Calculate the standard entropy change for the formation of 1.0 mol of the following compounds from the elements at 25 °C.a. C2H4 (g)Use the following data:JK. molC2H4 (g)C(s, graphite)H2 (g)219.365.6130.7A,S° =J/K-mol-rxnb. MgCO3 (s)Use the following data:JS°K- molMgCO3 (s)65.84Mg(s)C(s, graphite)02 (g)32.675.6205.07A,S° =J/K-mol-rxn

Introduction : We have it calculate entropy change for the following reaction .

nange a. C2H4(g) Use the following data: J S*, K· mol C,H4(g) C(s, graphite) H2 (g) 219.36 5.6 130.7 A,s* = J/K-mol-rxn b. MgCO3 (s) Use the following data: J S*, К - mol MgCO,(s) 65.84 Mg(s) C(s, graphite) 32.67 5.6 O2(8) 205.07 A,s° = J/K-mol-rxn

nange a. C2H4(g) Use the following data: J S, K· mol C,H4(g) C(s, graphite) H2 (g) 219.36 5.6 130.7 A,s = J/K-mol-rxn b. MgCO3 (s) Use the following data: J S*, К - mol MgCO,(s) 65.84 Mg(s) C(s, graphite) 32.67 5.6 O2(8) 205.07 A,s° = J/K-mol-rxn

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter17: Chemcial Thermodynamics

Section: Chapter Questions

Problem 17.51QE

See similar textbooks

Related questions

Q: Calculate ΔH for the reaction2 C(s) + H2(g) -----> C2H2(g)given the following chemical equations…

A: Given,

Q: Calculate the enthalpy of the reaction 4B(s)+302 (g)→2B2O3(s) given the following pertinent…

Q: A certain metallic element M formed an oxide which contained 89.70% M. The specific heat capacity of…

A: % of element = 89.70 % of oxygen = 100 - 89.70 = 10.3 If 100 g of the compound taken = 10.30 g O…

Q: Calculate the standard enthalpy change for the reaction 2A +B 20+2D Use the following data: AH…

Q: Consider the following reaction: H2(g) + ½ O2 (g) ------> H2O (g) The standard enthalpy of…

A: We can solve a given problem by using the Kirchhoff equation for enthalpy change It states that the…

Q: Calculate the total energy (kJ) required to heat a 17.5 g sample of benzene (C&H6) from 0.00 °C to…

A: Given that: molar mass: 78.11 g/mol cs,solid = 1.51 J/g*°C cs,liquid = 1.70 J/g*°C cs,gas = 1.05…

Q: Calculate the enthalpy change on the formation of methane gas from the elements, using the following…

A: Given: Heat of combustion of carbon (∆H°combustion of C) = 393.51 kJ/mol Heat of formation…

Q: 18. For the following combustion reaction of benzoic acid (HC7H5O2; molar mass = 122.1 g/mol)…

A: Final temperature would be 30.2°C (option C).

Q: The specific heat capacities (in units of J/g K) of element X, Y and Z are 0.379, 0.485 and 0.349,…

A: Specific heat capacity: The amount of heat that is required by the unit mass of a substance at the…

Q: The standard enthalpy change for the reaction 3 O2(g) → 2 03(g) is 285.4 kJ mol·' at 298 K and 1…

A: In the given question we have to calculate the enthalpy of Reaction at 380k.

Q: Calculate the change in enthalpy (in kJ/mol) for the following reaction using the data provided.…

A: Given information: ΔH°f = NaHCO3(s) = -947.7 kJ/mol ΔH°f = Na2CO3(s) = -1131 kJ/mol ΔH°f = H2O(g) =…

Q: What is the internal energy (in J) of 5.50 mol of an ideal monatomic gas at 201°C? J

A: Given: Monoatomic gas number of moles, n = 5.50 moles Temperature, T = 201°C = 474.15K

Q: If for the reaction: 2Fe(s) + O2(g) →2F€O(s) AHrn= -544 kJ/mol rxn, then for the reaction: FeO(s)…

A: Given, 2Fe(s) + O2(g)→ 2FeO(s) ∆Hrxn = - 544 kJ/mol

Q: Calculate the change in enthalpy (in kJ/mol) for the following reaction using the data provided.…

Q: Here you are invited to explore the implications of the temperature dependence of the heat capacity…

A: The equation for the molar heat capacity at constant pressure in terms of derivatives is as follows:

Q: The molar heat capacity of solid aluminium is 24.4 J K-1 mol -1 at 25°C. Calculate the change in…

Q: Calculate the standard enthalpy change for the reaction 2A+B=2C+2D Use the following data: AH₂…

Q: A certain hydrocarbon of the molecular formula C,H2, has a standard enthalpy of formation AH, =…

A: For the combustion reaction, the chemical equation is shown by equation (1) and the value for x is…

Q: Use Hess's Law to calculate the enthalpy change for the reaction WO3(s) + 3H2(g) → W(s) + 3H2O(g)…

A: The enthalpy of the first reaction is -1685.4 kJ. The enthalpy of second reaction is -477.84 kJ.

Q: Using the following data, calculate the standard heat of formation of IC1(g) in kJ/mol: Cl2 (g) → 2…

A: Enthalpy of formation :- The enthalpy change involved in the formation of 1 mole of a compound from…

Q: Dichloromethane (chloroform) if produced commercially in the following reaction: COClL + 2H,0, ==>…

Q: A certain hydrocarbon of the molecular formula CxH2x has a standard enthalpy of formation ∆Hf° =…

A: The correct method to calculate the value for x is attached below

Q: 21.7 g of a basic solution was mixed with 87.6 g of water in a calorimeter with a calorimeter…

Q: Carbon monoxide, CO, reacts with chlorine, Cl,, to form the very poisonous gas phosgene, COCI,.…

Q: A 0.500 mole sample of CO(g) is combusted in a constant pressure calorimeter to CO2(g). The…

A: Given: Initial temperature of calorimeter = 25.00 oC Final temperature of calorimeter = 27.50 oC…

Q: Formation of carbon dioxide Data: Standard molar enthalpy of formation of CO2 (g) at 300 K: AH°(CO2,…

A: Standard enthalpy of formation is enthalpy change when one mole of product is synthesized from its…

Q: 16. Given the following set of reaction data, C(s) + O2(8) → CO,(8) 2CO(g) +O2(g) 2H2 (8) + O2(g) AH…

A: C(s) +O2 ---> CO2 ∆H = -393.5 kj/mol 2CO + O2 --> 2CO2 ∆H = -566.0…

Q: 15 Calculate ΔGrxn in (kJ/mol) for the reaction for which ΔHrxn=-26.1kJ/mol ; ΔS=3.89J/molK at…

A: Gibb's Free energy isbthe change of free energy during a reaction. It can be positive negative or…

Q: A,H° = 86 kJ mol-1 , A,S = - 140 JK-1 mol-1 ,T = 299 K %3D Express your answer as an integer.

Q: The standard enthalpy change for the combustion of 1 mole of propane is –2043.0 kJ. C3H8(g)…

Q: You have a supply of ice at 0.0°C and a glass containing 150 g water at 25°C. The enthalpy of fusion…

A: Given that : Mass of Water (M1) = 150 g at Temperature (T1)= 25°C. The enthalpy of fusion for ice…

Q: From the enthalpies of reaction2 C(s) + O2(g)----->2 CO(g) ΔH = -221.0 kJ2 C(s) + O2(g) + 4…

A: Given:

Q: Using the data below, the ∆S⁰ is -326.3 J/K in the combustion of hydrogen in the presence of excess…

Q: How much energy is required to heat 54.0 g H 2O from a liquid at 25.0°C to a complete gas at 100 °C?…

A: There are two stages to calculate the energy required to heat a liquid from 25oC to a complete gas…

Q: Suppose 1.00 mol ice at –30°C is heated at atmospheric pressure until it is converted to steam at…

Q: The combustion of 1.839 g of glucose (C6H12O6) in a bomb calorimeter (Ccal = 4.60 kJ/℃) results in a…

A: The amount of glucose (C6H12O6) = 1.839 g Heat capacity of a bomb calorimeter = Ccal = 4.60 kJ/℃…

Q: Calculate the standard enthalpy change for the reaction 2A +B=20 + 2D Use the following data: AH…

A: The enthalpy change can be calculated via subtracting that of reactants from that of products.

Q: Given the standard enthalpies of formation for the following substances, determine the reaction…

A: The enthalpy change of a chemical reaction can be calculated by the standard heat of the formation…

Q: The integrated form of Kirchhoffs Law. A,H(T2) = A, H(T;) + A, Cp(T2 - T) where A,H(T;) and A,H(T2)…

Q: Calculate the total energy (kJ) required to heat a 17.5 g sample of benzene (C6H6) from 0 °C to 97.2…

A: Mass of benzene, m = 17.5 g Specific heat capacity of solid benzene, Cs = 1.51 J/g°C Temperature…

Q: Calculate the enthalpy change for the reaction C(s) + 2H2 (g)--->CH4(g) from the following data.…

A: # We have to use all the reaction and manipulate it in such a way that we get the desired equation .…

Q: From the enthalpies of reactionH2(g) + F2(g)-----> 2 HF(g) ΔH = -537 kJC(s) + 2 F2(g)------>…

A: Change in enthalpy of the reaction is the heat given our ar absorbed by the reaction. It is usually…

Q: 3. Use the appropriate data from the table to calculate the change in enthalpy for this reaction:…

Q: A certain hydrocarbon of the molecular formula CxH2x has a standard enthalpy of formation ∆Hf° =…

A: To solve this problem first we have to write the balanced chemical equation of combustion of…

Q: Given the following data on Phosphorus and its allotropes o ∆Hf kJ mol-1 ∆Gfo kJmol-1 So J…

A: Gibbs free energy is the energy utilized for doing certain work. In a reaction, a work done is…

Q: Another group performed the combustion of sucrose. Determine the AHcombustion (in kJ/mol) of sucrose…

Q: Calculate the enthalpy of the reaction below (AHrxn, in kJ) using the bond energies provided. N,(9)…

Q: Given the following processes and their respective enthalpies in kJ/mol: Li(s) -->…

Q: Calculate the standard enthalpy change for the reaction 2C8H18(l) + 21O2(g) → 8CO(g) + 8CO2(g) +…

Question

100%

Calculate the standard entropy change for the formation of 1.0 mol of the following compounds from the elements at 25 °C.
a. C2H4 (g)
Use the following data:
J
K. mol
C2H4 (g)
C(s, graphite)
H2 (g)
219.36
5.6
130.7
A,S° =
J/K-mol-rxn
b. MgCO3 (s)
Use the following data:
J
S°
K- mol
MgCO3 (s)
65.84
Mg(s)
C(s, graphite)
02 (g)
32.67
5.6
205.07
A,S° =
J/K-mol-rxn

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

Step 2

Step 3

Step 4

Trending now

This is a popular solution!

Step by step

Solved in 4 steps with 2 images

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Applications of Statistical Thermodynamics

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

The standard molar entropy of methanol vapor, CH3OH(g), is 239.8 J K1 mol-1. (a) Calculate the entropy change for the vaporization of 1 mol methanol (use data from Table 16.1 or Appendix J). (b) Calculate the enthalpy of vaporization of methanol, assuming that rS doesnt depend on temperature and taking the boiling point of methanol to be 64.6C.
10.69 If a sample of air were separated into nitrogen and oxygen molecules (ignoring other gases present), what would be the sign of for this process? Explain your answer. The next four questions relate to the following paragraph [Frank L. Lambert, Journal of Chemical Education, 76(10), 1999, 1385]. "The movement of macro objects from one location to another by an external agent involves no change in the objects' physical (thermodynamic) entropy. The agent of movement undergoes a thermodynamic entropy increase in the process."
In a spontaneous process, S(universe) is (a) 0 (b) = 0 (c) 0
The standard molar entropy of iodine vapor, I2(g), is 260.7 J Kl mol-1 and the standard molar enthalpy of formation is 62.4 kJ/mol. a) Calculate the entropy change for vaporization of 1 mol of solid iodine (use data from Table 16.1 or Appendix J). b) Calculate the enthalpy change for sublimation of iodine. c) Assuming that rSdoes not change with temperature, estimate the temperature at which iodine would sublime (change directly from solid to gas).
The synthesis of glucose directly from CO2 and H2O and the synthesis of proteins directly from amino acids are both non-spontaneous processes under standard conditions. Yet it is necessary for these to occur for life to exist. In light of the second law of thermodynamics, how can life exist?
Appendix J lists standard molar entropies S, not standard entropies of formation rS. Why is this possible forentropy but not for internal energy, enthalpy, or Gibbsfree energy?
A 2.50-mol sample of gas is compressed isothermally from 20.0 L to 5.00 L under a constant external pressure of 10.0 atm. Calculate w, q, U, and H for the process.
Explain why absolute entropies can be measured.
Limestone is predominantly CaCO3, which can undergo the reaction CaCO3(s)CaO(s)+CO2(g). We know from experience that this reaction is not spontaneous, yet S for the reaction is positive. How can the second law of thermodynamics explain that this reaction is not spontaneous?
What is the sign of the standard Gibbs free-energy change at low temperatures and at high temperatures for the formation of hydrogen sulfide from the elements? H2(g)+18S8(s)H2S(g)
a From a consideration of the following reactions, calculate Hf for ethane, C2H6(g). CH3CHO(g)+2H2(g)C2H6(g)+H2O(l);H=204kJ2H2(g)+O2(g)2H2O(g);H=484kJ2C2H5OH(l)+O2(g)2CH3CHO(g)+2H2O(l);H=348kJH2O(l)H2O(g);H(kJ)=442C2H5OH(l)4C(s)+6H2(g)+O2(g);H(kJ)=555 b From appropriate entropy data, calculate S for the formation of ethane from the elements. c Using the information from above, calculate Gf for ethane at 25C.
What is the sign of the standard Gibbs free-energy change at low temperatures and at high temperatures for the synthesis of ammonia? 3H2(g) + N2(g) 2NH3(g)