Use the data in table 4 to calculate the ΔH⁰ and ΔS⁰ for the dissolution of KNO3. Show your workwith annotated calculations. Table 4: Selected thermochemical valuesAH+° (kJ/mol)Sº (J/K-mol)K+ (aq)-252.4102.5NO3(aq)-207.4146.4KNO3(s)-494.6133.1AH accepted =(include units)AS accepted =(include units)

The problem is asking us to calculate the enthalpy change (ΔH⁰) and entropy change (ΔS⁰) for the…

Answered: Table 4: Selected thermochemical values…

Table 4: Selected thermochemical values AH+° (kJ/mol) Sº (J/K-mol) K+ (aq) -252.4 102.5 NO3(aq) -207.4 146.4 KNO3(s) -494.6 133.1 AH accepted = (include units) AS accepted = (include units)

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: The equilibrium constant, K,, for the following reaction is 0.365 at 1150 K. 2502(g) + 02(g)…

A: 2 SO2(g) + O2(g) ↔ 2 SO3(g)At T1 =1150 KKp1 = 0.365At T2 = 1250 K∆H° = -198 kJKp2 = To be…

Q: What is the A,G for the following reaction (in kJ mol-¹) at 298 K? 2 NO2 (g) = N2O4 (g) The…

A: Standard Gibbs free energy of formation of NO2(g), ∆Gfo(NO2, g) = 51.3 kJ.mol-1 Standard Gibbs free…

Q: From the values given below, calculate the values of AG° and AH° for the following reaction at 25…

A: Information about the question

Q: What is the balanced chemical equation for the reaction used to calculate ΔfH∘ΔfH∘ of…

A: The standard enthalpy of formation of a compound is the change of enthalpy during the formation of 1…

Q: and ASO, calculate the AGO value for the re e reaction is spontaneous at standard conditi AH° (kJ)…

A: Given, □H° = -74.9 kJ □S° = 186.3 J/K T = 298 K □G° = □H° - T(□S°)/1000

Q: The change in enthalpy and entropy of the reaction below are -166 KJ and -284.8 J/K respectively. If…

A: Gibbs free energy of a reaction can be used to determine the spontaneity of a reaction. Write the…

Q: he free energy for a reaction can be related to the equilibrium constant through the formula below.…

A: For the dissociation of borax reaction, standard enthalpy change, ∆Ho = 188.69 kJ/mol standard…

Q: the following reaction: N204 2NO2 Kc = 0.212 at 100°C Calculate AG° in J mol for the reaction. (R =…

A: Equilibrium reactions are chemical reactions in which the reactions are processed in both the…

Q: A student determines the value of the equilibrium constant to be 7.86x10-37 for the following…

A: Given-> Keq = 7.86 × 10-37 Moles of H2S = 2.28 moles

Q: the free energy for a reaction can be related to the equilibrium constant through the formula below.…

A: When solid borax is added to water, the following equilibrium is established.…

Q: a) If the difference in the Gibbs free energy AG is -4.0 kJ mol¹ at 298 K. What is the Keq for this…

A: According to the question, The gibbes free energy ∆G° is given by = -4.0 kJ/molThe temperature is…

Q: Calculate ΔGrxn at 298 K under the conditions shown below for the following reaction. Remember what…

A: The given reaction is shown below: SO3(g) + H2O(g) → H2SO4(liq) Given information: ΔG°= -90.5 kJ…

Q: From the following series of reactions find the free energy of formation of N204(g) at 25°C: % N2(g)…

Q: Calculate the Gibbs free energy (in kJ) at 25 degrees C of the following reaction using the data in…

A: For a general reaction aA + bB → cc + dD…

Q: a) If the difference in the Gibbs free energy AG° is 3.5 kJ mol at 298 K. What is the Ken for this…

A: Standard free energy (∆G°) :- It is the free energy change accompanying a reaction at 298…

Q: 6-g A student determines the value of the equilibrium constant to be 1.69×1025 for the following…

Q: Calculate the DHf for the reaction below using the Born-Haber cycle. For thermodynamic data, check…

Q: (b) 4 CH,NH,(g) + 9 0,(g) → 4 CO,(g) + 10 H,O(€) + 2 N,(g) (c) Fe,0,(s) + 4 CO(g) → 3 Fe(s) + 4…

A: The standard free energy is denoted by the symbol ∆G∘. It is change in free energy which takes place…

Q: Calculate ΔGo at 91oC for the dissolution an ionic solid which has a Ksp of 2.2 x 10-8 at 91oC.…

Q: A chemist is studying the reaction below, 200, (g) + 4H,0 (g)-2CH,OH (g) + 30,; (g) The reaction…

A: Entropy is the measure of the degree of randomness of a system. More the randomness of a system,…

Q: Using the data from the previous steps, calculate the standard Gibbs Free Energy for the…

Q: For a C2D equilibrium reaction, if the enthalpy change in standard condition is 60 kJ/mol, if there…

A: The equilibrium reaction taking place is given as, => C ↔ 2 D Given: ΔH = 60 KJ/mol = 60000 J/mol…

Q: Chemistry Van't Hoff studied the temperature dependence of the equilibrium constant, K, using two…

A: The solution of the given question is

Q: A student determines the value of the equilibrium constant to be 4.76x1033 for the following…

A: Given data contains, The given reaction is, H2g+Cl2g→2HClg Equilibrium constant for the reaction is…

Q: 8. Use the free-energy information data on the table of Standard Thermodynamic Properties for…

Q: T5A.3- Calculate the standard reaction Gibbs free energy [in kJ/mol] at 341 K assuming that the…

A: T = 341 K ∆H = -322.5 kJ/mol ∆S = 126.7 J/K mol

Q: 2. Consider the equilibrium A(g) 2 B(g) +C(g) One mole of A is placed in a vessel at 298 K and…

A: The equilibrium reaction taking place is given as, => A (g) -------> B (g) + C (g) Given:…

Q: Explain what will happen in the following system if some SO3(g) is added: SO₂(g) + NO₂(g) = SO3(g) +…

A: According to Le Chatelier principle ,after attainment of equilibrium if we change the pressure…

Q: What are the effects of temperature changes on the spontaneously of reactions for which DelthaH is…

A: Several factors like enthalpy, entropy and temperature contribute to make a reaction spontaneous by…

Q: A student determines the value of the equilibrium constant to be 8.22x107 for the following…

A: Gibbs' equation ∆G=∆G°+RTlnK At equilibrium condition ∆G=0 So the first equation is reduced to…

Q: Calculate AS values for the following reactions by using tabulated Sº values from Appendix C. (a)…

Q: [References] What is the standard free-energy change AG at 25°C for the following reaction? H2 (9) +…

Q: Dinitrogen tetroxide decomposes to nitrogen dioxide: N2O4 (9) → 2 NO2 (g) A, H° 55.3 kJ mol-¹ At 298…

A: The balanced chemical equation is,N2O4(g) 2NO2(g) = 55.3 KJ/molIn…

Q: the free energy for a reaction can be related to the equilibrium constant through the formula below.…

A: Given: When solid borax is added to water, the following equilibrium is…

Q: help please answer in text form with proper workings and explanation for each and every part and…

A: The pressure equilibrium constant Kp for the reaction I2(g)+Cl2(g)→2ICl(g) can be written…

Q: of 16 For a gaseous reaction, standard conditions are 298 K and a partial pressure of 1 atm for all…

A: The given equilibrium reaction is N₂(g) + 3 H₂(g) 2NH3(g)The standard change in Gibbs free energy…

Q: gs. What nas nappe y Entropy ns constant Decreases ns constant Increases Increases ases ses…

A: When Ice is added into the hot water then, ice melts. The energy of hot water is used to melt the…

Q: 7. The equilibrium constant for the reac- tion N2(8) + O2(g) 2NO(g) at 2130°C is 2.5 × 10-3. Why is…

Q: how do I complete this? i am unsure of how to work this out.

A: The direct relation between the change in Gibbs Free Energy and the equilibrium constant is - ∆G =…

Q: e energy, what is th

A: The following areas terms are used in the plate design procedure:

Q: Consider the reaction 2NO(g) + O₂(9) 2NO₂(9) Using the standard thermodynamic data in the tables…

A: Answer: In the given reaction oxidation of NO into NO2 is taking place whose chemical equation is…

Q: The following reaction presents a ΔH0 and ΔG0 of 217.9 kJ/mol and 72.4 kJ/mol respectively, at 600…

A: ReactionCH4 (g) + H2O (g) → CO(g) + 3H2 (g)∆H° = 217.9 kJ /mol∆G° = 72.4 kJ/molTemperature = T = 600…

Q: calculate ΔG rxn at 325 K for the hypothetical reaction below A2B8 (g) + 3O2 (g) ----> 2AO (g) ΔH°f…

Q: 2. Using values of AH°; and S°, calculate AG°xn for the following reaction: NH3 (g) + HNO3(aq) →…

A: In this question, ∆H°f and ∆S°f for a reaction is given and ∆G°rxn is to be calculated. The given…

Q: Reaction AH at 298 K 3 Y + 2 X2O → 2 X2Y + YO2 146.9 kJ Y + O2 → YO2 - 296.4 kJ O -149.5 kJ O 443.3…

Question

Use the data in table 4 to calculate the ΔH⁰ and ΔS⁰ for the dissolution of KNO3. Show your work
with annotated calculations.

Table 4: Selected thermochemical values
AH+° (kJ/mol)
Sº (J/K-mol)
K+ (aq)
-252.4
102.5
NO3(aq)
-207.4
146.4
KNO3(s)
-494.6
133.1
AH accepted =
(include units)
AS accepted =
(include units)

AI-Generated Solution

AI-generated content may present inaccurate or offensive content that does not represent bartleby’s views.

Unlock instant AI solutions

Tap the button
to generate a solution

Click the button to generate
a solution

SEE SOLUTION

Similar questions

NH3(aq) + H2O (l) ⇆ NH4+(aq) + OH- (aq) 1. If the Kb for this reaction at 298K is 1.8 x 10-5, calculate ΔG⁰ (R= 8.314J/mol K)
Gibbs’ Free Energy and Equilibrium ConstantSolve the following problems. Show your solution. 3. Calculate the equilibrium constant for the following reaction at 298 K.3C2H2 (g) ↔ C6H6 (g)ΔG° +209.97 +129.7
At 25oC, Ka for acid dissociation of aspiring (C9H8O4) is 3.0 x 10-4. Calculate ΔGo for the reaction C9H8O4 (aq) + H2O(l) H3O+(aq) + C8H7O4-(aq)
Determine spontaneity of each reactions. Calculate Gibbs free energy. Sn+4 + Fe+2 → Sn+2 + Fe 3Sn+4 + 2Cr → 2Cr+3 + 3Sn+2 3Fe+2 → Fe + 2Fe+3
Calculate the Gibbs free energy
a) For a reaction with AH = -152.6 kJ mol-¹ and AS°= -543.8 J K-¹ mol-¹ at 25 °C, how will AGº change if the reaction temperature is increased? Explain your answer. b) Calculate the equilibrium constant for the reaction at 80 °C, showing your working (assume AH and AS° are temperature independent).
Calculate the value of ΔdissolveG0 from the values of ΔdissolveH0 and ΔdissolveS0 and comment on the spontaneity of the dissolution process. ΔoplosG0/kJ mol-1 = ΔoplosH0-TΔoplosS0 = 19.69 kJ mol-1 - (298.15 K) x (80.15 x 10-3 kJ K-1 mol-1) = -4.21 kJ m comment:
Using Delta H° Delta S°, calculate Delta Go and K for the following reaction:HBr(g) + Cl2(g) ---> HCl(g) + Br2(l)What type of reaction is this? Is it spontaneous at room temperature? If it is a type 2 or 3, calculate at what temperature it will be at equilibrium. *open image for clarification*
6
Predict whether reaction would proceed spontaneously or not for the following system at 298 K and write net reaction for each? Write the net equation for each sample. (Eo for Cu2+/Cu:0.34, Ag+/Ag: +0.8, NO3-/NO:+0.96) Metallic silver in 1 M HNO3 Metallic copper in 1 M HCl
Consider the vaporization of carbon disulfide. CS₂ (1) = CS₂(g) Free energies and enthalpies of formation can be found here Calculate the standard free energy for this reaction and the standard enthalpy for this reaction. AG = K25C 2.5 Calculate the equilibrium constants for this reaction at 25 °C and at CS₂'s normal boiling point. Tbp 0.346 Incorrect Calculate the normal boiling point of CS₂. 290.322 kJ/mol Incorrect ΔΗ° = 27.7 °C Kbp 0.355 Incorrect kJ/mol
What’s the answer for this