For each reaction, calculate AHrn, ASn, and AGxn 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. N2O4(8) – 2 NO2(g) b. NH4C1(s) c. 3 H2(8) + Fe2O3(s) → 2 Fe(s) + 3 H2O(8) d. N2(8) + 3 H2(8) 0.25 HCl(8) + NH3(8) - | 2 NH3(8) HO

For the following example, identify the following:   F2(l) → F2(g)   A. at low temperature, the reaction is spontaneous and ΔG < 0 and at high temperature, the reaction is spontaneous and ΔG < 0 B. at low temperature, the reaction is nonspontaneous and ΔG > 0 and at high temperature, the reaction is spontaneous and ΔG < 0 C. at low temperature, the reaction is spontaneous and ΔG < 0 and at high temperature, the reaction is nonspontaneous and ΔG > 0 at low temperature, the reaction is nonspontaneous and ΔG > 0 and at D. high temperature, the reaction is nonspontaneous and ΔG > 0 It is not possible to determine without more information.

C3H8 (g) + 502 (g) --> 3CO2 (g) + 4H2O (g) + 2200 k) Given the above equation, which statement is correct? A. can be spontaneous at all temperatures B. can be spontaneous at high temperatures O C. can be spontaneous at low temperatures D. can be spontaneous at no temperatures

The following reaction is endothermic. 2NH3(g) → N2(g) + 3H2(g) This means the reaction   A. will be spontaneous at high temperatures. B. will be spontaneous at low temperatures. C. is not spontaneous at any temperature. D. is spontaneous at all temperatures.

49.For the decomposition of hydrogen peroxide to water and oxygen,         H2O2(g) ⟶⟶ H2O(g) + O2(g) ΔΔH° = -106 kJ, and ΔΔS° = +0.0580 kJ/K. In what temperature range is the reaction spontaneous (ΔΔG° < 0)? A. The temperature must be greater than 1.83××103 K B. The temperature must be less than 1.83 ××103 K. C. The temperature must be between 225 K and 1.83 ××103 K. D. ΔΔG° is always less than zero. E. ΔΔG° is never less than zero.

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)

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

A reaction has a ΔH of -87.36 kJ and a ΔS of -175.3 J/K. At what temperature (in K) does the reaction become spontaneous?     626.4 K     This reaction is always spontaneous     498.3 K     434.6 K     This reaction is never spontaneous

At what temperatures will a reaction be spontaneous if AH = +158 kJ and AS = +411 %3D J/K? O The reaction will never be spontaneous. O The reaction will be spontaneous at any temperature. O All temperatures above 384 K O All temperatures below 384 K