Question

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?

Homework Answers

Answer #1

5)

A)

deltaH = -45.0KJ

deltaS = -103J/K

= -0.103 KJ/K

we have below equation to be used:

deltaG = deltaH - T*deltaS

for reaction to be spontaneous, deltaG should be negative

that is deltaG<0

since deltaG = deltaH - T*deltaS

so, deltaH - T*deltaS < 0

-45.0- T *-0.103 < 0

T *0.103 < 45.0

T < 437 K

So, the reaction will be spontaneous at standard temperature as well which is 273 L

Answer: yes

B)

deltaH = -45.0KJ

deltaS = -103J/K

= -0.103 KJ/K

T = 450 K

we have below equation to be used:

deltaG = deltaH - T*deltaS

deltaG = -45.0 - 450.0 * -0.103

deltaG = 1.35 KJ

Answer: 1.35 KJ

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
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
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 I2(s)--->2I(g), delta Ho=+213.6 kJ and delta So=+245.2 J/K. (a) Calculate delta Go. Is...
For the reaction I2(s)--->2I(g), delta Ho=+213.6 kJ and delta So=+245.2 J/K. (a) Calculate delta Go. Is the reaction spontaneous at this temp? Is the reaction spontaneous at this temp? (b) Calculate delta G at 250o C. is the reaction spontaneous at this temp? (c) At what Celcius temp will this reaction be spontaneous? (d) Calculate the thermodynamic equilibrium constant for this reaction at 25oC. Will this be Kp or Kc ? (e) If this reaction occurred in a closed vessel...
Calculate delta G at 82 C for reactions in which a. delta H = 293 kj...
Calculate delta G at 82 C for reactions in which a. delta H = 293 kj delta S = -695 J/K b. delta H = -1137 kJ; delta S = 0.496 kJ/K c. delta H = -86.6 kJ; delta S = -382 J/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.
given the following information A+B->2D delta H=-710.9kJ delta S= 298.0J/K C->D     delta H =515kJ delta S=-192...
given the following information A+B->2D delta H=-710.9kJ delta S= 298.0J/K C->D     delta H =515kJ delta S=-192 J/K calculate the delta G for the following reaction at 298K. A+B->2C **PLEASE SHOW WORK**
calculate the standard free energy change delta G for reaction N2 (g) +3H2(g)—>2NH3 N2 delta H=0.00kj...
calculate the standard free energy change delta G for reaction N2 (g) +3H2(g)—>2NH3 N2 delta H=0.00kj mol^-1s=+191.5J mol^-1K^-1 H2 delta H=0.00kj mol^-1,s = +130.6j mol^-1 k-1 NH3 delta H=-46.0kj mol^-1,s =192.5 J mol^-1 k-1 A. +112.3 kJ B.-87.6kJ C.-7.4kJ D.-32.9 kJ E.-151.1kJ
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...
Apply the Free Energy equation to identify whether reactions with the following values of delta H...
Apply the Free Energy equation to identify whether reactions with the following values of delta H and Delta S are spontaneous or nonspontaneous and whether they are exothermic or endothermic: a. delta H = -128 kJ; delta S = 35 J/K at 500k b. delta H = +67kJ; delta S= -140 J/K at 250k c. delta H = +75 kJ; delta S = 95J/K at 800k
Consider the following reaction. CH3OH(g) CO(g) + 2 H2(g) DELTA-H = +90.7 kJ (a) Is the...
Consider the following reaction. CH3OH(g) CO(g) + 2 H2(g) DELTA-H = +90.7 kJ (a) Is the reaction exothermic or endothermic? (b) Calculate the amount of heat transferred when 45.0 g of CH3OH(g) are decomposed by this reaction at constant pressure. DELTA-H =___ kJ (c) If the enthalpy change is 20.0 kJ, how many grams of hydrogen gas are produced? _____g (d) How many kilojoules of heat are released when 11.5 g of CO(g) reacts completely with H2(g) to form CH3OH(g)...