ZuoTi.Pro
Question

Reactions in which a substance decomposes by losing CO2 are called decarboxylation reactions. The decarboxylation of...

Reactions in which a substance decomposes by losing CO2 are called decarboxylation reactions. The decarboxylation of acetic acid proceeds as follows.

CH3COOH(l)-->CH4(g)+CO2(g)

Calculate the minimum temperature at which this process will be spontaneous under standard conditions. Assume that ΔH° and ΔS° do not vary with temperature. (CH3COOH(l): ΔH°f=-487.0 kj/mol, ΔS°=159.8J/mol K).

science   chemistry   
0 0
Add a comment Improve this question Transcribed image text
Next > < Previous
Sort answers by oldest

Homework Answers

Answer #1

Given equation: CH,COOH(I)-> CH4(g)+CO2 (g) Enthalpy of reaction, AH 487.0kJ-mol1 Change in entropy, AS -159.8J-mol1 K-1 Calc

1 1
Add a comment
Know the answer?
Add Answer to:
Reactions in which a substance decomposes by losing CO2 are called decarboxylation reactions. The decarboxylation of...
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for? Ask your own homework help question. Our experts will answer your question WITHIN MINUTES for Free.
Similar Homework Help Questions

  • 1a) For which of the following reactions is ΔSo > 0? a. 2 C2H6(g) + 7...

    1a) For which of the following reactions is ΔSo > 0? a. 2 C2H6(g) + 7 O2(g) à 4 CO2(g) + 6 H2O(g) b. H2CO(g) + O2(g) à CO2(g) + H2O(l) c. N2(g) + 3 H2(g) à 2 NH3(g) d. NH3(g) + HI(g) à NH4I(s) 1b) For a particular chemical reaction ΔH = 7.0 kJ and ΔS = –17 J/K. Under what temperature condition is the reaction spontaneous? a) When T > 412 K. b) The reaction is not spontaneous...

  • Why a Substance Can Be a Liquid at Room Temperature? Calculate ΔS∘total for the evaporation of...

    Why a Substance Can Be a Liquid at Room Temperature? Calculate ΔS∘total for the evaporation of water at 25∘C. H2O (l) ⇄ H2O (g) ΔH∘f (kJ/mol) Sm∘ (J/mol*K) H2O (l) - 285.830 69.91 H2O (g) - 241.818 188.83 ΔS∘ system? ΔS∘surroundings? ΔS∘total?

  • Substance BaCO3(s) | BaO(s) CO2(g) BaCO3(s) = Bao(s) + CO2(g) A.HⓇ/kJ mol -1213.0 -548.0 -393.5 Sº...

    Substance BaCO3(s) | BaO(s) CO2(g) BaCO3(s) = Bao(s) + CO2(g) A.HⓇ/kJ mol -1213.0 -548.0 -393.5 Sº / 1 mol K- 112.1 72.1 213.8 a. Using the information in the table above, show that the reaction is not spontaneous under standard conditions by calculating 4,Gº. {5 marks) b. If Baco, is placed in an evacuated flask, what partial pressure of CO2 will be present when the reaction reaches equilibrium? (3 marks) c. Can the reaction be made more spontaneous by an...

  • H2 reacts with the halogens (X2) according to the reaction: H2(g)+X2(g)⇌2HX(g) where X2 can be Cl...

    H2 reacts with the halogens (X2) according to the reaction: H2(g)+X2(g)⇌2HX(g) where X2 can be Cl2, Br2, or I2. Reactant/Product   ΔH∘f(kJ/mol)   ΔS∘f(J/mol⋅K) H2(g)   0   130.7 Cl2(g)   0   223.1 HCl(g)   -92.3   186.9 Br2(g)   30.9   245.5 HBr(g)   -36.3   198.7 I2(g)   62.42   260.69 HI(g)   26.5   206.6 Part A Calculate ΔH∘ for the reaction between hydrogen and Cl2. Express your answer using four significant figures. ΔH∘ Δ H ∘ =    kJ Previous AnswersRequest Answer Incorrect; Try Again; 11 attempts remaining Part B Calculate ΔS∘...

  • For reactions carried out under standard-state conditions, the equation ΔG = ΔH − TΔS becomes ΔG°...

    For reactions carried out under standard-state conditions, the equation ΔG = ΔH − TΔS becomes ΔG° = H° − TΔS°. Assuming ΔH° and ΔS° are independent of temperature, one can derive the equation: ln( K2 K1 ) = ΔH° R ( T2 − T1 T1T2 ) where K1 and K2 are the equilibrium constants at T1 and T2, respectively. Given that at 25.0°C, Kc is 4.63×10−3 for the reaction N2O4(g) longrightleftarrow 2NO2(g) ΔH° = 58.0 kJ/mol calculate the equilibrium constant...

  • Here are the delta H, delta S and delta G values from my textbook: (first value...

    Here are the delta H, delta S and delta G values from my textbook: (first value is delta H, second value is delta S, third is delta G) CO2: -393.5 , 213.6 , -394.4 CH4: -75, 186, -51 CO : -110.5 , 197.9 , -137.3 CH3COOH : -484.2 , 159.8 , -389.45 CH3OH : -238 , 126.8 , -166.3 Q3. Using the thermodynamics data given in the appendix, calculate ΔH·AS) and ΔG, for the following reactions that produce acetic acid:...

  • Methane can react with water to form carbon dioxide and hydrogen according to the following equation:...

    Methane can react with water to form carbon dioxide and hydrogen according to the following equation: CH4(g) + 2H2O(g) ↔ CO2(g) + 4H2(g) Use the following thermodynamic data at 298 K to determine the temperature at which the reaction goes from being spontaneous to nonspontaneous. Substance CH4(g) H2O(g) CO2(g) H2(g) ΔHºf (kJ/mol) -74.87 -241.8 -393.5 0 ΔGºf (kJ/mol) -50.81 -228.6 -394.4 0 Sºf (J/Kmol) 186.1 188.8 213.7 130.7

  • At equilibrium, the free energy change, ΔG, of any system is zero: ΔG=0=ΔH−TΔS So, under equilibrium...

    At equilibrium, the free energy change, ΔG, of any system is zero: ΔG=0=ΔH−TΔS So, under equilibrium conditions, this equation can be rearranged as T=ΔHΔS Part A Glacial acetic acid is the concentrated form of acetic acid, the acid in vinegar. The term "glacial" refers to the appearance of the solid form, which resembles glacial ice. What is the melting point of this compound, in degrees Celsius, based on its thermodynamic data shown here? ΔHfus (kJ/mol) = 24.32 ΔSfus [J/(K⋅mol)] =...

  • 2. For the following example, identify the following. H2O(l) → H2O(s) question 2 options a negative...

    2. For the following example, identify the following. H2O(l) → H2O(s) question 2 options a negative ΔH and a negative ΔS a positive ΔH and a negative ΔS a negative ΔH and a positive ΔS a positive ΔH and a positive ΔS It is not possible to determine without more information. 3. Calculate ΔS°rxn for the following reaction. The S° for each species is shown below the reaction. C2H2(g) + H2(g) → C2H4(g) S°(J/mol∙K) 200.9 130.7 219.3 Question 4 options:...

  • 1) Moles of CO2 required to inflate 80-L driver-side air bag at room temperature and pressure...

    1) Moles of CO2 required to inflate 80-L driver-side air bag at room temperature and pressure 2) Balanced equation for the reaction of NaHCO3 and CH3COOH to CO2 3) Mass of NaHCO3 needed for the reaction (84.0 g/mol) 4)Volume of vinegar required (0.833 M acetic acid)

ADVERTISEMENT
Free Homework Help App
Download From Google Play
Scan Your Homework
to Get Instant Free Answers
Need Online Homework Help?
Ask a Question
Get Answers For Free
Most questions answered within 3 hours.
ADVERTISEMENT
ADVERTISEMENT
ADVERTISEMENT