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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3. Use the data oven i the table to calculate AHrxn, ASrxn, AGrxn, and Keq for the following reaction at 298 K. With showing all work. 2 HNO3(aq) + NO(g) →3 NO2(g) + H2O(1) K=? S° ΔΗ/ (kJ/mol) Compound (J /mol-K) 146 HNO3(aq) NO(g) NO2(g) H20(1) - 206.57 90.29 210.65 A. Calculate 4H°rxn: 33.2 239.9 -285.84 69.94 B. Calculate AS`rxn: C. Using the answers from a. And b. Calculate. AGʻrxn.:
A chemical engineer is studying the two reactions shown in the table below. In each case, he fills a reaction vessel with some mixture of the reactants and products at a constant temperature of 72.0 °C and constant total pressure. Then, he measures the reaction enthalpy AH and reaction entropy AS of the first reaction, and the reaction enthalpy AH and reaction free energy AG of the second reaction. The results of his measurements are shown in the table. Complete the table. That is, calculate AG for the first reaction and AS for the second. (Round your answer to zero decimal places.) Then, decide whether, under the conditions the engineer has set up, the reaction is spontaneous, the reverse reaction is spontaneous, or neither forward nor reverse reaction is spontaneous because the system is at equilibrium. C₂H₂(g) + 50₂(g) → 3CO₂(g) + 4H₂O(1) 2CO₂ (g) + 4H₂O(g) → 2CH, OH (g) + 30₂ (g) ΔΗ = -1220. ΚΙ J K AS-6432. AG - KJ Which is spontaneous? O this reaction O the reverse reaction…
For each of the following processes would AS° be expected to be negative or positive? Why? 0:(g) + 2H:(g) 2H;0(g) H;O() H;0(s) NH:(g) + HCI3) NHCI(g) 2NH,NO:(s) 2N2(g) + 0:(g) + 4H;0(g) N204(g) → 2NO:(g)
A chem V ngineer is studying the two reactions shown in the table below. In each case, he fills a reaction vessel with some mixture of the reactants and products at a constant temperature of 90.0 °C and constant total pressure. Then. he measures the reaction enthalpy AH and reaction entropy AS of the first reaction, and the reaction enthalpy AH and reaction free energy AG of the second reaction. The results of his measurements are shown in the table. Complete the table. That is, calculate AG for the first reaction and AS for the second. (Round your answer to zero decimal places.) Then, decide whether, under the conditions the engineer has set up, the reaction is spontaneous, the reverse reaction is spontaneous, or neither forward nor reverse reaction is spontaneous because the system is at equilibrium. AH = 2220, kJ J AS = 6113. K AG = kJ 3co,() + 4H,0(1) → C,H,(g) + 50,(g) Which is spontaneous? O this reaction O the reverse reaction O neither AH = -951. kJ J AS = AG = – 14. kJ 2A1(s)…
33.6 g of a salt solution was mixed with 27.5 g of water in a calorimeter with a calorimeter constant of 66.5 J K-1 with all substances initially at 30.9 °C. The resulting solution was observed to be at a temperature of 12.2 °C and have a heat capacity of 3.97 J g K-1. Determine q for the mixing process. Oa. -5780 J Ob. 4540 J Oc. 8.05 x 104 J Od. 5780 J Oe. -7.86 x 104 J
→ 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
For the reaction given below, AH --1516 kJ at 25"C und AS--432.8 J/K at 25°C, This reaction is spontaneous SiH,(g) + 2 0:(g) SiO;()+2 H,0(6)
Calculate the reaction enthalpy for the decomposition of hydrogen peroxide, 2H2O20 H26) + O26) 2H2) + O216 2H2O0 + O26 from the following data: H2O20; AH°RXN = -187.8 kJ - 2H2O0; AH°Rxn = -571.6 kJ
A chemical engineer is studying the two reactions shown in the table below. In each case, she fills a reaction vessel with some mixture of the reactants and products at a constant temperature of 100.0 °C and constant total pressure. Then, she measures the reaction enthalpy AH and reaction entropy AS of the first reaction, and the reaction enthalpy AH and reaction free energy AG of the second reaction. The results of her measurements are shown in the table. Complete the table. That is, calculate AG for the first reaction and AS for the second. (Round your answer to zero decimal places.) Then, decide whether, under the conditions the engineer has set up, the reaction is spontaneous, the reverse reaction is spontaneous, or neither forward nor reverse reaction is spontaneous because the system is at equilibrium. 2Al(s) + 3H₂O(g) → Al₂O₂ (s) + 3H₂(g) 2CO₂(g) + 4H₂O(g) → 2CH₂OH(g) + 30₂ (g) ΔΗ = -951. kJ AS = -2549. AG = | KJ -0-/21 K Which is spontaneous? this reaction the reverse reaction…
A chemical engineer is studying the two reactions shown in the table below. In each case, he fills a reaction vessel with some mixture of the reactants and products at a constant temperature of 146.0 °C and constant total pressure. Then, he measures the reaction enthalpy AH and reaction entropy AS of the first reaction, and the reaction enthalpy AH and reaction free energy AG of the second reaction. The results of his measurements are shown in the table. Complete the table. That is, calculate AG for the first reaction and AS for the second. (Round your answer to zero decimal places.) Then, decide whether, under the conditions the engineer has set up, the reaction is spontaneous, the reverse reaction is spontaneous, or neither forward nor reverse reaction is spontaneous because the system is at equilibrium.