ll Verizon ?5:55 AM9 100%webassign.netAmong other things, an ideal fuel for the control thrusters of a space vehicleshould decompose in a spontaneous exothermic reaction when exposed to anappropriate catalyst. Evaluate the following substances under standard stateconditions as suitable candidates for fuels. (Provide AG° and AH° in kJ/molreactant.)(a) nitrous oxide:N,0(g) → N2(9) + 1/2 0,(9)AG° =kJ/molAH° =kJ/molSpontaneityO spontaneousO nonspontaneousThermicityO endothermicO exothermicSuitabilityO suitableO not suitable(b) diborane:B,H,(9) - 2 B(s) + 3 H,(9)AG° =kJ/molAH° =kJ/molSpontaneityO spontaneousO nonspontaneousThermicityO endothermicexothermicSuitabilityO suitableO not suitable(c) dinitrogen trioxide:N,0,(9) – N,(9) + 3/2 0,(9)AG° =KJ/molAH° -kJ/molSpontaneityO spontaneousO nonspontaneousThermicityO endothermicO exothermicSuitabilityO suitableO not suitable(d) aluminum hydride:AIH, (s) – Al(s) + 3/2 H,(9)AG° =kJ/molΔΗ' -kJ/molSpontaneityO spontaneousO nonspontaneousThermicityO endothermic

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Answered: (a) nitrous oxide: N,O(g) - N,(g) + 1/2…

(a) nitrous oxide: N,O(g) - N,(g) + 1/2 0,(9) AG° - |kJ/mol AH° - kJ/mol Spontaneity spontaneous nonspontaneous Thermicity endothermic exothermic Suitability suitable not suitable

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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der the following reaction: 2NO2(g) N₂O4 (9) Part A Part B Calculate AG at 298 K if the partial pressures of NO₂ and N₂O4 are 0.36 atm and 1.64 atm, respectively. Express the free energy in kilojoules to two decimal places. |ΨΕΙ ΑΣΦ AG= -6288.99 Submit Previous Answers Request Answer ? Review I Consta kJ X Incorrect; Try Again; 4 attempts remaining This value of free energy is more negative than AG for the reaction (i.e., more spontaneous), but the partial pressure of ta about four times greater than that of the reactant, so the free-energy change is expected to be more positive than AG (i.e spontaneous). Given that AG = AG + RTln Q, calculate the value of Q (it should be greater than 1 for the specified conditions), and free energy from Part A to find the free-energy change at the given partial pressures. Make certain values are expressed in before summing them.
Use the data given in the table to calculate the value of AGan at 25" C for Compound AG; (kJ/mol) the reaction described by the equation A +387.7 B +655.8 A+B=C +402.0 kJ AGxn = mol If AHan and ASin are both positive values, what drives the spontancous reaction and in what direction at standard conditions? The spontaneous reaction is enthalpy-driven to the left. The spontaneous reaction is entropy-driven to the right. The spontaneous reaction is entropy-driven to the left. The spontaneous reaction is enthalpy-driven to the right.
If AS at 25°C sys =-198.3 J/K, is the reaction spontaneous N2 + 3H2 → 2NH3 • AS univ = AS sys + AS surr > ? AS surr (AHsys)/T Determine the AHrxn • AH° N2(g) = 0 kJ/mol • AH° H2(g) = 0 kJ/mol • AH°; NH3(g) = -46.19 kJ/mol
26. A mole of perfect gas at 27°C is expanded isothermally from an initial pressure of 3.00 atm to a final pressure of 1.00 atm in two ways (a) reversibly, (b) against a constant external pressure of 1.00 atm. Cal- culate q, w, AU, AH, AS, ASsurr, AStot for both. (+2.74 kJ, -2.74 kJ, 0, 0, 9.13 J/K, -9.13 J/K, 0 ||1.66 kJ, -1.66 kJ, 0, 0, 9.13 J/K, -5.53 J/K, 3.60 J/K) T=27°C 300 K b) w - - Peut av = -(1 atm) (ner - her NRT ) Pf P₁ IsoT w AU÷0 q = -((atm) 1 mol. 8.314 /mol.K - 300K I atm W = -16.6 kJ. 9 = 16.6 kJ AS: grev= UT Imol. 8.314 /mol.K·3.00K 3 atm 27. A block of copper of mass 500 g and initially at 293 K is in thermal contact with an electric heater of resistance 1 kOhm and negligible
Gaseous SO2Cl2 reacts with liquid water to form hydrogen chloride gas and liquid sulfuric acid. Using data tabulated in Appendix G of your text, calculate the enthalpy change, in units of kJ/mol, for the formation of 2 mol of liquid sulfuric acid.
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M Preq 3 Consider the reaction 00 E D 4HCI(g) + O₂(g) 2H₂O(g) + 2Cl₂(8) for which AH° = -114.4 kJ and AS° = -128.9 J/K at 298.15 K. J/K (1) Calculate the entropy change of the UNIVERSE when 1.775 moles of HCI(g) react under standard conditions at 298.15 K. ASuniverse (2) Is this reaction reactant or product favored under standard conditions? Submit Answer (3) If the reaction is product favored, is it enthalpy favored, entropy favored, or favored by both enthalpy and entropy? If the reaction is reactant favored choose 'reactant favored'. 4 000 000 R F DO LO V % 5 [Review Topics] [References] Use the References to access important values if needed for this question. T Retry Entire Group 8 more group attempts remaining Cengage Learning Cengage Technical Support G 6 B Y H & 7 N U 1 * 8 J M 9 K बैं O < L P Previous Email Instructor Save and Exit { + 11 Next ? } ]
Be sure to answer all parts. From the following combinations of AH and AS, predict if a process will be spontaneous at a high or low temperature: (a) both AH and AS are negative Process is spontaneous at high and low temperatures. Process is spontaneous at high temperatures and nonspontaneous at low temperatures. Process is nonspontaneous at high and low temperatures. Process is nonspontaneous at high temperatures and spontaneous at low temperatures. (b) AH is negative and AS is positive Process is spontaneous at high and low temperatures. Process is spontaneous at high temperatures and nonspontaneous at low temperatures. Process is nonspontaneous at high and low temperatures. Process is nonspontaneous at high temperatures and spontaneous at low temperatures. (c) both AH and AS are positive Process is spontaneous at high and low temperatures. Process is spontaneous at high temperatures and nonspontaneous at low temperatures. Process is nonspontaneous at high and low temperatures.…
(Q74) A certain process is nonspontaneous at low temperatures. Given that AHX = 201.2 kJ and ASPxn = 876 J/K, at what temperature (in °C) will the process become spontaneous? %3D (Report your Celsius temperature to one decimal place --> if your answer has a decimal place of "O" and Canvas chops it off, don't worry about it).
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 136.0 °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 = -5426. K C,H, (g) + 50,(8) → 3C0,g) + 4H,0() AG = kJ Which is spontaneous? O this reaction O the reverse reaction O neither ΔΗ 50. ky AS = 6CI, (g) + 2Fe,0.(s)…