Standard molar entroples, S, in J/K are given below eacCh reaclant and product in the reaction shIown belovw. The standard entropy of reaction, AS , for this J. CH4(g) + 2 O2(g) → CO2(g) + 2 H20() 213.6 reaction is 186.2 _205.0 _69.9 Express your answer using four significant figures.

1. Please consider 0.15 gm of Constantan (a Cu/Ni alloy widely used in thermocouples, c = 390 J/•K-kg) that cooled through exposure to the laboratory atmosphere (T 22 •C) from 620 C to 20 C. a. Please determine the change in entropy of the Constantan (in J/ K- kg). b. Please determine the change in entropy of the laboratory atmosphere (in J/ K-kg). c. Please determine the change in entropy of the universe (in J/ K-kg). %3D

Traduction: Given the reaction: determine the entalpy change for the next ecuation: 8. Dada la reaccion 4AICI3(s) + 302(g) → 2Al2O3(s) + 6CI2(g); AH= -529.0 kJ %3D determine AH para la siguiente rea ión Cl2(g) + %Al2O3(s) %AICI3(s) + ½O2(g) +529.0 kJ +88.2 kJ +176.3 kJ +264.5 kJ a)

1 2 words O English (United States) Calculating dG from dH and d 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 130.0 °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. ALO3(s) + 2Fe(s)- 2Al(s) + Fe₂O₂ (s) co₂(g) + 2H₂O(g) - CH₂(g) + 20₂ (8) AH = 852. kJ AS = 2044. MacBook Air AG=kJ…

A chem.. 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 52.0 °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 J AS = 557. K N, (g) + 0, (g) → 2NO (g) AG = N, (g) + 0,(8) kJ Which is spontaneous? this reaction the reverse reaction neither ΔΗ - - 1353. kJ J AS = K 2CH,OH (g) + 30,(g)…

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The reaction 2N;O)- 2N2(9) + Oz(g) has AH° - -163.14 kJ. What is the value of AE for the decomposition of 194 g of N20 at 25 °C? If we assume that AH doesn't change appreciably with temperature, what is AE for this reaction at 234 °C? At 25 °C: AE - i kJ At 234 °C: AE - kJ

Hìnt: No calculations are required. For the reaction 2C02(g) + 5H2(g)→C2H2(g) + 4H20(g) AH° = 46.5 k) and AS° = -125 J/K %3D At standard conditions, this reaction would be product favored at relatively low temperatures. at relatively high temperatures. at no temperature. O at all temperatures.

Estimate the entropy change for the reaction: 2NO2 (g) + N204 (g) Standard entropy and enthalpy of formation S (U/mol K) Species H>(8) H(g) O:(8) O(g) N:(g) N(g) NO(g) H,O (g) H;0 (1) N,0 (g) NO2 (g) N2O N,Os(g) N20s(s) NHANO,(s) AH", (kJ/mol) 130.6 114.6 218.0 205 161 249.2 191.5 153.2 472.7 210.7 90.25 188.7 -241.8 69.91 -285.8 219.7 82.05 240.0 33.2 304.2 9.2 356 11 178 -43.1 151.1 -365.6