CO (g) + 2 O₂ (g) → CO₂ (g) a) For this gas phase reaction, determine (i) ArxnH (in kJ/mole) and (ii) ArxnS (in J/mol-K) at 298 K per mole of CO. b) The temperature-dependence of the enthalpies of the three reaction species can be found using data gathered at the NIST Webbook site under the heading "Gas phase thermochemistry data- Gas Phase Heat Capacity (Shomate Equation)". Use the formula for HⓇ and coefficients given there to determine what ArxnH would be (in kJ/mol) at 400 K. c) Spectroscopic studies of diatomic molecules can provide insight into the bond strengths of those molecules. They indicate that the bond energy of O₂ is 498.34 kJ/mol, and that of CO is 1072 kJ/mol. We can approximate the enthalpy of a reaction as being equivalent to the energy required to break bonds among the reactants minus the energy recovered when new bonds are made. What value would this approximation imply for the average strength (in kJ/mole) of each of the two C-O bonds in CO2?

CO (g) + 2 O₂ (g) → CO₂ (g) a) For this gas phase reaction, determine (i) ArxnH (in kJ/mole) and (ii) ArxnS (in J/mol-K) at 298 K per mole of CO. b) The temperature-dependence of the enthalpies of the three reaction species can be found using data gathered at the NIST Webbook site under the heading "Gas phase thermochemistry data- Gas Phase Heat Capacity (Shomate Equation)". Use the formula for HⓇ and coefficients given there to determine what ArxnH would be (in kJ/mol) at 400 K. c) Spectroscopic studies of diatomic molecules can provide insight into the bond strengths of those molecules. They indicate that the bond energy of O₂ is 498.34 kJ/mol, and that of CO is 1072 kJ/mol. We can approximate the enthalpy of a reaction as being equivalent to the energy required to break bonds among the reactants minus the energy recovered when new bonds are made. What value would this approximation imply for the average strength (in kJ/mole) of each of the two C-O bonds in CO2?

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...

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At -13.0 °C the pressure equilibrium constant K, = 5.8 x 10 for a certain reaction. Here are some facts about the reaction: • Some of the reactants are liquids and solids. • If the reaction is run at constant pressure, the volume increases by 14.%. • The constant pressure molar heat capacity C = 2.03 J· mol. K'. - 1 %3D As Yes. 10 Using these facts, can you calculate K, at 0.80 °C? d. No. If you said yes, then enter your answer at right. Round it to 2 significant digits. Yes, and K, will be bigger. If you said no, can you at least decide whether K¸ at Yes, and K. will be 0.80 °C will be bigger or smaller than K̟ at –13.0 °C? smaller. d. No. Continue Submit Assignment 144H TAKING YOU TO A NEW REALITY et unvmedreabiy PREDATOR
For a certain equilibrium reaction, the following data are given AH = -57.2 kJ/mol K = 1.2 x 104 Which of the following statements are supported by the given data? AG = AH - TAS 0, since K >> 1 AG = - RTINK > 1 AG = AH - TAS > 0, the reaction is thermodynamically unfavorable
7. (a A 5.00 mol sample of an ideal gas is compressed irreversibly and isothermally at 150.00 K from an initial volume of 30.00 L in two steps: Step #1: Pext = 5.00 bar, Step #2: Pext = 20.00 bar. Determine the value of the total work and heat involved (in J). (b) Describe in words what happens to the total amount of work if the compression occurs in three steps. (c). Assuming the process could be done in one or multiple steps and the process could be reversible or irreversible, determine the minimum and maximum amount of work that could be done to complete the compression.
A 0.500 mole sample of CO(g) is combusted in a constant pressure calorimeter to CO2(g). The temperature is observed to rise from 25.00°C to 27.50°C. The heat capacity of the calorimeter (calorimeter constant) is 56.6 kJ/K. What isA H in kJ/(mole of CO) for the reaction? A) –283 kJ/mol B +283 kJ/mol -282 kJ/mol D +282 kJ/mol
The value of AHT for the following reaction is 169.5 kJ. The value of AH for CaO(s) s kmd. CaCO3 (s)- Cao (s) * CO2 ) Standard Enthalpies of Formation of Some Inorganic Substances at 25'C TABLE 6.4 Subatance A mol) Substance A /mo) -1876 Ag(s) AgC) AKS) 127.0 ALO) "1669.8 Mg(s) MgO) Br() HBrg Cigraphite) Cidiamond) -36.2 -S01.S -11129 1.90 NH4 NO) -110.5 463 904 33.35 Cas) 35.6 NO) CCO(s) 966 Og) HCKg Car) 92.3 Sirhombic Scenonocinic) so-co so Fig) -716 Hg) Hg) 20.15 2418
→ C ||| = www-awa.aleks.com/alekscgi/x/Isl.exe/1o_u-lgNslkr7j8P3jH-lvgXwPgmUhvlCeeBZbuluBY TUHz/m/I OTHERMOCHEMISTRY Calculating the heat of reaction from molar reaction enthalpy a... A chemist measures the energy change AH during the following reaction: Cl₂(g)+H₂(g) → 2 HCl(g) Use the information to answer the following questions. This reaction is... Suppose 68.3 g of Cl₂ react. Will any heat be released or absorbed? 75°F Sunny If you said heat will be released or absorbed in the second part of this question, calculate how much heat will be released or absorbed. Explanation ΔΗ = - 184. kJ Round your answer to 3 significant digits. Check endothermic. O exothermic. O Yes, absorbed. O Yes, released. O No. H Q Search 0 0x10 X S a C 4 4 1/3 Andrew V Relate © 2023 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessibility 25 4 ? ➤III olo Ar 7:37 PM 7/16/2023
A 0.576 g sample of liquid C5H12 was combusted using excess oxygen gas inside a bomb calorimeter, with the products being carbon dioxide gas and liquid water. The calorimeter's heat capacity is 4.957 kJ °C^-1. If the temperature inside the calorimeter increased from 25.0 °C to 35.1 °C, determine A,U for this reaction in kl mol (with respect to C3H12). Do not worry about how realistic the final answer is.
One industrial, large-scale method for refining iron ore to elemental iron is the reaction at high temperatures with carbon monoxide. Calculate AGº for the reaction of iron(III) oxide with carbon monoxide to give elemental iron and carbon dioxide. Use data in the table below: Substance Ag(s) AgCl(s) Al(s) Al₂O3(s) C(s) (graphite) CO(g) CO₂(g) CH4(g) CH₂Cl(g) CH₂OH(1) C₂H₂(g) C₂H4(g) C₂H6(g) C₂H18(1) C₂H,OH() Ca(s) CaCO3(s) CaCl₂(s) 197.9 213.6 186.2 234.2 126.8 CO(NH,),(s) 104.6 CO(NH,),(aq) 173.8 200.8 219.8 229.5 466.9 161 Substance Ag(s) AgBr(s) AgCl(s) Al(s) Al₂O3(s) C(s) (graphite) C₂H₂(g) C₂H₂(g) C₂H6(g) C₂H Ca(s) Standard Entropies of Some Typical Substances at 298.15 K CaBr₂(s) CaCO3(s) CaCl₂(s) CaO(s) Fe₂O3(s) H₂(g) H₂O(g) H₂O(1) (J mol-¹ K-¹) 42.55 96.2 28.3 51.0 CO(g) CO₂(g) CH4(g) CH₂Cl(g) CH31(g) CH₂OH(1) CO(NH₂)2(s) (urea) CO(NH,),(aq) AG° = kJ 5.69 Ca(OH)2 (s) CaSO4(s) CaSO4 H₂O(s) CaSO4-2H₂O(s) Cl₂(g) Fe(s) 41.4 92.9 114 Substance (J mol-¹ K-¹) CaO(s) 40 Ca(OH)₂ (s)…
A styrofoam calorimeter contains 60.0 mL of o.750 M H.C,H 0, at 3 6 22.8°C. When 9.83 g NaHCO, is added to the calorimeter, the temperature of the resulting solution decreases to a minimum of 5.1°C. The reaction that occurs is: HаCоН,О-(aд) + 3 NaHCO3(aq) > NagCgHsО7(ag) + 3 СО2(9) + 3 Н-0(1) AHreaction = ??? What is the (experimental) enthalpy change for this reaction, AH ? (Use the total mass of reaction solution and 4.18 J/(g °C) for the specific heat of the solution in your calculations.) kJ/mol
At -8.64 °C the concentration equilibrium constant K = 7.7 for a certain reaction. Here are some facts about the reaction: -1 • The initial rate of the reaction is 5.3 mol·L¯¹·s¯¹. . If the reaction is run at constant pressure, 132. kJ/mol of heat are absorbed. • The constant pressure molar heat capacity C = 2.97 J'mol K¹. Yes. Using these facts, can you calculate K at 16. °C? x10 O No. If you said yes, then enter your answer at right. Round it to 2 significant digits. If you said no, can you at least decide whether Kat 16. °C will be bigger or smaller than K at -8.64 °C? C Yes, and K will be bigger. Yes, and K will be smaller. No.
. 2 H2S(g) + 3 O2(g) → 2 SO2(g) + 2 H2O(g) Delta Hrxn = -1036 kJ; Delta Srxn = -153.2 J/K At above what temperature (roughly) the reaction becomes nonspontanesous? A)158.7 K B) 298 K C) 6.762 × 103 K D) 273.16K F) 6.762 K
1. Argon is allowed to expand isothermally (at 298 K) and reversibly from an initial molar volume of 5.0 L/mol to a final molar volume of 11 L/mol. (a) Calculate the work (in units of kJ to 4 sig. figs.) done assuming it behaves as an ideal gas (b) Calculate the work (in units of kJ to 4 sig. figs) assuming it is non-ideal using the van der Waals equation where a = 1.34 atm L2 mol-2 b = 3.20 x 10-2 L mol-1