Question

For a particular reaction at 128.1 °C, ΔG = 377.52 kJ/mol, and ΔS = 556.72 J/(mol·K)....

For a particular reaction at 128.1 °C, ΔG = 377.52 kJ/mol, and ΔS = 556.72 J/(mol·K).

Calculate ΔG for this reaction at -78.3 °C.

= ? kJ / mol

Homework Answers

Answer #1

ΔG     = ΔH -TΔS

T   = 128.1 C0   = 128.1+273   = 401.1K

ΔG = 377.52 kJ/mol,

ΔS = 556.72 J/(mol·K)   = 0.55672Kj/mole-K

ΔG     = ΔH -TΔS

377.52 = ΔH -401.1*0.556.72

ΔH = 377.52+401.1*0.556.72   = 600.82KJ

T = -78.3 °C.   = -78.3+273 = 194.7K

ΔG     = ΔH -TΔS

         = 600.82-194.7*0.55672   =492.43Kj/mole

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 at 221.9 °C, ΔG = -92.39 kJ/mol, and ΔS = 130.33 J/(mol·K)....
For a particular reaction at 221.9 °C, ΔG = -92.39 kJ/mol, and ΔS = 130.33 J/(mol·K). Calculate ΔG for this reaction at -54.3 °C. ____________ kJ/mol
For a particular reaction at 188.9 °C, ΔG = 287.40 kJ/mol, and ΔS = 811.42 J/(mol·K)....
For a particular reaction at 188.9 °C, ΔG = 287.40 kJ/mol, and ΔS = 811.42 J/(mol·K). Calculate ΔG for this reaction at 4.1 °C.
For a particular reaction at 152.8 °C, ΔG = -966.13 kJ/mol, and ΔS = 459.28 J/(mol·K)....
For a particular reaction at 152.8 °C, ΔG = -966.13 kJ/mol, and ΔS = 459.28 J/(mol·K). Calculate ΔG for this reaction at -54.9 °C.
For a particular reaction at 132.0 °C, ΔG = 496.12 kJ/mol, and ΔS = 302.61 J/(mol·K)....
For a particular reaction at 132.0 °C, ΔG = 496.12 kJ/mol, and ΔS = 302.61 J/(mol·K). Calculate ΔG for this reaction at 0.4 °C.
For a particular reaction at 111.6 °C, ΔG = 131.35 kJ/mol, and ΔS = 201.60 J/(mol·K)....
For a particular reaction at 111.6 °C, ΔG = 131.35 kJ/mol, and ΔS = 201.60 J/(mol·K). Calculate ΔG for this reaction at -25.3 °C.
Consider the reaction: Ca(s) + 2 H2O(ℓ) → Ca(OH)2(aq) + 2H2(g) ΔfH°(kJ/mol) 0 -285.83 -1002.82 0...
Consider the reaction: Ca(s) + 2 H2O(ℓ) → Ca(OH)2(aq) + 2H2(g) ΔfH°(kJ/mol) 0 -285.83 -1002.82 0 S°(J/K·mol) 41.59 69.95 -74.5 130.7 What are the values of ΔH°, ΔS° and ΔG° ΔH° =   kJ/mol ΔS° =   J/mol·K ΔG° =   kJ/mol
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
Calculate ΔG∘ (in kJ/mol) for the following reaction at 1 atm and 25 °C: C2H6 (g)...
Calculate ΔG∘ (in kJ/mol) for the following reaction at 1 atm and 25 °C: C2H6 (g) + O2 (g)  → CO2 (g) + H2O (l) (unbalanced) ΔHf C2H6 (g) = -84.7 kJ/mol; S C2H6 (g) = 229.5 J/K⋅mol; ΔHf ∘ CO2 (g) = -393.5 kJ/mol; S CO2 (g) = 213.6 J/K⋅mol; ΔHf H2O (l) = -285.8 kJ/mol; SH2O (l) = 69.9 J/K⋅mol; SO2 (g) = 205.0 J/K⋅mol
What can be concluded about a chemical reaction with ΔH = 9.3 kJ/mol & ΔS =...
What can be concluded about a chemical reaction with ΔH = 9.3 kJ/mol & ΔS = 31 J/mol·K at 27°C? The reaction will proceed spontaneously in the reverse direction as written. The reaction will proceed spontaneously in the forward direction as written. The reaction is already at equilibrium and so neither the forward not the reverse reaction can occur. It is impossible to make conclusions about what direction the reaction will proceed without further information. The reaction is already at...
Use data in Appendix C in the textbook to calculate ΔH∘ in (kJ/mol) , ΔS∘ in...
Use data in Appendix C in the textbook to calculate ΔH∘ in (kJ/mol) , ΔS∘ in (j/mol-K) , and ΔG∘ in (kJ/mol) at 25 ∘C for each of the following reactions: 2P(g)+10HF(g)→2PF5(g)+5H2(g) Appendix C: P(g): dH:316.4; dG: 280.0; S:163.2 HF(g): dH: -268.61; dG: -270.70; S:173.51 PF5(g): dH:-1594.4; dG: -1520.7; S: 300.8 H2(g): dH:217.94; dG: 203.26; S: 114.60