Question

For a particular reaction, delta H is 67.6 kJ/mol and delta S is 126.9 J/(molk). Assuming...

For a particular reaction, delta H is 67.6 kJ/mol and delta S is 126.9 J/(molk). Assuming these values change very little with temperature, over what temperature range is the reaction spontaneous in the forward direction?

The reaction is spontaneous for temperatures

less than? Greater than?

T= ???? K

Homework Answers

Answer #1

delta G has to be negative for spontaneous reaction that is delta G < 0

                                                                                 deltaH-T*deltaS <   0

                                                                                  67.6*1000J - T* 126.9J < 0

                                                                                   so 67600   < T*126.9

                                                                                    so 67600/126.9    <   T

                                                                                         523.7   <T

                       So reaction to be spontaneous T >523.7 K

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
Find the temperature (in K) above which a reaction with a delta H of 123.0 kJ/mol...
Find the temperature (in K) above which a reaction with a delta H of 123.0 kJ/mol and a delta S of 90.0 J/K×mol becomes spontaneous. Use four significant figures. T=________K
For the reaction C(s) + H2O(g) CO(g) + H2(g) H° = 133.3 kJ/mol and S° =...
For the reaction C(s) + H2O(g) CO(g) + H2(g) H° = 133.3 kJ/mol and S° = 121.6 J/K mol at 298 K. At temperatures greater than ________ °C this reaction is spontaneous under standard conditions.
A) The ΔHvap of a certain compound is 42.25 kJ·mol–1 and its ΔSvap is 67.47 J·mol–1·K–1....
A) The ΔHvap of a certain compound is 42.25 kJ·mol–1 and its ΔSvap is 67.47 J·mol–1·K–1. What is the boiling point of this compound? B) For a particular reaction, ΔH° is -13.9 kJ/mol and ΔS° is -41.6 J/(mol·K). Assuming these values change very little with temperature, over what temperature range is the reaction spontaneous in the forward direction?
For a given reaction, ΔH = -26.6 kJ/mol and ΔS = -77.0 J/K⋅mol. The reaction is...
For a given reaction, ΔH = -26.6 kJ/mol and ΔS = -77.0 J/K⋅mol. The reaction is spontaneous ________. Assume that ΔH and ΔS do not vary with temperature. For a given reaction,  = -26.6 kJ/mol and  = -77.0 J/Kmol. The reaction is spontaneous ________. Assume that  and  do not vary with temperature. at T > 298 K at all temperatures at T < 345 K at T < 298 K at T > 345 K
5. For a given reaction Delta H Standard = -45 kJ and Delta S Standard =...
5. For a given reaction Delta H Standard = -45 kJ and Delta S Standard = -103 J/K. A. Is the reaction spontaneous? At what T does it become spontaneous? B. What is Delta G at 450 K?
28.Consider a reaction for which ?H =-30.91 kJ/mol, ?S =-93.2J/K-mol. Which of the following statements is...
28.Consider a reaction for which ?H =-30.91 kJ/mol, ?S =-93.2J/K-mol. Which of the following statements is true? A)The reaction is spontaneous at all temperatures B)The reaction is spontaneous at low temperatures?332 K C)The reaction is spontaneous at high temperatures?332 K D)The reaction is spontaneous at high temperatures?3.02 K E)The reaction is never spontaneous 13.Calculate the pH of a buffer solution that is 0.250 M in HClO and 0.170 M KClO. The acid ionization constant for HClO at 298 K is...
HgO(s) Hg(g) O2(g) Enthaply Delta H kj/mol -90.8 61.3 Entropy Delta S   j/mol. K 70.3 174.9...
HgO(s) Hg(g) O2(g) Enthaply Delta H kj/mol -90.8 61.3 Entropy Delta S   j/mol. K 70.3 174.9 205.0 Above is a table of thermodynamics date for the chemical species in the reaction: 2HgO(s) ----> 2Hg(g)+ O2(g) at 25 C A) Calculate the molar entropy of reaction at 25 C B) Calculate the standard Gibbs free enregy of the reaction at 25 C given that the enthaply of reaction at 25 C is 304.2 Kj/mol C)Calculate the equilibrium constant for the reaction...
The enthalpy of a reaction is 50 kj/mol, and the enthaply is 223 J/K mol. What...
The enthalpy of a reaction is 50 kj/mol, and the enthaply is 223 J/K mol. What is the minimum temperature for this reaction to be spontaneous?
If delta H=-50.0kJ and deltaS=-0.500 kj/k, the reaction is spontaneous below a certian temperature. Calculate the...
If delta H=-50.0kJ and deltaS=-0.500 kj/k, the reaction is spontaneous below a certian temperature. Calculate the temperature express your answer numerically in kelvins
For the reaction 2NO(g) + O2(g) → 2NO2(g), ∆H° = -113.1 kJ/mol and ∆S° = -145.3...
For the reaction 2NO(g) + O2(g) → 2NO2(g), ∆H° = -113.1 kJ/mol and ∆S° = -145.3 J/K·mol. Under which temperature conditions would the reaction be spontaneous?
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT