Chemistry & Chemical Reactivity
10th Edition
ISBN: 9781337399074
Author: John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher: Cengage Learning
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Chapter 18, Problem 107SCQ
Interpretation Introduction
Interpretation:
It should be predicted that the given statements are true or false.
Concept introduction:
A system is said to be stable when it is in the lowest energy state. A product can be thermodynamically stable or kinetically labile or both. In general, the product that have lowest activation energy is formed easily. However, the
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Chapter 18 Solutions
Chemistry & Chemical Reactivity
Ch. 18.3 - Predict which substance in each pair has the...Ch. 18.3 - Prob. 18.2CYUCh. 18.4 - Based on rH and rS, predict the spontaneity of the...Ch. 18.6 - Prob. 18.4CYUCh. 18.6 - Prob. 18.5CYUCh. 18.6 - Oxygen was first prepared by Joseph Priestley...Ch. 18.6 - Prob. 18.7CYUCh. 18.6 - Prob. 18.8CYUCh. 18.6 - Prob. 18.9CYUCh. 18.7 - Consider the hydrolysis reactions of creatine...
Ch. 18.7 - Prob. 1.2ACPCh. 18.7 - The decomposition of diamond to graphite...Ch. 18.7 - It has been demonstrated that buckminsterfullerene...Ch. 18 - Solid NH4NO3 is placed in a beaker containing...Ch. 18 - Acetic acid, a weak acid, was added to a beaker...Ch. 18 - Identify the following processes as either...Ch. 18 - Identify the following processes as either...Ch. 18 - Prob. 5PSCh. 18 - Predict whether each of the following processes...Ch. 18 - Indicate which of the following processes are...Ch. 18 - Prob. 8PSCh. 18 - Prob. 9PSCh. 18 - Prob. 10PSCh. 18 - Prob. 11PSCh. 18 - Calculate the entropy change that occurs when 1.00...Ch. 18 - Prob. 13PSCh. 18 - Calculate the change in entropy of a system with...Ch. 18 - The third law of thermodynamics says that a...Ch. 18 - Identify trends in S values: (a) For the halogens:...Ch. 18 - Which substance has the higher entropy? (a) dry...Ch. 18 - Which substance has the higher entropy? (a) a...Ch. 18 - Use S values to calculate the standard entropy...Ch. 18 - Use S values to calculate the standard entropy...Ch. 18 - Calculate the standard entropy change for the...Ch. 18 - Calculate the standard entropy change for the...Ch. 18 - Calculate the standard entropy change for the...Ch. 18 - Calculate the standard entropy change for the...Ch. 18 - Is the reaction Si(s) + 2 Cl2(g) SiCl4(g)...Ch. 18 - Is the reaction Si(s) + 2 H2(g) SiH4(g)...Ch. 18 - Calculate S(universe) for the decomposition of 1...Ch. 18 - Calculate S(universe) for the formation of 1 mol...Ch. 18 - Classify each of the reactions according to one of...Ch. 18 - Classify each of the reactions according to one of...Ch. 18 - Using values of fH and S, calculate rG for each of...Ch. 18 - Using values of fH and S, calculate rG for each of...Ch. 18 - Using values of fH and S, calculate the standard...Ch. 18 - Using values of fH and S, calculate the standard...Ch. 18 - Using values of fG, calculate rG for each of the...Ch. 18 - Using values of fG, calculate rG for each of the...Ch. 18 - For the reaction BaCO3(s) BaO(s) + CO2(g), rG =...Ch. 18 - For the reaction TiCl2(s) + Cl2(g) TiCl4(), rG =...Ch. 18 - Determine whether the reactions listed below are...Ch. 18 - Determine whether the reactions listed below are...Ch. 18 - Heating some metal carbonates, among them...Ch. 18 - Calculate rH and rS for the reaction of tin(IV)...Ch. 18 - The ionization constant, Ka, for acetic acid is...Ch. 18 - Prob. 44PSCh. 18 - The standard free energy change, rG, for the...Ch. 18 - Prob. 46PSCh. 18 - Calculate rG at 25 C for the formation of 1.00 mol...Ch. 18 - Prob. 48PSCh. 18 - Prob. 49PSCh. 18 - Prob. 50PSCh. 18 - Compare the compounds in each set below and decide...Ch. 18 - Using standard entropy values, calculate rS for...Ch. 18 - About 5 billion kilograms of benzene, C6H6, are...Ch. 18 - Hydrogenation, the addition of hydrogen to an...Ch. 18 - Is the combustion of ethane, C2H6, product-favored...Ch. 18 - Prob. 56GQCh. 18 - When vapors from hydrochloric acid and aqueous...Ch. 18 - Calculate S(system), S(surroundings), and...Ch. 18 - Methanol is now widely used as a fuel in race...Ch. 18 - The enthalpy of vaporization of liquid diethyl...Ch. 18 - Calculate the entropy change, rS, for the...Ch. 18 - Using thermodynamic data, estimate the normal...Ch. 18 - Prob. 63GQCh. 18 - When calcium carbonate is heated strongly, CO2 gas...Ch. 18 - Sodium reacts violently with water according to...Ch. 18 - Yeast can produce ethanol by the fermentation of...Ch. 18 - Elemental boron, in the form of thin fibers, can...Ch. 18 - Prob. 68GQCh. 18 - Prob. 69GQCh. 18 - Estimate the boiling point of water in Denver,...Ch. 18 - The equilibrium constant for the butane ...Ch. 18 - A crucial reaction for the production of synthetic...Ch. 18 - Calculate rG for the decomposition of sulfur...Ch. 18 - Prob. 74GQCh. 18 - A cave in Mexico was recently discovered to have...Ch. 18 - Wet limestone is used to scrub SO2 gas from the...Ch. 18 - Sulfur undergoes a phase transition between 80 and...Ch. 18 - Calculate the entropy change for dissolving HCl...Ch. 18 - Some metal oxides can be decomposed to the metal...Ch. 18 - Prob. 80ILCh. 18 - Prob. 81ILCh. 18 - Prob. 82ILCh. 18 - Titanium(IV) oxide is converted to titanium...Ch. 18 - Cisplatin [cis-diamminedichloroplatinum(II)] is a...Ch. 18 - Prob. 85ILCh. 18 - Explain why each of the following statements is...Ch. 18 - Decide whether each of the following statements is...Ch. 18 - Under what conditions is the entropy of a pure...Ch. 18 - Prob. 89SCQCh. 18 - Consider the formation of NO(g) from its elements....Ch. 18 - Prob. 91SCQCh. 18 - The normal melting point of benzene, C6H6, is 5.5...Ch. 18 - Prob. 93SCQCh. 18 - For each of the following processes, predict the...Ch. 18 - Heater Meals are food packages that contain their...Ch. 18 - Prob. 96SCQCh. 18 - Prob. 97SCQCh. 18 - Prob. 98SCQCh. 18 - Iodine, I2, dissolves readily in carbon...Ch. 18 - Prob. 100SCQCh. 18 - Prob. 101SCQCh. 18 - Prob. 102SCQCh. 18 - Prob. 103SCQCh. 18 - Prob. 104SCQCh. 18 - The Haber-Bosch process for the production of...Ch. 18 - Prob. 106SCQCh. 18 - Prob. 107SCQ
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- Cobalt(II) chloride hexahydrate, CoCl26H2O, is a bright pink compound, but in the presence of very dry air it loses water vapor to the air to produce the light blue anhydrous salt CoCl2. Calculate the standard free-energy change for the reaction at 25C: CoCl26H2O(s)CoCl2(s)+6H2O(g) Here are some thermodynamic data at 25C: What is the partial pressure of water vapor in equilibrium with the anhydrous salt and the hexahydrate at 25C? (Give the value in mmHg.) What is the relative humidity of air that has this partial pressure of water? The relative humidity of a sample of air is Relativehumidity=partialpressureofH2O(g)inairvaporpressureofwater100 What do you expect to happen to the equilibrium partial pressure over the hexahydrate as the temperature is raised? Explain.arrow_forwardC6H5CHO reacts with H₂ to form C6H5CH₂OH. The equilibrium constant, Kp, for this reaction is 1.79 at 523 K. C6H5CHO(g) + H₂(g) 2CH₂CH₂OH(g) The standard enthalpy change for this reaction (AHº) is -55.5 kJ/mol. (a) Predict the effect on the production of C6H₂CH₂OH when the temperature of the equilibrium system is increased. ŵ (b) Use the van't Hoff equation to estimate the equilibrium constant for this reaction at 632 K. Kp at 632 K =arrow_forwardC6H5CHO reacts with H2 to form C6H5CH2OH. The equilibrium constant, Kp, for this reaction is 1.79 at 523 K. C6H5CHO(g) + H2(g) C6H5CH2OH(g) The standard enthalpy change for this reaction (ΔH°) is -55.5 kJ/mol. (a) Predict the effect on the production of C6H5CH2OH when the temperature of the equilibrium system is increased. is production favored or disfavored? (b) Use the van’t Hoff equation to estimate the equilibrium constant for this reaction at 645 K. Kp at 645 K =arrow_forward
- Consider the following general equation for a chemical reaction. A(g) + B(g) → C(g) + D(g) ∆H° reaction = -10 kJ (a) Describe the two factors that determine whether a collision between molecules of A and B results in a reaction. (b) How would a decrease in temperature affect the rate of the reaction shown above? Explain your answer. (c) Explain why a catalyst increases the rate of a reaction but does not change the value of the equilibrium constant for that reaction. NOTE: Please briefly explain and answer a,b and c. Thank you.arrow_forwardFor the following pair of reaction diagrams, identify which of the pair is catalyzed. Explain your reasoning. 50 45 40 35 30 25 20 50 45 40 35 30 25 20 15 10 5 15 10 5 Extent of reaction Extent of reaction (a) (b) Energy (kJ) Energy (kJ)arrow_forwardA reaction A(aq)+B(aq)−⇀↽−C(aq) has a standard free‑energy change of −4.65 kJ/mol at 25 °C. What are the concentrations of A, B, and C at equilibrium if, at the beginning of the reaction, their concentrations are 0.30 M, 0.40 M, and 0 M, respectively? [B]= M [A]= M [C]= M How would your answers change if the reaction had a standard free‑energy change of +4.65 kJ/mol? All concentrations would be higher. There would be no change to the answers. There would be less A and B but more C. There would be more A and B but less C. All concentrations would be lower.arrow_forward
- A chemist fills a reaction vessel with 8.79 atm methane (CH4) gas, 1.16 atm oxygen (O2) gas, 0.995 atm carbon dioxide (CO2) gas, and 1.22 atm hydrogen (H2) gas at a temperature of 25.0°C. Under these conditions, calculate the reaction free energy AG for the following chemical reaction: CH()+0,(g) CO,(g)+2H₂(g) Use the thermodynamic information in the ALEKS Data tab. Round your answer to the nearest kilojoule.. 1kJ х Garrow_forwardHow do the following changes affect the value of theequilibrium constant for a gas-phase exothermic reaction:(a) removal of a reactant, (b) removal of a product,(c) decrease in the volume, (d) decrease in the temperature,(e) addition of a catalyst?arrow_forwardWhat will happen to the equilibrium, NaHCO3(s)Na2CO3(s) + CO2(g) + H2O(g);Ho = 136 kJ when: (a) the temperature is decreased(b) the volume of the container is increased (c) water vapor is removed(d) additional Na2CO3 is added(e) pressure of CO2 is increasedarrow_forward
- For the reaction given below, the arrhenius actication energy is 15.5 kj.mol-1. Find Δ≠ H0arrow_forwardExplain the lack slow or lack of a reaction at 4 degrees Celcius. is this situation reversible or recoverable?arrow_forward24 A reaction has a standard free‑energy change of −15.00 kJ mol−1(−3.585 kcal mol−1).Calculate the equilibrium constant for the reaction at 25 °C. keq=?arrow_forward
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