PHYSICAL CHEMISTRY-STUDENT SOLN.MAN.
2nd Edition
ISBN: 9781285074788
Author: Ball
Publisher: CENGAGE L
expand_more
expand_more
format_list_bulleted
Videos
Textbook Question
Chapter 3, Problem 3.33E
Dentists might use a mixture of
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solution
Students have asked these similar questions
Give correct detailed Solution
b) Determine the standard enthalpy change and std. Gibbs free energy change of D
reaction at 400 k for the reaction
CO(g) +2H2(g) → CH;OH (g)
At 298.15 K, AH CO (9)= -26.41 kcal/mol, AH.CH,0H(9)= -48.08 kcal/mol,
(9)= -32.8079 kcal/mol, AG CH30H(g)= -38.69 kcal/mol,
The standard heat capacity of various components is given by,
C = a + bT + cT2 + dT³, where C is in cal/mol-K and T is in K
b x10²
c x105
d x10º
Сomponent
CH3OH
a
4.55
2.186
-0.291
-1.92
CO
6.726
0.04
0.1283
-0.5307
H2
6.952
-0.0457
0.09563
-0.2079
4) a) A reaction chamber is divided into two sections by a partition on which a valve is
inserted. One section contains pure gas A and the other section has a mixture of gases A and
B. What happens when the valve is opened? Explain this process in terms of chemical
potential.
b) The decomposition of etane into etene and hydrogen takes places at 1000 K and under 1
bar total pressure.
C,H6(g) → C2H48) + H2«g)
The composition of the mixture at equilibrium is as follows :
H2(g): 32, C2H4(g): 32, and C,H6(g):36 (mol, %).
According to the data;
Calculate K, at 1000K
Calculate Kp at 298.15 K, AH° = 145 kJ/mol
Calculate AG° at 298.15 K
Chapter 3 Solutions
PHYSICAL CHEMISTRY-STUDENT SOLN.MAN.
Ch. 3 - Decide whether the following processes will be...Ch. 3 - Try to find one additional example of a...Ch. 3 - Consider the following quantities for a...Ch. 3 - Consider the following quantities for a four-step...Ch. 3 - What is the temperature of the low-temperature...Ch. 3 - What is the temperature of the high - temperature...Ch. 3 - Prob. 3.7ECh. 3 - Explain why the high-temperature reservoir of a...Ch. 3 - Superheated steam is steam with a temperature...Ch. 3 - Prob. 3.10E
Ch. 3 - The Carnot cycle is defined as having a certain...Ch. 3 - In thermodynamics, the pathway in a...Ch. 3 - A refrigerator is the reverse of an engine: Work...Ch. 3 - Efficiency is given by equations 3.5, 3.6, and...Ch. 3 - What is the entropy change for an ideal Carnot...Ch. 3 - What is the entropy change for the melting of...Ch. 3 - What is the entropy change for the solidification...Ch. 3 - Explain why the statement No process is 100...Ch. 3 - What is the change in entropy of 1.00mole of water...Ch. 3 - Prob. 3.20ECh. 3 - One mole of He warms up irreversibly at constant...Ch. 3 - Consider a monatomic ideal gas in a piston...Ch. 3 - A 0.500-mol sample of an ideal gas has an initial...Ch. 3 - SO2 in a piston chamber kept in a...Ch. 3 - A normal breath has a volume of about 1L. The...Ch. 3 - An automobile tire contains 15.6L of air at...Ch. 3 - An automobile tire contains 15.6L of air at...Ch. 3 - A sample of ideal gas from a compressed gas...Ch. 3 - Prob. 3.29ECh. 3 - In Example 3.5, a heat capacity of 20.78J/molK was...Ch. 3 - Prob. 3.31ECh. 3 - 4.00L of Ar and 2.50L of He, each at 298K and...Ch. 3 - Dentists might use a mixture of 40N2O and 60O2 as...Ch. 3 - A 5.33-g piece of Cu metal is heated to 99.7C in...Ch. 3 - A sample of 1.00mol of silver at 150C is placed in...Ch. 3 - Prob. 3.36ECh. 3 - What is the change in entropy when 2.22mol of...Ch. 3 - Estimate the entropy change of an 800-lb engine...Ch. 3 - Calculate the molar entropy change of the gas that...Ch. 3 - A normal breath is about 1L in volume. Assume you...Ch. 3 - The first law of thermodynamics is sometimes...Ch. 3 - Troutons rule states that the entropy of boiling...Ch. 3 - Prob. 3.43ECh. 3 - Argue from Boltzmanns definition for entropy that...Ch. 3 - Prob. 3.45ECh. 3 - Which system has the higher entropy? a A clean...Ch. 3 - Which system has the higher entropy? a 1g of solid...Ch. 3 - The absolute entropy of He at 298.15K is...Ch. 3 - The absolute entropy of Kr at 298.15K is...Ch. 3 - The element helium is thought to remain a liquid...Ch. 3 - Order the following substances in order of...Ch. 3 - The molar entropy change for a process is...Ch. 3 - What is the entropy change of a process if ...Ch. 3 - One mole of ideal gas expands isothermally and...Ch. 3 - Why isnt the entropy of elements in their standard...Ch. 3 - Determine the entropy of formation, fS, of the...Ch. 3 - The thermite reaction has solid aluminum powder...Ch. 3 - Prob. 3.58ECh. 3 - Determine the differences in the rxnS under...Ch. 3 - Calcium carbonate has two crystalline forms,...Ch. 3 - The chemical formula for gasoline can be...Ch. 3 - Prob. 3.62ECh. 3 - Prob. 3.63ECh. 3 - Plants take in CO2(g) and H2O(l) and make glucose,...Ch. 3 - Prob. 3.65ECh. 3 - Prob. 3.66ECh. 3 - Plots of Cp/T versus T are used to determine the...
Knowledge Booster
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
- Another step in the metabolism of glucose, which occurs after the formation of glucose6-phosphate, is the conversion of fructose6-phosphate to fructose1,6-bisphosphate(bis meanstwo): Fructose6-phosphate(aq) + H2PO4(aq) fructose l,6-bisphosphate(aq) + H2O() + H+(aq) (a) This reaction has a Gibbs free energy change of +16.7 kJ/mol of fructose6-phosphate. Is it endergonic or exergonic? (b) Write the equation for the formation of 1 mol ADP fromATR for which rG = 30.5 kJ/mol. (c) Couple these two reactions to get an exergonic process;write its overall chemical equation, and calculate theGibbs free energy change.arrow_forwardUse the appropriate tables to calculate H for (a) the reaction between copper(II) oxide and carbon monoxide to give copper metal and carbon dioxide. (b) the decomposition of one mole of methyl alcohol (CH3OH) to methane and oxygen gases.arrow_forwardb) Determine the standard enthalpy change and std. Gibbs free energy change of reaction at 400 k for the reaction СO(g) +2H2(g) — CHОН (g) At 298.15 K, AH.co (0)= -26.41 kcal/mol, AH AG.co (9)= -32.8079 kcal/mol, AG cH,oh(9)= -38.69 kcal/mol, °.CH20H(9)= -48.08 kcal/mol, The standard heat capacity of various components is given by, CO = a + bT + cT² + dT³, where C, is in cal/mol-K and T is in K b x10² с х105 d x10° Соmponent CH3OH а 4.55 2.186 -0.291 -1.92 CO 6.726 0.04 0.1283 -0.5307 H2 6.952 -0.0457 0.09563 -0.2079arrow_forward
- X(9) + 4Y(9) = 3Z(g) K, = 3.12 x 10 2 bar 2 at a temperature of 287 °C. Calculate the value of Ke.arrow_forwardCalculate the value of the equilibrium constant, Ke, for the reaction Q(g) + X(g) 2 M(g) + N(g) given that Ke = M(g) = Z(g) 6R(g) = 2N(g) + 4 Z(g) 3 X(g) + 3 Q(g) = 9R(g) .116 Kel = 3.57 Kc2 = 0.524 Kc3 = 14.6arrow_forwardConsider the natural environment of CO2. What is the difference between an open and closed system for Carbon dioxide. What is constant in an open system and what is constant in a closed system and the laws that govern these constant values. create a sketch of the carbonate system on an open and closed system.arrow_forward
- Provide the formal definition of enthalpy and explain all symbols used in it. Explain how the change in enthalpy is related to certain thermodynamic property (other than Gibbs energy).arrow_forwardThe equilibrium constant for the reaction, 3 H2(g) + N2(g)= 2NH3(g), at a given temperature is 1.4 x 10–7. Calculate the equilibrium concentration of ammonia, if [H2] = 1.2 x 10–2 mol L–1 and [N2] = 3.2 x 10–3 mol L–1.arrow_forwardDetermine the standard enthalpy change and std. Gibbs free energy change of reaction at 400 k for the reaction CO(g) +2H2(g) → CH3OH (g) At 298.15 K, ∆Hf,CO (g) 0 = -26.41 kcal/mol, ∆Hf,CH3OH(g) 0 = -48.08 kcal/mol, ∆Gf,CO (g)0 = -32.8079 kcal/mol, ∆Gf,CH3OH(g) 0 = -38.69 kcal/mol,The standard heat capacity of various components is given by,Cp0 = a + bT + cT2 + dT3, where Cp0is in cal/mol-K and T is in KComponent a b ×102 c ×105 d ×109CH3OH 4.55 2.186 -0.291 -1.92CO 6.726 0.04 0.1283 -0.5307H2 6.952 -0.0457 0.09563 -0.2079arrow_forward
- Establish the relation between K and Kc for the reaction H2CO(g) ⇋ CO(g) + H2(g).arrow_forwardA geochemist in the field takes a 9.0 mL sample of water from a rock pool lined with crystals of a certain mineral compound X. He notes the temperature of the pool, 15. C, and caps the sample carefully. Back in the lab, the geochemist first dilutes the sample with distilled water to 400. mL.. Then he filters and evaporates all the water under vacuum. Crystals of X are left behind. The researcher washes, dries and weighs the crystals. They weigh 0.045 g. Using only the information above, can you calculate the solubility of Xin water at 15.° C7 If you said yes, calculate it. Be sure your answer has a unit symbol and 2 significant digits. yes O no 0 0.9 H ロ･ロ X 0 Garrow_forward2. Consider a closed vessel containing a mixture of ideal gases A and B that undergo the chemical reaction: A=bB, where b is an unknown stoichiometric coefficient. The equilibrium mole fraction xд is measured but xB is unknown. The equilibrium mole fraction xд increases when the temperature in the vessel is increased with the pressure held constant and Ꮖ Ꭺ decreases when the pressure in vessel is increased with the temperature held constant. Explain these observations in terms of inequalities involving the enthalpy of reaction AH and the stoichiometric coefficient b in Eq. (7).arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
Chemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage Learning
Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning
Chemistry: Principles and Reactions
Chemistry
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:Cengage Learning
Chemistry: The Molecular Science
Chemistry
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:Cengage Learning
The Laws of Thermodynamics, Entropy, and Gibbs Free Energy; Author: Professor Dave Explains;https://www.youtube.com/watch?v=8N1BxHgsoOw;License: Standard YouTube License, CC-BY