For a chemical reaction to be spontaneous at all temperatures in the reverse direction, which of the following conditions must be met? AS° > 0, AH° < 0 AS° < 0, AH° < 0 It is not possible for a reaction to be spontaneous in the reverse direction at all temperatures. AS° < 0, AH° > 0 AS° > 0, AH° > 0

Calculate the standard free-energy change AG" and the equilibrium constant K, for the following reaction at 25°c. Co(g) + 3H3 (9) → CH, (g) + H20(g) Substance AG (kJ/mol) Co() -137.2 H2 (9) CH, (g) -50.80 H2 O(9) -228.6 AG° kJ K,

A reaction has values ΔS = 72.3 J K mol-1 and ΔH = 47.0 kJ mol-1. At what temperature (in °C) will this reaction become spontaneous?

For a chemical reaction to be spontaneous at all temperatures, which of the following conditions must be met? O Itis not possible for a reaction to be spontaneous at all temperatures. O AS° > 0, AH > 0 O AS° > 0, AH 0

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.

AS is positive for which of the following reactions

For each reaction, calculate ΔH°rxn, ΔS°rxn, and ΔG°rxn at 25 °C and state whether or not the reaction is spontaneous. If the reaction is not spontaneous, would a change in temperature make it spontaneous? If so, should the temperature be raised or lowered from 25 °C?a. 2 CH4( g)------->C2H6( g) + H2( g)b. 2 NH3( g)------> N2H4( g) + H2( g)c. N2( g) + O2( g)-------->2 NO( g)d. 2 KClO3(s)-------->2 KCl(s) + 3 O2( g)

Consider the reaction: H2( g) + I2( g)Δ2 HI( g)The following data show the equilibrium constant for this reaction measured at several different temperatures. Use the data to find ΔH°rxn and ΔS°rxn for the reaction.Temperature                        Kp150 K                                   1.4 * 10- 6175 K                                   4.6 * 10- 4200 K                                  3.6 * 10- 2225 K                                  1.1250 K                                   15.5

47. Fill in the blanks in the table. Both AH and AS refer to the system. MISSED THIS? Read Section 19.60; Watch KCV 19.60 ΔΗ + AS + + AG Temperature dependent Low Temperature Spontaneous High Temperature Spontaneous Nonspontaneous Nonspontaneous

On the basis of AG° for each of the following reac- tions, decide whether the reaction is spontaneous or nonspon- taneous as written. Or, if you expect an equilibrium mixture with significant amounts of both reactants and products, say 18.51 so. a. SO2(g) + 2H,S(g) → 3S(s) + 2H,O(g); AG° = –91 kJ b. 2H,O2(aq) O2(g) + 2H2O(I); AG° = -211 kJ