At 25°C, the reaction N2(g) + 3 H2(g) --> 2 NH3(g) is extremely slow,although thermodynamics showsthat it is spontaneous.(delta) Hᵒreaction = -92600 J/mol.What is (delta)Suniverse?

Answered: At 25°C, the reaction N2(g) + 3 H2(g) -…

Chemistry

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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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5.) Which of the following statements accurately describes the spontaneity of the reaction below?Al2O3(s) + 2Fe(s) → 2Al(s) + Fe2O3(s) H°rxn = 830.8 kJ/mol, S°rxn = 168 J/mol·K a. The reverse reaction is always spontaneous.b. The reaction is spontaneous above 4945 K.c. The reaction is spontaneous below 4945 K.d. The reaction is always spontaneous.e. There is not enough information to determine.
2H2O(g) ----> 2H2(g) + O2(g) The reaction above is only spontaneous at temperatures above 2000K. Is the reaction endothermic (+ΔH) or exothermic (-ΔH)?
Please report in correct sigfigs and in units of kJ/mol
Hint: No calculations are required. For the reaction 2HBr(g) + Cl2(g)- >2HCI(g) + Br2(g) AH° = -81.1 kJ and AS° =-1.20 J/K At standard conditions, this reaction would be product favored O at all temperatures. O at relatively high temperatures. O at no temperature. O at relatively low temperatures.
5-For the reaction, A+B C, AH-+30 kJ; AS°=+50 J/K.Therefore the reaction is: (a) spontaneous at all temperatures. (b) nonspontaneous at all temperatures. (d) irreversible at all temperatures (c) reversible at all temperatures 6- How much heat is necessary to convert 2mol of water at( 50°C) to steam at 150°C?The molar heat capacity of liquid water and steam are 75.3 J/mol. K and 36.4 J/mol. K respectively. The heat of vaporization 40.7 KJ/mol. a-81400J 7- From the reactions: b-82.337KJ c-753J d-3641 e- none of them Cgraphia +2H2(g) → CHA(R) AH = -79.9KJ C(graphia + 2Cl2(g) → CCla AH = -139KJ H 20 + Cl₂00) → HCL) AH-92.3KJ 202) calculate AH, for the reaction CH ACE +4Cl2) a- (-615.1KJ) c-(-428.3KJ) 4HCI+CCI b-(-311.2KJ) d- none of them
9) For which set of values of AH and AS will a reaction be non-spontaneous at 25°C? a) AH• = -10 kJ, AS = - 15 J b) AH• = - 10 kJ, AS= +5 J c) AH° = + 5 kJ, AS = +8J
Using H° data, calculate the standard enthalpy change for the reaction at 298K. 2 NH3(g) HNO3(aq) --> NO2(g) 2 H20(1) AH° (KJ/mol) -46.19 -206.6 33.84 -285.83 (Note: the table AH values are located directly below the corresponding compound, this is the number found in the Appendix)
For reaction Na2CO3(s) + 2HC(g) -> NaCl(s) + CO2(g) -> H20(l) ΔH is -144.1 KJ. What is ΔU?
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 63.0 °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.
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 74.0 °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 = 181. kJ AS = -499. K ? 2NO(g) N, (g) + 0, (g) AG = kJ Which is spontaneous? this reaction the reverse reaction neither
Consider the reaction that happens at -13 °C: 1A + 2B 8C + 6D. Using the data from the table: B C D AH; (kJ mol 1) 309 144.4 149.5 s° (U mol 1 K1) 61.4 33.6 76.4 153.4 calculate AG° (in kJ) of the reaction. (assume that values of AH and S do not change with the temperature) Enter a number with sign (+ or -) to 1 decimal place in kJ.
4

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At 25°C, the reaction N2(g) + 3 H2(g) - -> 2 NH3(g) is extremely slow, although thermodynamics shows that it is spontaneous. (delta) Hᵒreaction = -92600 J/mol. What is (delta)Suniverse?