0
-46.1
192.4
35.1
5.7
195
23.3
240
32.0
205.1
29.4
Integrals
Equations of state
xn+1
x" dx
;n + -1
RT
a
; van der Waals
V2
n + 1
Vm
In x
В
RT
1 +
Vm
+ ...
; virial
Vm
1
dx
1
- In (аx — b)
ax
a
Nomenclature – but, when in doubt, write it out!
AH Change in enthalpy for an arbitrary process (units of energy)
AHm Change in enthalpy for an arbitrary process, per mole (energy/mole)
AH, or AHn Standard molar enthalpy of reaction, per mole, between separated products and reactants, each in the
standard states for the phases specified and at the specified temperature. (energy/mole)
rxn
10
Transcribed Image Text:Useful info 1 bar = 10° Pa 1 atm = 1.013bar R = 8.314 J/K-mol NA = 6.022x1023 mol = 8.206x10 L-atm/K-mol 3 = 8.206x10° m²-atm/K-mol 8 = 9.807 m/s? Pm[H2O] = 1.00 g/mL = 760 Torr = 62.36 L-Torr/K-mol 1 mbar = 10 bar 1J = 10² L-bar = 9.870×10³ L-atm= 0.2390 cal = 10² cm= 10° mm= 10° µm = 10° nm=101º A 1J = 1 Pa-m³ 1 L-atm = 101.3 J 1 m³ = 10³ L = 106 cm³ At 298 K (only): %3D RT = 2.478 kJ/mol (= 24.46 L-atm/mol) Physical Properties of Selected Substances mol. wt. ΔΗ Sm J/(mol·K) J/(mol·K) Cp,m AHus melting temp AHap boiling temp kJ/mol g/mol 39.9 kJ/mol K kJ/mol K 154.84 Ar(g) C(s,grpht.) CH;OH(1) CH;OH(g) CH4(g) CO(g) CO,(g) H,(g) H,O(1) H,O(g) NH;(g) O2(g) Properties of pure phases are for standard conditions of 298 K and 1 atm. Phase transition enthalpies are valid at the indicated phase transition temperature, at 1 atm. 20.786 12.01 8.53 32.04 -238.66 81.6 3.16 175.2 35.29 337.2 32.04 -200.66 43.9 16.04 -74.8 35.3 0.94 91 8.2 112 28.0 -110.53 29.14 44.0 -393.5 213.74 37.11 2.0 116.1 28.8 18.0 -285.8 69.9 75.3 6.0 273 40.6 373 18.0 -241.8 188.8 33.6 18.0 -46.1 192.4 35.1 5.7 195 23.3 240 32.0 205.1 29.4 Integrals Equations of state xn+1 x" dx ;n + -1 RT a ; van der Waals V2 n + 1 Vm In x В RT 1 + Vm + ... ; virial Vm 1 dx 1 - In (аx — b) ax a Nomenclature – but, when in doubt, write it out! AH Change in enthalpy for an arbitrary process (units of energy) AHm Change in enthalpy for an arbitrary process, per mole (energy/mole) AH, or AHn Standard molar enthalpy of reaction, per mole, between separated products and reactants, each in the standard states for the phases specified and at the specified temperature. (energy/mole) rxn 10
Expert Solution
trending now

Trending now

This is a popular solution!

steps

Step by step

Solved in 3 steps

Blurred answer
Knowledge Booster
Thermochemistry
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.
Similar questions
  • SEE MORE QUESTIONS
Recommended textbooks for you
Chemistry
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Organic Chemistry
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Elementary Principles of Chemical Processes, Bind…
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY