Chemistry for Engineering Students
4th Edition
ISBN: 9781337398909
Author: Lawrence S. Brown, Tom Holme
Publisher: Cengage Learning
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Chapter 10, Problem 10.63PAE
During
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1. Polymerization reactions are complicated somewhat because they involve very large numbers
of molecules. But we can demonstrate the general features of the thermodynamics of
polymerization by considering a much smaller model system. Instead of considering the
formation of polyethylene, for example, we can begin with the following reaction in which two
ethylene molecules combine with hydrogen to form butane:
2 C2H4 + H2g → GH10)
Use the table below to calculate ASº.
Compound
(J mol" K')
Compound
U mol" K')
130.6
CO:(g)
213.6
O:(g)
205.0
C,H(g)
310.03
II,O()
CI L(g)
69.91
186.2
I1,0(g)
188.7
CIL(E)
219.5
NH(g)
1923
C,H,N(O
178.91
When ethene is mixed with hydrogen in the presence of a platinum catalyst, hydrogen adds across the double bond to form ethane. At room temperature, the reaction goes to completion. Predict the signs of ∆H° and ∆S° for this reaction. Explain these signs in terms of bonding and freedom of motion.
Substance
C₂Hg(g)
O₂(g)
CO₂(g)
H₂O(g)
The thermodynamic data calculated above for this reaction
C3Hg(g) + 5 O₂(g)
AH (kJ/mol)
-104.70
0.0
-393.51
-241.8
A,G=
AH-2043.0 kJ mol¹ and A,S 100.62 J K mol
3 CO₂(g) + 4H₂O(g)
kJ mol-1
Calculate A,G in kJ mol¹ if the reaction mixture is at 146°C. (You have 2 attempts until the answer will be given; you have already tried 0 times)
S (J/mol/K)
270.30
205.1
213.74
188.8
Chapter 10 Solutions
Chemistry for Engineering Students
Ch. 10 - Prob. 1COCh. 10 - . explain the concept of entropy in your own...Ch. 10 - Prob. 3COCh. 10 - . state the second law of thermodynamics in words...Ch. 10 - Prob. 5COCh. 10 - Prob. 6COCh. 10 - Prob. 7COCh. 10 - Prob. 8COCh. 10 - Prob. 9COCh. 10 - Prob. 10CO
Ch. 10 - Prob. 10.1PAECh. 10 - Prob. 10.2PAECh. 10 - Prob. 10.3PAECh. 10 - Prob. 10.4PAECh. 10 - Prob. 10.5PAECh. 10 - Use the web to learn how many pounds of plastics...Ch. 10 - On the basis of your experience, predict which of...Ch. 10 - In the thermodynamic definition of a spontaneous...Ch. 10 - 1f the combustion of butane is spontaneous, how...Ch. 10 - Identify each of the processes listed as...Ch. 10 - Identify each of the processes listed as...Ch. 10 - Athletic trainers use instant ice packs that can...Ch. 10 - Are any of the following exothermic processes not...Ch. 10 - Enthalpy changes often help predict whether or not...Ch. 10 - When a fossil fuel burns, is that fossil fuel the...Ch. 10 - Murphy's law is a whimsical rule that says that...Ch. 10 - Prob. 10.17PAECh. 10 - Some games include dice with more than six sides....Ch. 10 - How does probability relate to spontaneity?Ch. 10 - Prob. 10.20PAECh. 10 - For each pair of items, tell which has the higher...Ch. 10 - For each process, tell whether the entropy change...Ch. 10 - Without doing a calculation, predict whether the...Ch. 10 - For the following chemical reactions, predict the...Ch. 10 - What happens to the entropy of the universe during...Ch. 10 - Prob. 10.26PAECh. 10 - One statement of the second law of thermodynamics...Ch. 10 - Prob. 10.28PAECh. 10 - Prob. 10.29PAECh. 10 - Which reaction occurs with the greater increase in...Ch. 10 - Which reaction occurs with the greater increase in...Ch. 10 - Methanol is burned as fuel in some race cars. This...Ch. 10 - Limestone is predominantly CaCO3, which can...Ch. 10 - Suppose that you find out that a system has an...Ch. 10 - Use tabulated thermodynamic data to calculate the...Ch. 10 - Prob. 10.36PAECh. 10 - Calculate S for the dissolution of magnesium...Ch. 10 - Calculate the standard entropy change for the...Ch. 10 - Through photosynthesis, plants build molecules of...Ch. 10 - Find websites describing two different attempts to...Ch. 10 - Prob. 10.41PAECh. 10 - Prob. 10.42PAECh. 10 - Under what conditions does G allow us to predict...Ch. 10 - There is another free energy state function, the...Ch. 10 - 10.45 Calculate G at 45°C for reactions for which...Ch. 10 - 10.46 Discuss the effect of temperature change on...Ch. 10 - The reaction CO2(g)+H2(g)CO(g)+H2O(g) is not...Ch. 10 - Prob. 10.48PAECh. 10 - Prob. 10.49PAECh. 10 - For the reaction NO(g)+NO2(g)N2O3(g) , use...Ch. 10 - 10.51 The combustion of acetylene was used in...Ch. 10 - Natural gas (methane) is being used in...Ch. 10 - Silicon forms a series of compounds analogous to...Ch. 10 - Explain why Gf of O2 (g) is zero.Ch. 10 - Using tabulated thermodynamic data, calculate G...Ch. 10 - Using tabulated thermodynamic data, calculate G...Ch. 10 - Calculate G for the dissolution of both sodium...Ch. 10 - Phosphorus exists in multiple solid phases,...Ch. 10 - 10.59 The normal melting point of benzene, C6H6,...Ch. 10 - Prob. 10.60PAECh. 10 - Estimate the temperature range over which each of...Ch. 10 - Recall that incomplete combustion of fossil fuels...Ch. 10 - During polymerization, the system usually becomes...Ch. 10 - Prob. 10.64PAECh. 10 - Prob. 10.65PAECh. 10 - The recycling of polymers represents only one...Ch. 10 - Prob. 10.67PAECh. 10 - When ice melts, its volume decreases. Despite this...Ch. 10 - 10.69 If a sample of air were separated into...Ch. 10 - Prob. 10.70PAECh. 10 - An explosion brings down an old building, leaving...Ch. 10 - Prob. 10.72PAECh. 10 - Prob. 10.73PAECh. 10 - Prob. 10.74PAECh. 10 - Prob. 10.75PAECh. 10 - Some say that the job of an engineer is to fight...Ch. 10 - A beaker of water at 40C (on the left in the...Ch. 10 - Why is it usually easier to use G to determine the...Ch. 10 - The molecular scale pictures below show snapshots...Ch. 10 - Prob. 10.80PAECh. 10 - Diethyl ether is a liquid at normal temperature...Ch. 10 - Calculate the entropy change, S , for the...Ch. 10 - Gallium metal has a melting point of 29.8°C. Use...Ch. 10 - Methane can be produced from CO and H2.The process...Ch. 10 - 10.85 Iodine is not very soluble in water, but it...Ch. 10 - The enthalpy of vaporization for water is 40.65 kJ...Ch. 10 - Determine whether each of the following statements...Ch. 10 - Nickel metal reacts with carbon monoxide to form...Ch. 10 - Polyethylene has a heat capacity of 2,3027 J g-1...Ch. 10 - A key component in many chemical engineering...Ch. 10 - The reaction shown below is involved in the...Ch. 10 - Using only the data given below, determine G for...Ch. 10 - The graph below shows G as a function of...Ch. 10 - Prob. 10.94PAECh. 10 - Prob. 10.95PAECh. 10 - Prob. 10.96PAECh. 10 - Prob. 10.97PAECh. 10 - Prob. 10.98PAECh. 10 - Thermodynamics provides a way to interpret...Ch. 10 - Prob. 10.100PAECh. 10 - 10.101 Fluorine reacts with liquid water to form...Ch. 10 - 10.102 Ammonia can react with oxygen gas to form...Ch. 10 - Prob. 10.103PAECh. 10 - 10.104 (a) When a chemical bond forms, what...
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- Compound ∆Hf (kJ/mole) ∆S (J/mole K) CO2(g) –393.5 +213.8 CO2 (aq) –413.8 +117.6 N2O4 9.16 +304.4 NO2 33.2 240.1 CaCO3 –1207.6 91.7 CaO –634.9 +38.1 I2 (g) 62.42 260.69 HI(g) 26.5 206.6 H2 (g) 0 130.7 (a) For the following reactions, using the provided ∆H and ∆S data, determine whether each one would be spontaneous or nonspontaneous at 25°C CO2(g) à CO2(aq) N2O4(g)-------- à2 NO2(g) CaCO3(s) ----à CaO (s) + CO2(g) H2 (g) + I2(g)---- à 2 HI (g)arrow_forwardUsing thermodynamic data, estimate the normal boiling point of methanol. (Recall that liquid and vapor are in equilibrium at 1.0 atm pressure at the normal boiling point.) The actual normal boiling point of methanol is 64.7 °C. Compound A,H° (kJ/mol) s* (J/mol · K) CH3OH(2) -238.4 127.19 CH3OH(g) -201.0 239.7 Normal boiling point = °Carrow_forwardWhen a native protein in solution is heated to a high enough temperature, its polypeptide chain will unfold to become the denatured protein. The temperature at which a large portion of the protein unfolds is called the melting temperature. The melting temperature of a certain protein is found to be 47°C, and the enthalpy of denaturation is 3.80 × 102 kJ/mol. Assume that the denaturation is a two-state process; that is, native protein → denatured protein The single protein chain has 123 amino acids. Calculate the entropy of denaturation per amino acid.arrow_forward
- Given the following thermodynamic data: CO2(g) + 2NH3(g) → CO(NH2)2(s) + H2O(l) ΔH°298 =-133.3 kJ ΔG°298 =-6.97 kJ ΔH°f (kJ/mol) -393.5 -46.11 -285.8 S° (J/mol K) 213.6 192.3 104.6 69.91 a) Determine ΔH⁰f for CO(NH2)2(s) b) Determine K for the reaction at 298 K c) Determine ΔS⁰ for the reaction in units of J/K d) Determine ΔG if the pressure of CO2 is 0.450 bar and the pressure of NH3 is 0.650 bar e) Determine K for the reaction at 250 Karrow_forwardUsing the table of thermodynamic data provided, for the reaction below: CS₂(1) + 302(g) → CO2(g) + 2SO2(g) Compound CO₂(g) CS₂(1) O₂(g) SO₂(g) SO₂(g) AHºf (kJ/mol) -393.5 89.0 0 -296.8 -395.7 S°(J/K mol) 213.8 151.3 205.15 248.2 256.8 Determine/calculate and report the following values in the labelled boxes below: a) The standard enthalpy change (AH°, in kJ/mol) of the reaction. b) The standard entropy change (AS°, in J/K mol) of the reaction. c) The standard free energy change (AG°, in kJ/mol) of the reaction. d) The free energy change (AG, in kJ/mol) of the reaction at 7.50 x 10² K.arrow_forward1. What is the importance of heat of reaction in the laboratory? 2. Cite some factors that could possibly affect the ∆H in the experiment of heat of reaction.arrow_forward
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- Use the following equations to calculate the heat of the reaction for the synthesis of diborane. 2B(s) + 3/2 O2(g) → B2O3(s) ∆ Ho = -1273 kJ B2H6(g) + 3 O2(g) → B2O3(s) + 3H2O(g) ∆ Ho = -2035 kJ H2(g) + 1/2 O2(g) → H2O(l) ∆ Ho = -286 kJ H2O (l) → H2O (g) Δ Ho = 44 kJ Calculate ∆Ho for the following reaction:2B(s) + 3H2(g) → B2H6(g)arrow_forwardArguably one of the most fundamental concepts in physical science is that of the second law of thermodynamics. Summarize the second law and make sure to include the two key aspects of the second law.arrow_forwardWhat is a driving force? Name two common and important driving forces, and give an example of each. What is entropy? Although the total energy of the universe is constant, is the entropy of the universe constant? What is a spontaneous process?arrow_forward
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