Answered: Two systems, each composed of two…

Two systems, each composed of two particles represented by circles, have 20 J of total energy. Which system, A or B, has the greater entropy? Why? System A System B 12] 10J 81

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 graph represents the energy change of a chemical reaction. Which must be true about the entropy…

A: Given, the energy profile diagram: We have to find the correct statement about the entropy of the…

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

A: Spontaneity is predicted by change is gibbs energy, if change in gibbs energy is negative then the…

Q: 2.045 g of a new compound with formula C9H8O2 is burned in a bomb calorimeter. During the…

Q: Methane reacts with chlorine gas to produce methyl chloride and hydrogen chloride. This reaction is…

A: A reaction is spontaneous when ∆G of the reaction is negative and ∆G is determined by the formula :…

Q: When solid sodium chloride is cooled from 25°C to 0.°C, the entropy change is –4.4 J/mol. K. Is this…

A: Entropy is a measure of the degree of disorder or randomness in a system. It is a thermodynamic…

Q: Consider the following reaction: 2 NO(g) N2(g) + O2(g) The enthalpy change at 298 K for this…

A: The given equilibrium reaction is 2 NO(g) ----------> N2(g) + O2(g) The enthalpy change at 298…

Q: 2 H2(g) + O2(g) → 2 H2O(l) HCl(g) → H+(aq) + Cl-(aq) Na(s) + 1/2 Cl2(g) → NaCl(s) What is right?…

Q: Two systems, each composed of two particles represented by circles, have 20 J of total energy. Which…

A: The system which has greater entropy has to be given and the reason has to be explained.

Q: Each farm is 333.0 acres and for each acre on the farm 135.0 bushels of corn are produced. Each…

A: In this problem it is given that Each farm is 333.0 acres and for each acre on the farm 135.0…

Q: Consider the following reaction, 2A2(g) + 2B2C(l) ⟶⟶4BA(g) + C2(g) What is Δ?ΔH for the reaction,…

A: Consider the following reaction, 2A2(g) + 2B2C(l) ⟶⟶4BA(g) + C2(g) What is ΔH for the reaction ?

Q: 2 Ag20(s) → 4 Ag(s) + O2(g) Thermodynamic data are given below. 2 Ag20(s) → 4 Ag(s) + 02(g)…

A: NO, decomposition of silver (I) Oxide is not favored at 25 deg C.

Q: 6. Calculate AG for the combustion of propane. C3H8(g) + 50₂(g) → 3CO₂(g) + 4H₂O(g) C3H8(g) -24.5…

Q: Change An exothermic chemical reaction between a solid and a liquid results in gaseous products. A…

A: Answer: Spontaneity of the reaction can be decided on the basis of the value of Gibbs free energy…

Q: Consider the solution process for NH4NO3(s): NH4NO3(s) → NH4+(aq) + NO3-(aq) When a 4.25g…

A: Answer:- This question is answered by using the simple concept of enthalpy of solution using the…

Q: A chemical system produces 155 kJ of heat and does 22 kJ of work. What is ΔE for the surroundings?a)…

A: In order to solve this question, we will use the first law of thermodynamics which states that…

Q: Sodium hydroxide (39.9971 g/mol) reacts with excess H2SO4 in a constant-pressure calorimeter. The…

A: Given ∆T = 29°CMass of reaction mixture = M = 120 gSpecific heat of solution = Cs = 4.184 J/g°CHeat…

Q: 2Al(s) + 3Cl2(g) → 2AlCl3(s) Find the change in internal energy for this reaction. Enter in kJ.

A: The given equation is:

Q: When 1.99 g of sucrose is combusted in a constant volume (bomb) calorimeter, 32.8 kJ of heat is…

Q: The sun catalyzes the atmospheric reaction as seen below. 2N2O(g)+O2(g)→4NO(g) This reaction would…

A: Answer :- The reaction will have a Positive ΔS , because the moles of gas increases.…

Q: According to the following reaction, how much energy is evolved during the reaction of 32.5 g B2H6…

A: Given reaction: B2H6 (g) + 6Cl2 (g) → 2BCl3 (g) + 6HCl (g) ∆H∘rxn = -1396 kJ We have to calculate…

Q: ΔEsys

Q: Consider the following generic reaction: A+2B→C+3D with ΔH = 111 kJ . Determine the value of ΔH for…

Q: What is the change in the energy of surroundings when the system absorbs 17.5 kJ of energy and…

A: It is given that system absorbs 17.5 kJ of energy and the work done is 5×103 J. It is known that 1 J…

Q: Potassium nitrate is mixed into water which causes an endothermic reaction. The initial water temp…

Q: Upon heating, baking soda decomposes as follows, creating the holes in baked bread: 2NaHCO3(s) -->…

A: 39.0 g of NaHCO3 decomposes to produce energy of -30.0 kJ39.0 g of NaHCO3=39.0 g of NaHCO3×1 mole of…

Q: Identify the three statements from the list below that BEST describe the first law of…

A: Solution : Thermodynamics is a branch of chemistry that shows the effects of heat, energy and…

Q: During a certain reversible process, the surroundings undergo an entropy change, ∆Ssurr = -78…

A: As per the thermodynamic concept, the entropy of universe is the sum of entropy of system and…

Q: Combustion of C12H22O11(s) (sucrose or "table sugar") produces CO2(g) and H2O(l). When 1.43 g of…

Q: Which statement is true of the internal energy of the system andits surroundings following a process…

A: The change internal energy is positive that is ∆Esys=+65 kJ.

Q: When you add water to a small amount of sodium chloride (NaCl), the solid dissolved and the solution…

A: The question is based on the concept of chemical thermodynamics . we need to explain effect on…

Q: Consider the reaction: 3CH4(g) → C3H8(g) + 2H2(g) a. Calculate Gof at 298 K (From Appendix C Gof…

A: According to the question, The reaction is as follows, 3CH4(g) → C3H8(g) + 2H2(g) The value for the…

Q: Liquid butane combust in air. Predict the sign for Delta G, Delta S, and Delta H at 25 C:

A: The balanced chemical equation for combustion of butane will be- 2C4H10 (l) + 13O2 (g) →…

Q: What is the entropy change, in J mol-1 K-1, when 100.0 g of water boils at 100.0 oC?…

A: ∆Hvap= 40.7 kJ/mol = 40.7 × 1000 J/mol Water boils at 100°C = 373 K For the vapourization of water,…

Q: A 80.0 mL sample of 0.300 M aqueous hydrochloric acid is added to 80.0 mL of 0.300 M aqueous ammonia…

A: The objective of this question is to calculate the enthalpy change (ΔrH) per mole of HCl and NH3…

Q: Suppose that two systems, each composed of two particles rep- resented by circles, have 20 J of…

A: Entropy is a measure of the extent of energy dispersal, and it rises with the number of comparable…

Q: The graph represents the energy change of a chemical reaction. Which must be true about the entropy…

Q: Use Hess's law to calculate ΔG°rxn using the following information. CO(g) → C(s) + 1/2…

A: Record the given data, CO2(g) → C(s) + O2(g) ΔG°rxn = +394.4 kJ CO(g) + 1/2 O2(g) →…

Q: The combustion of 2.474 g of propanol (C3H7OH) increases the temperature of a bomb calorimeter…

Q: Change A solid absorbs heat and turns to a gas. During an endothermic chemical reaction, a gas is…

A: Answer:The spontaneity of the reaction can be decided on the basis of the value of Gibbs free energy…

Q: Calcium carbonate decomposes according to the following reaction.…

A: Hey, since you are posted a question with multiple sub-parts, we will answer first three sub-parts.…

Q: Calculate the change in entropy that occurs in the system when 40.7 g of acetone (C3 H6O) vaporizes…

A: entropy change calculation during the process of vaporization:

Q: Solid potassium fluoride is dissolved in water in a perfect calorimeter. When 10.00 grams of…

A: In this question we have to calculate ΔHº for the reaction below KF (s) ➝ K+ (aq) + F – (aq)…

Q: Determine ΔE for octane combustion in units of kJ/mol octane.When a 4.50-g sample of liquid octane…

A: The temperature of the calorimeter is raised by 26.6 degree Celsius, so this amount of heat was…

Q: Nitrogen oxide (NO) has been found to be a key component in many biological processes. It also can…

A: Given that The moles of NO = 1 The heat evolved = 57.0 kJ. Mass of nitrogen oxide = 8.00 g. To find…

Q: Which statement DOES NOT describe the entropy of a system in its molecular state? Entropy changes…

A: The degree of randomness in a system is measured in terms of entropy. The higher the entropy greater…

Q: - In which of the following systems is(are) work done by the surroundings on the system? Assume…

Q: The enthalpy change (ΔHrxn) for a certain reaction is 700.0 kJ/mol. The same reaction has an…

Q: Which statement is true of the internal energy of the system and its surroundings following a…

A: The first law of thermodynamics states that the energy of the universe is constant i.e. the sum of…

Q: In the upper atmosphere, ozone is produced from oxygen gas in the following reaction. 3O2(g) →…

A: The change of enthalpy to form one mole of a substance from its constituent elements when all the…

Question

Two systems, each composed of two particles represented by
circles, have 20 J of total energy. Which system, A or B, has the
greater entropy? Why?
System A
System B
12]
10J
81

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

Step 3

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

A 50.0 mL sample of 0.150 M aqueous hydrochloric acid is added to 50.0 mL of 0.150 M aqueous ammonia in a coffee cup calorimeter. The following reaction occurs when the two solutions are mixed: HCl(aq) + NH3(aq) → NH4Cl(aq) The temperature of the solution increases by 2.30°C. Calculate ΔrH per mole of HCl and NH3 reacted. Assume no heat is lost to the calorimeter, and the density and specific heat capacity of the solution is that of pure water (d=1 g/mL, Cs = 4.18 J/gK).
Calculate the change of the entropy of the system in J/K for the following phase transition: condensation of 64.1 g methanol The molar mass of methanol (CH3OH) is 32.04 g/mo%; the enthalpy of vaporization of methanol is 37.6 kJ/mol; the boiling point of methanol is 64.7°C A) -3640 B) -1130 C) 1.13446677 D) -223 E) 0.22258
In the following experiment, solid CaCl2 (M = 110.98 g/mol) is dissolved in water:CaCl2(s) → Ca2+(aq) + 2Cl-(aq) ΔsolnH = ? kJ mol−1A 4.00 g sample of CaCl2 is added to a coffee-cup calorimeter containing 125 g of H2O. The initial temperature of water in the calorimeter is 22.0°C and the final temperature is 27.5°C. What is the enthalpy change for the dissolution reaction (ΔsolnH) in kJ per mole of CaCl2? Assume the specific heat capacity of the solution is the same as water (Cs=4.18 J g-1 °C-1) and that no heat is lost to the calorimeter.
Consider the following reactions at 298 K. 2 03(g) → 3 O₂(g) O₂(g) → 2 0(g) NO(g) + O3(g) → NO₂(g) + O₂(g) ΔΗΘ Aat H ᎪᎻᎾ = -427.0 kJ/mol = 495.0 kJ/mol = -199.0 kJ/mol Apply Hess's law to calculate the standard reaction enthalpy for the reaction NO(g) + O(g) → NO₂(g)
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)
Which one of the following reactions cannot proceed spontaneously as written at any temperature? Assume that ΔH°rxn does not depend on temperature. A. 2Cl2O(g) → 2Cl2(g) + O2(g) ΔH°rxn = –151 kJ B. 3O2(g) → 2O3(g) ΔH°rxn = +284 kJ C. COCl2(g) → CO(g) + Cl2(g) ΔH°rxn = +112 kJ D. 2C(s) + 2S(s) + O2(g) → 2COS(g) ΔH°rxn = –137 kJ E. N2O4(g) → 2NO2(g) ΔH°rxn = +171 kJ
Given the following reaction and its enthalpy change, and the sign of the entropy change that you get using what you know of trends in entropy, S, when is this reaction spontaneous? 2 ClO2 (g) + 2 TiCl4 (l) → 2 TiO2 (s) + 5 Cl2 (g) Delta H = – 343.8 kJ Select one: a. This reaction is spontaneous at lower temperatures, but not at higher temperatures. b. This reaction is spontaneous at higher temperatures, but not at lower temperatures. c. This reaction is never spontaneous. d. none of these e. This reaction is spontaneous at all temperatures.
In a coffee-cup calorimeter, 0.800 g of ammonium nitrate is mixed with 37.5g of water at an initial temperature of 31.0 ^oC The ΔH for the solution of ammonium nitrate is 26.6 KJ/mol NH4NO3. Calculate the final temperature of the calorimeter in celsius after the salt has dissolved.
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.
Read the descriptions of physical or chemical changes in the table below. Then decide whether the change will be spontaneous, if you can. Change During an endothermic chemical reaction, four moles of gaseous reactants are turned into two moles of gaseous products. A solid precipitates from a solution, releasing heat as it does so. A solid absorbs heat and turns to a gas. Is this change spontaneous? Yes. O No. O Can't decide with information given. O Yes. O No. O Can't decide with information given. O Yes. O No. O Can't decide with information given.
Nitric oxides, NONO and NO2NO2, contribute to air pollution, acid rain, and the depletion of the ozone layer. After NONO forms in the combustion chamber of an automobile engine, it reacts further with oxygen to form NO2NO2. The reaction is given by: 2NO(g)+O2(g)→2NO2(g). Calculate ΔS∘rxn for the reaction? Entropy values given by following table SubstanceSubstance S∘ (J/mol⋅K)S∘ (J/mol⋅K) NO2NO2 240.0 O2O2 205.2 NONO 210.8
Suppose 9.44 g of calcium chloride, CaCl2, (MM=111.0 g/mol) is added to 222. g water at 21.84oC in a styrofoam cup calorimeter, and the temperature rose to 29.76oC. Calculate a value for ΔH in the equation: CaCl2(s) + H2O(l) → Ca2+(aq) + 2Cl-(aq) ΔH = ??? kJ/mol. (Assume that the styrofoam cup does not absorb any heat nor allow any heat loss; assume the specific heat of the resulting solution is 3.88 J/(goC))