In the gas phase, formic acid forms a dimer, \(2 \text{HCOOH(g)} \rightleftharpoons (\text{HCOOH})_2\text{(g)}\). For this reaction, \(\Delta H^\circ = -60.1 \ \text{kJ/mol}\) and \(\Delta G^\circ = -13.9 \ \text{kJ/mol}\) at 25°C. Find the equilibrium constant (\(K_p\)) for this reaction at 75°C.

Answered: Image /qna-images/answer/9439d6a9-1cde-4ae4-a1de-fdee4cc06809.jpg

In the gas phase, formic acid forms a dimer, 2HCOOH(g) (HCOOH)2(g). For this reaction, ΔΗ -60.1 kJ/mol and AG = -13.9 kJ/mol at 25°C. Find the equilibrium constant (Kp) for this reaction at 75 °C. =

In the gas phase, formic acid forms a dimer, 2HCOOH(g) (HCOOH)2(g). For this reaction, ΔΗ -60.1 kJ/mol and AG = -13.9 kJ/mol at 25°C. Find the equilibrium constant (Kp) for this reaction at 75 °C. =

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Related questions

Q: Calculate AG° xn indicated in the following reaction using the given information. CiO(g)…

Q: Question 3 : We start with a sample of pure A(g). The following equilibrium is established 2 A(g)…

A: Answer: In this question, with the help of given data, we will calculate the value of equilibrium…

Q: At 460 K, AG = -10.90 kJ/mol for the reaction 2 A (g) → B (g). If the partial pressures of A and B…

Q: НО + ELOH Rho = 2.61 H2O/EŁOH

A: Generally, the information of sign and magnitude of reaction constant rho value is determined with…

Q: A) Write the equalibrium expression for N2 + 3H2----> 2NH3 NH3= .2 N2= .01 H2= .1 b) which is…

Q: Calculate AG°rxn for the reaction below at 25.0 °C CO(g) + H2O(1) → H2(g) + CO2(g) given AG°f…

A: Given reaction is, CO(g) + H2O(l) →H2(g) + CO2(g) Given data, ∆Gof[CO(g)] = -137.2 KJ/mol…

Q: 2. Calculate the temperature at which the reaction below will be at equilibrium Given . Br2(l) →…

A: Since the value of ΔG becomes = 0 at equilibrium And since ΔG = ΔH - TΔS where T is in Kelvin ΔH =…

Q: A student determines the value of the equilibrium constant to be 4.54x10-15 for the following…

A: As ∆G = - RT ln K If k < 1 then ∆G = +ve & If k >1 then ∆G = -ve For the given…

Q: If AG°rxn is 10.9 kJ/mol, determine AGxn at 525 K, when TiCl4(g) = 0.750 atm. TiClą(liq) → TİC|«(g)…

Q: For the following reaction, 10.7 grams of nitrogen monoxide are allowed to react with 9.54 grams of…

A: The following is the equation of the given chemical reaction. 2NO(g) + O2(g) → 2NO2 (g) One mole of…

Q: Determine the equilibrium constant for a reaction at 200 K if AG° =17.7 kJ/mol. (R = 8.314 J/mol K)

A: The relationship between ΔGo and equilibrium constant (K) is ΔGo = -RT lnK

Q: Given AG°F [NO] = 87 kJ/mol and AG°F [N2O] = 104 kJ/mol, what is AG° for the following reaction? 4…

A: ΔGf for dioxygen is zero.

Q: The standard reaction free energy AG =-800. kJ for this reaction: CH (9) + 20,(g)→CO,(g) + 2 H,0(g)…

Q: An endothermic reaction is carried out under standard conditions. The equilibrium constant, Keq, for…

A: Answer: Below shown relation will be used to calculate Standard Gibbs free energy change:…

Q: 13 of 48 Calculate AG° for the reaction, 2C2H2(9)+302(g)→4CO(g)+2H2O(g), given AG°; for…

A: The given chemical reaction is: 2C2H2(g) + 3O2(g) → 4CO(g) + 2H2O(g) The values of ∆Gof for all the…

Q: Gibbs’ Free Energy and Equilibrium Constant Solve the following problems. Show your solution. 1.…

Q: Consider the following reactions: A= B, Kı=6.02 A= C, K2=2.00 What is K for the reaction C= B?

Q: This reaction has K = 2.3 * 10-18. Are the reactants or the products favored?

A: The given value of K is 2.3 × 10-18

Q: Calculate the equilibrium constant (K) for the following reaction at 298 K using the given free…

Q: Consider a general reaction enzyme A(aq) = = B(aq) The AGO of the reaction is -5.250 kJ. mol-¹.…

Q: (Q80) The enthalpy of vaporization (AH°vap) of water is 44.0 kJ/mol. If the equilibrium constant for…

Q: The equilibrium constant for a particular reaction has a value of 7.40 × 10−4 at a temperature of…

A: Equilibrium constant, K = 7.40 × 10-4 Temperature , T = 24.4°C = ( 24.4 + 273)K = 297.4 K…

Q: The equilibrium constant, Kp, for the following reaction is 0.636 at 600 K. CoCl2(g) ? CO(g) +…

A: The objective of this question is to find the value of the equilibrium constant, Kp, at a different…

Q: (Q78) The equilibrium constant (Keg) for the formation of dinitrogen tetroxide (N2O4) from nitrogen…

Q: Calculate ΔG° using the following reaction and information below . CH3CH2OH(g) + 3O2(g) ---> 2CO2(g)…

A: The relation between ΔG°, ΔH°, and ΔS° is as follows ΔG°=ΔH° – TΔS° Where T is temperature and…

Q: 3 The synthesis of methanol from carbon dioxide and hydrogen has a AG°= -25.1 kJ/mol. What is the…

A: At equilibrium Gibbs free energy ∆G0 = - RT ln K ∆G0= - 25.1 KJ / mol R = 0.008314 KJ / mol k T =…

Q: A student determines the value of the equilibrium constant to be 2.57×10-10 for the following…

A: Fe2O3 + 3H2 ---> 2Fe + 3H2O T = 298 K R = 8.314 J/mol Keq = 2.57 × 10-10

Q: Consider the following reaction: 4NH3(aq) + 5O2(g) ⇌ 6H2O(g) + 4NO(g) a. Calculate ΔG0 at 25°C…

A: The standard Gibbs free energy of a reaction is calculated as: ∆G°=∑n∆G°f (products)-∑m∆G°f…

Q: 23. Predict whether this reaction is product-favored at 25°C by calculating the change in standard…

A: Use Gibbs free energy equation to determine the reaction is spontaneous or non-spontaneous. If delta…

Q: 4. Does growth of corals: Ca²+ + CO3²- → CaCO3(s) cause atmospheric CO2 to increase or decrease?…

A: Growth of corals will decrease the atmosphere CO2

Q: The equilibrium constant, K,, for the following reaction is 0.160 at 298 K. 2NOBr(g) 2NO(g) + Br2(g)…

A: Given that: K1 = 0.160 T1 = 298 K T2 = 420 K ΔH = 16.1 kJ= 16100 J To find the values of…

Q: What is AG° for the reaction CH,OH(g) → CO(g) + 2 H,(g) at 25°C? kJ/mol AH° = +90.7 kJ/mol 3 AS° =…

Q: Calculate the AH°, AS°, and AG at 298 K for the following reaction: (Use the values found in…

Q: Using the information from appendix G, calculate the value of K for the following equilibrium at…

Q: e standard Gibbs Free Energy, AG n rxn, for th

A: The standard Gibbs free energy of formation of a compound is the change of Gibbs free energy that…

Q: Calculate the value of Δ?∘rxnΔGrxn∘ for the following reaction at 278 K. Ka = 2.9 × 10–8 and assume…

A: delta G is known as free energy of thermodynamical system , it is used to find maximum reversible…

Q: Use the information below to calculate ΔG°298 for the following reaction: NO (g) + O (g) ⇌ NO2…

A: The given data's are: 2 O3 (g) ⇌ 3 O2 (g) ΔG°298 = +489.6 kJ…

Q: A reaction has a standard free-energy change of-13.20 kJ mol*(-3.155 kcal mol¯*). Calculate the…

Q: consider dissolution of calcium fluoride at 25C. what is the ΔG (kj/mol) for the formation of…

A: Given,Ksp of CaF2 = Temperature (T)= Gas constant (R)= To find the for the formation of CaF2.

Q: The equilibrium constant for a particular reaction has a value of 4.84 × 10−5 at a temperature of…

A: Equilibrium constant (k) = 4.84×10-5 Temperature (T) = 20.1°C = (20.1+273.15) K T = 293.25 K ΔG° = ?…

Q: The equilibrium constant for the reaction N204 (g) =* 2 NO2 (g) is 0.200 at 65 °C. Calculate AG° for…

A: Given :- N2O4(g) <-----> 2NO2(g) K = 0.200 T = 65°C To calculate :- ∆G° for this reaction

Question

In the gas phase, formic acid forms a dimer, \(2 \text{HCOOH(g)} \rightleftharpoons (\text{HCOOH})_2\text{(g)}\). For this reaction, \(\Delta H^\circ = -60.1 \ \text{kJ/mol}\) and \(\Delta G^\circ = -13.9 \ \text{kJ/mol}\) at 25°C. Find the equilibrium constant (\(K_p\)) for this reaction at 75°C.

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 2 steps with 2 images

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

For the reaction below, the AH° = -113.1 kJ/mol and AS = -145.3 J/K-mol. Calculate the equilibrium constant, K, for this reaction at 25°C. 2NO(g) + O2(g) 2NO2(g)
Given the following information below, determine AGxn at equilibrium. 12(g) + Cl2(g) 2 ICI(g) 11 K, = 81.9 (at 298 K) O 1 O +10.9 kJ O -10.9 kJ
Calculate E∘cell�cell∘ for a redox reaction with n� = 2 that has an equilibrium constant of K� = 24 (at 25 ∘C∘C). Calculate ΔrG∘Δr�∘ for a redox reaction with n� = 2 that has an equilibrium constant of K� = 24 (at 25 ∘C∘C).
If AG°rxn is 10.9 kJ/mol, determine AGrxn at 525 K, when TiCl4(g) = 0.250 atm. TiClą(liq) →TICI4(g)
For a chemical reaction, Keg at 373 K is 94.7. Calculate AG°373 (in kJ). O - 14.1 O + 6.13 - 294 + 14.1 O- 6.13
Determine the temperature of a reaction if K = 1.20 x 106 when AG° = +22.70 kJ/mol.
7. AG° = -49.6 kJ at 25 °C for the Haber process. What is the value of the equilibrium constant at this temperature? N2 (g) + 3 H2 (B) t 2 NH) (g)
Determine the AG° for the reaction of hydrogen and oxygen to form water. 2H2 (g) + O2 (g)→ 2H2O (g) AS°= -89.0 J/K AH°= -483.6 KJ
What is AG° for the reaction CH₂OH(g) → CO(g) + 2 H₂(g) at 25°C? AH° = +90.7 kJ/mol kJ/mol
In the Haber process, ammonia is synthesized from nitrogen and hydrogen: N2(8) + 3H2(g) → 2NH3(g) AG° at 298 K for this reaction is -33.3 kJ/mol. The value of AG at 298 K for a reaction mixture that consists of 1.9 atm N2, 1.6 atm H2, and 0.65 atm NH3 is O -1.8 O -104.5 O-3.86 x 103 O-7.25 x 10 -40.5
Calculate the temperature at which the reaction below will be at equilibrium, then explain how this temperature can affect the spontaneity, meaning how using higher or lower than this temp can affect the value of delta G. Given. Br2(l) → Br2 (g), ΔH = 31.0 kj/mol ΔS = 92.9 j/mol
What is the equilibrium constant for a reaction at 25 degrees Celsius. The value of delta G is -56.8kJ/mol