8) A given reaction absorbs 125 kJ of energy and gains 11.8 J/K of entropy. Under...

Question

Question

8) A given reaction absorbs 125 kJ of energy and gains 11.8 J/K of entropy. Under what conditions will the reaction be sponta

science chemistry

Answer 1

Answer #1

$\Delta$ G = $\Delta$ H - T $\Delta$ S

amount of energy is absorbed = 125 KJ

hence , $\Delta$ H = +125 KJ

gains entropy, hence $\Delta$ S also positive

$\Delta$ S= + 11.8 J/K

reaction will be spontaneous when $\Delta$ G < 0

so,

T $\Delta$ S > $\Delta$ H

^or, T > $\frac{\Delta H}{\Delta S}$

or, T > $125 x 1000 11.8$

or,T > 10593 K .

hence reaction will be spontaneous above temperature 10593 K.

Answer 2

Similar Homework Help Questions

A spontaneous reaction has a value of ΔH° of -11.8 kJ and ΔS° of -61.4 J/K....

A spontaneous reaction has a value of ΔH° of -11.8 kJ and ΔS° of -61.4 J/K. At what temperature does this reaction become nonspontaneous? 1. 192K 2. 83.7 K 3. 229 K 4. 273 K
For a given reaction, AH is 111 kJ and AS is -249 J/K. At what temperatures...

For a given reaction, AH is 111 kJ and AS is -249 J/K. At what temperatures is the reaction spontaneous? A. T< 446 K B. None. The reaction is never spontaneous. C. The reaction is spontaneous at all temperatures. D.T> 73 K E.T>446 K
1. A reaction has AH = 100 kJ/mol and AS = 250 J/mol K. a. Is...

1. A reaction has AH = 100 kJ/mol and AS = 250 J/mol K. a. Is the reaction spontaneous at room temperature? b. If not, under what temperature conditions will it become spontaneous? 2. Consider the following reaction at 298 K: N204(g) = 2NO2(g) KP=0.142 What is the standard free energy change at this temperature? Is the reaction spontaneous at this temperature?

For a particular chemical reaction Delta H =6.8 kJ and Delta S = -29 J/K. Under...

For a particular chemical reaction Delta H =6.8 kJ and Delta S = -29 J/K. Under what temperature condition is the reaction spontaneous? A) When T < -234 K B) When T < 234 K C) The reaction is spontaneous at all temperatures D) When the reaction is not spontaneous at any temperatures E) When T > 234 K
For a given reaction, ΔH = +20.8 kJ and ΔS = +27.6 J/K. The reaction is...

For a given reaction, ΔH = +20.8 kJ and ΔS = +27.6 J/K. The reaction is spontaneous __________ A) At T < 754 K B) At T > 133 K C) At all temperatures D) At T > 754 K E) At T < 133 K
The enthalpy of a certain reaction is +233 kj/mol and the entropy is +110J/molk. Above what...

The enthalpy of a certain reaction is +233 kj/mol and the entropy is +110J/molk. Above what temperature will the reaction be spontaneous. The enthalpy of a certain reaction is +233 kJ/mol, and the entropy is +110 J/mol K. Above what temperature will the reaction be spontaneous? 8.

For a particular chemical reaction Delta H = 6.5 kJ and Delta S = -33 J/K....

For a particular chemical reaction Delta H = 6.5 kJ and Delta S = -33 J/K. Under what temperature condition is the reaction spontaneous? When T> 197 K. When T< 197 K. The reaction is not spontaneous at any temperature. When T < -197 K. The reaction is spontaneous at all temperatures.
A certain reaction has Ho = 79.70 kJ and So = -55.80 J/K. (a) Is this...

A certain reaction has Ho = 79.70 kJ and So = -55.80 J/K. (a) Is this reaction exothermic, endothermic or isothermic (neither)? This reaction is ---Select--- exothermic endothermic isothermic . (b) Does this reaction lead to a decrease, an increase, or no change in the degree of disorder in the system? This reaction leads to ---Select--- a decrease an increase no change in the disorder of the system. (c) Calculate Go for this reaction at 298 K. If this value is less...
A reaction has a ΔH°= 204.6 kJ and a ΔS°= -19.5 J/K. a. Given the sign...

A reaction has a ΔH°= 204.6 kJ and a ΔS°= -19.5 J/K. a. Given the sign and magnitude of ΔH and ΔS, will the reaction be spontaneous at all temperatures, nonspontaneous at all temperatures? Briefly explain your reasoning. b. Calculate the standard free energy change for the reaction at 298 K. c. Is the reaction spontaneous or nonspontaneous at 298 K?

1. Thermodynamic data at 298 K. So (J/K) AHOf (kJ/mol) 205 0 O2 (g) 239 142.7...

1. Thermodynamic data at 298 K. So (J/K) AHOf (kJ/mol) 205 0 O2 (g) 239 142.7 O3 (g) a) Calculate the standard entropy change for the production of ozone from oxygen at 298 K. Is this an increase or decrease in randomness? Explain briefly. -> 203 (g) 302 (g) b) Calculate the standard free energy change for this reaction. Is this reaction spontaneous under standard conditions? c) Calculate the AG° of formation for ozone.