### Calculating Standard Entropy Change for the Reaction:**Reaction:**\[ \text{H}_2(\text{g}) + \text{Br}_2(\text{l}) \rightarrow 2 \text{HBr}(\text{g}) \]To find the value of standard entropy change, ΔSº, for the reaction, we use the given standard thermodynamic properties of the substances involved.**Given Table:**#### Standard Thermodynamic Properties for Selected Substances| Substance | \(\Delta H_f^\circ\) (kJ mol⁻¹) | \(\Delta G_f^\circ\) (kJ mol⁻¹) | \(S^\circ\) (J K⁻¹ mol⁻¹) ||-----------|---------------------|-----------------------|-------------------------------|| \(\text{Br}_2(\text{l})\) | 0 | 0 | 152.23 || \(\text{Br}_2(\text{g})\) | 30.91 | 3.142 | 245.5 || \(\text{Br}(\text{g})\) | 111.88 | 82.429 | 175.0 || \(\text{Br}^-\) (aq) | -120.9 | -102.82 | 80.71 || \(\text{BrF}_3(\text{g})\) | -255.60 | -229.45 | 292.42 || \(\text{HBr}(\text{g})\) | -36.3 | -53.43 | 198.7 |#### Steps to Calculate \(\Delta S^\circ_{\text{reaction}}\):1. **Identify the standard entropy values (\(S^\circ\)) for each substance:** - \(S^\circ (\text{H}_2(\text{g}))\) = **Assumed Known for Calculation** - \(S^\circ (\text{Br}_2(\text{l}))\) = 152.23 J K⁻¹ mol⁻¹ - \(S^\circ (\text{HBr}(\text{g}))\) = 198.7 J K⁻¹ mol⁻¹2. **Apply the formula for the standard entropy change:** \[ \Delta

Answered: Image /qna-images/answer/d5f31a32-2f0b-4454-aec6-e3277741ce5b.jpg

Answered: Use the table below to answer the…

Use the table below to answer the questions that follow. The value of standard entropy change, AS°, for the following reaction, H2(g) + Br2(1) → 2 HBr(g) is J/K.

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: Using Thermochemical Data, calculate ΔS for the following reaction. Is entropy increasing or…

A: ANSWER IS

Q: ) True or False? If false, correct the statement. a) The entropy of a substance increases…

A: The entropy of a substance increases when a substance changes from liquid to vapor at any…

Q: At 25°C, the formation of ammonia from its elements results in a decrease in entropy (∆SRXN = -197…

A: According to the question about the formation of ammonia we have, The Change (decrease) in the…

Q: Consider the following reaction for the production of hydrogen cyanide. NH3 (g) + S(s) + CH4…

Q: Consider the balanced reaction 3 A + 7 B → 3 C + 7 D and the absolute entropies provided in the…

Q: For a particular reaction at 187.3 °C, AG = -989.95 kJ, and AS = 662.97 J/K. Calculate AG for this…

Q: 1) Which of the following statements is TRUE? A) ASuniverse is always greater than zero for a…

A: The condition of spontaneity of a reaction is that overall change in Gibbs free energy should be…

Q: The heat of vaporization of carbon disulfide, CS2, at 25 C is 27.2 Kj/mol. What is the entrophy…

Q: At 25°C, the formation of ammonia from its elements results in a decrease in entropy (∆SRXN = -197…

A: we have to calculate the value of ∆SUNIV

Q: Lighters are usually fueled by butane(C4H1O). When 1 mole of butane burns at constant pressure it…

A: Given: Moles of butane= 1 mol Heat produced =2658 kJ Amount of work done=3 kJ To Calculate: the…

Q: Calcium oxide (CaO), also called quicklime is prepared by decomposing limestone (CaCO3) in a kiln at…

A: We can calculate Gibbs free energy by using formula ∆G= ∆H - T×∆S Where ∆G = Gibbs free energy…

Q: What is the entropy change (in J/K) associated with the formation of 15.0 g of SO2 for the reaction…

Q: The addition of 121 g potassium fluoride to 591 mL of water (d = 1.00 g/mL) causes the temperature…

A: The mass of solution is calculated as shown,

Q: Use data from Appendix IIB to calculate ΔS∘rxnΔSrxn∘ for each of the reactions given.…

Q: Read the descriptions of physical or chemical changes in the table below. Then decide whether the…

A: Q1. Since the reaction is endothermic, that means you have to provide heat during the reaction,…

Q: Predict the sign of ∆S for physical and chemical processes?

A: Solution : Entropy is a thermodynamic property that is a quantitative measure of the randomness…

Q: Predict the sign of ΔSfor these processes: 2 H2(g) + O2(g) → 2 H2O(l) H2O(l) → H2O(s) CaCO3(s) →…

A: Entropy of gases is higher than of liquid and solid. Order of entropy gas> liquid >solid

Q: Predict the sign of ΔU, q, and w in the reaction given. 2C₆H₆ (s) + 7O₂ (g) → 4CO₂ (g) + 6H₂O (g)

A: ∆U = +ve q = +ve w = -ve

Q: For the reaction below AH = +92.2 kJ, and AS = +198.7 J/K. Estimate the temperature at which this…

A: To find the temperature.

Q: Calculate AS° for the following reaction. N2( g) + 2 O2( 9) → 2 NO2( g) S°, J/(K · mol) 191.5…

Q: In freezing a mole of liquid water at the freezing point; the enthalpy of fusion is 6.0lkJ/mol…

A: The enthalpy of fusion is 6.01 KJ/mol To determine : entropy of system , surrounding and universe

Q: Сalculate ∆H° for the reaction: N2O(g) + 1/2 O2(g) → 2NO(g)

Q: Consider the following half-reactions: F2(g) + 2 e ® 2 F(aq) E° = +2.87 V Cu2+(aq) + 2 e ® Cu(s)…

A: You have asked multiple type questions, we will solve only first questions for you. If you want any…

Q: For a particular reaction, Δ?∘=−28.4 kJ/mol and Δ?∘=−87.9 J/(mol⋅K). Assuming these values change…

A: Given: ΔHo = -28.4 KJ/mol = -28400 J/mol. And the value of ΔSo = -87.9 J/mol.K.

Q: Calculate ΔGrxn at 7.2 °C for a reaction that has ΔHrxn= 29.4 kJ and ΔSrxn= 78.08 J/K

A: Given :- Temperature = 7.2°C ΔHrxn= 29.4 kJ ΔSrxn= 78.08 J/K To calculate :- ΔGrxn

Q: Chloroform, CHCl3, is a solvent and has been used as an anesthetic. The heat of vaporization of…

A: We have: Thus, the amount of energy required to boil 1.44 moles of CHCl3 is:

Q: ΔGo

Q: Calculate the standard free energy change (kJ/mol) for the reaction shown at a temperature of 298.15…

Q: ΔSsurrounding = J/K for the reaction at 298 K. 2 H2(g) + O2(g) → 2 H2O(g) ΔHrxn = −483.6…

Q: Using the tables, what is the standard entropy change for the following reaction? CH4 (g) + 2 O2…

A: To determine the standard entropy change (ΔS°) for a chemical reaction, we need to use the standard…

Q: for this reaction: H2O(g) → H2O(l) → (gets hot, s

A: When water changes its states from gas to liquid there is a change in states of water from gaseous…

Q: For a particular reaction at 179.4 °C, AG = -801.20 kJ, and AS = 915.51 J/K. Calculate AG for this…

Q: For the reaction 2 NH3 (g) --> N2 (g)+ 3 H2 (g) , ∆H = +92 kJ. Which of the following is true?…

A: The given reaction is, 2 NH3 (g) --> N2 (g)+ 3 H2 (g) , ∆H = +92 kJ ∆H is positive, that means…

Q: Which statement is true for the temperature dependence of the reaction below if DH = 1319 kJ/mol and…

Q: What is the entropy change (in J/K) when 43.3 g of liquid sulfur at its melting temperature of…

A: Answer:Entropy is the measure of system's disorderliness or randomness. In more possible microstates…

Q: The value of ΔH° for the reaction below is −5314 kJ. The amount of heat that is released by the…

A: Balanced chemical equation: 2C4H10(g) + 13O2(g) → 8CO2(g) + 10H2O(l) ΔH° = −5314 kJ From the…

Q: When 10.00 grams of NH4CN (s) is dissolved in 120.0 grams of water inside a perfect calorimeter, the…

Q: What is the lowest temperature at which the reaction of C(s) with H2O(g) to produce H2(g) and CO(g)?…

A: The lowest temperature would be 981..3153°C.

Q: N2 (g) + 3H2 (g) → 2NH3 (g) b Ag+ (aq) + Cl- (aq) → AgCl (s) c CaO (s) + CO2 (g) → CaCO3 (s)…

A: In the above reaction standard molar entropy of Gas is highert thanLiquids

Q: Given ΔHrxn = -98.9 kJ and ΔSrxn = - 94.0 J/K at 25 oC for the combination reaction of sulfur…

A: Answer:- This question is answered by using the simple concept of calculation of Standard Gibbs free…

Q: What is the change of entropy in the vaporization of 5 grams of ice cube at 0C to steam at 100 C.…

A: The degree of randomness of the system is called entropy. Specific heat capacity of water(c)=…

Q: Predict the sign of ∆S in the system for each of the following reactions a. 2C6H14(l) + 19O2(g) →…

A: How to determine sign of entropy Sign of entropy of a chemical reaction determined by knowing the…

Q: N2 (9) + 3H2 (9) + 2NH3 (9) does favor formation of products at room temperature but does not favor…

A: Answer

Q: Calculate ΔSuniv for the following reaction at 300K. 2 NO(g) + O2(g) 2NO2(g) ΔHrxn =…

Q: Calculate ΔrH° for the combustion of methane gas, CH4 : CH4(g) + 2 O2(g) → CO2(g) + 2…

A: The standard enthalpy change for the formation of one mole of a compound from its elements in their…

Q: Use the following data to calculate AGºrxn for the equation below using enthalpy and entropy of…

Q: Calculate the change of the entropy of the system in J/K for the following phase transition:…

A: Given data - Mass of methanol = 64.1 g Molar mass of methanol = 32.04 gmol-1 Enthalpy of…

Q: If you have a reaction that occurs in aqueous solution, and raises the temperature of 15.9 g of…

A: As the reaction is exothermic , it liberates heat which rises the temperature of water so sign of…

Question

### Calculating Standard Entropy Change for the Reaction:

**Reaction:**
\[ \text{H}_2(\text{g}) + \text{Br}_2(\text{l}) \rightarrow 2 \text{HBr}(\text{g}) \]

To find the value of standard entropy change, ΔSº, for the reaction, we use the given standard thermodynamic properties of the substances involved.

**Given Table:**

#### Standard Thermodynamic Properties for Selected Substances

| Substance | \(\Delta H_f^\circ\) (kJ mol⁻¹) | \(\Delta G_f^\circ\) (kJ mol⁻¹) | \(S^\circ\) (J K⁻¹ mol⁻¹) |
|-----------|---------------------|-----------------------|-------------------------------|
| \(\text{Br}_2(\text{l})\) | 0 | 0 | 152.23 |
| \(\text{Br}_2(\text{g})\) | 30.91 | 3.142 | 245.5 |
| \(\text{Br}(\text{g})\) | 111.88 | 82.429 | 175.0 |
| \(\text{Br}^-\) (aq) | -120.9 | -102.82 | 80.71 |
| \(\text{BrF}_3(\text{g})\) | -255.60 | -229.45 | 292.42 |
| \(\text{HBr}(\text{g})\) | -36.3 | -53.43 | 198.7 |

#### Steps to Calculate \(\Delta S^\circ_{\text{reaction}}\):

1. **Identify the standard entropy values (\(S^\circ\)) for each substance:**
- \(S^\circ (\text{H}_2(\text{g}))\) = **Assumed Known for Calculation**
- \(S^\circ (\text{Br}_2(\text{l}))\) = 152.23 J K⁻¹ mol⁻¹
- \(S^\circ (\text{HBr}(\text{g}))\) = 198.7 J K⁻¹ mol⁻¹

2. **Apply the formula for the standard entropy change:**
\[
\Delta

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:- the values given in the question

VIEW

Step 2:- Calculation of standard entropy change of the reaction using formula

VIEW

Step 3:- Answer

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 3 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

Consider the following thermochemical equations. Reaction ΔrH° / kJ mol−1 HBr(g) ⟶ H(g) + Br(g) 365.7 H2(g) ⟶ 2 H(g) 436.0 Br2(g) ⟶ 2 Br(g) 193.9 What is ΔrH° for the reaction below? HBr(g) ⟶ ½ H2(g) + ½Br2(g) Give your answer in kJ mol−1, accurate to one decimal place. Kindly double check your solution.
3. Calculate the value of ΔSo for the formation of POCl3 from its constituent elements, as shown below. P2(g) + O2(g) + 3Cl2(g) → 2POCl3(g)
Calculate the standard free-energy changes for the following reactions at 25°C. CH4(g) + 2O2(g) → CO2(g) + 2H2O(l) 2MgO(s) → 2Mg(s) + O2(g) Inorganic Substances Substance ΔHo (kJ/mol) f ΔGo (kJ/mol) f So (J/K·mol) CO(g) -110.5 -137.3 197.9 CO2(g) -393.5 -394.4 213.6 H2(g) 0 0 131.0 H2O(l) -285.8 -237.2 69.9 O2(g) 0 0 205.0 Organic Substances CH4(g) -74.85 -50.8 186.2 Mg(s) 0 0 32.5 MgO(s) -601.8 569.6 26.78 Table 1. Selected Thermodynamic Data at 1 atm and 25°C* *The ΔHof, ΔGof and S° values for ions are based on the reference states ΔHof (H+) = 0, ΔGof (H+) = 0, and S°(H+) = 0.
Calculate ΔGo for a reaction for which ΔHo = 24.6 kJ and ΔSo= 132 J/K at 298 K.
Calculate AS°rxn for the following reaction. The S° for each species is shown below the reaction. N2H4(l) + H2(g) → 2 NH3(g) ings S°(J/(mol·K)) 121.2 130.7 192.8 O -59.1 J/K es O 311.0 J/K O 133.7 J/K O -133.7 J/K O 637.5 J/K
Calculate the entropy (in J/K) change when 186.8 g of liquid cyclohexane, C6H12, freezes at 6.47°C. The boiling point is 80.74°C, the melting point is 6.47°C, the enthalpy of vaporization is 32.0 kJ/mol, and the enthalpy of fusion is 2.68 kJ/mol for cyclohexane. Report your answer to 3 sig figs, but do NOT include units.
What is entropy, and what is ΔS for a reaction, and what does it mean if ΔS is positive or negative?
What is the standard molar entropy change of the following reaction? 8 NH3(g) + 10 O2(g) → 8 NO(g) + 12 H2O(g) Given: S°NH3 = 193 J/K·mol; S°O2 = 205 J/K·mol; S°NO = 211 J/K·mol; S°H2O = 189 J/K·mol
A mixture of CO(g) and H2(g) is produced by passing steam over hot charcoal: H2O(g)+ C(s)->H2(g)+CO(g) Using the appropriate thermodynamic values in the table below, calculate the lowest temperature at which the reaction is spontaneous under standard conditions. Compound ΔGf (kJ/mol) ΔHf (kJ/mol) ΔHf (kJ/mol) H2O(g) –228.6 –241.8 188.8 H2O(ℓ) –237.2 –285.8 69.9 C(s) 0.0 0.0 5.7 H2(g) 0.0 0.0 130.6 CO(g) –137.2 –110.5 197.7 O2(g) 0.0 0.0 205.0 _____K
Calculate the entropy (in J/K) change when 866.7 g of liquid cyclohexane, C6H12, freezes at 6.47°C. The boiling point is 80.74°C, the melting point is 6.47°C, the enthalpy of vaporization is 32.0 kJ/mol, and the enthalpy of fusion is 2.68 kJ/mol for cyclohexane. Report your answer to 3 sig figs, but do NOT include units.
For a particular reaction, Δ?=−14.20 kJ and Δ?=−198.5 J/K. Calculate Δ? for this reaction at 298 K
Consider the chemical reactions below and their given deltaG of reactions; NiO(s) → Ni(s)+0,(g) AG° = +115 kJ C(s) +0,(g)→CO(g) AG° = -250 kJ MnO(s) → Mn(s)+0,(g) AG° = +280 kJ If Manganese metal is burned (i.e., combustion in excess oxygen) with NiO(s), metallic Ni and Mno can be produced (through coupled reactions). Select one: O True O False