Energy > The image below shows two configurations of a system of 4 particles. Energy levels increase going upward. Sample A has a total energy of 5), while sample B has a total energy of 8J. Which sample (A or B) has the greatest entropy nts (Hint: how many different arrangements of particles could produce a state with the same overall energyl? 3 ok 2. 1 B Meou The sample with the greatest entropy is Select

Energy > The image below shows two configurations of a system of 4 particles. Energy levels increase going upward. Sample A has a total energy of 5), while sample B has a total energy of 8J. Which sample (A or B) has the greatest entropy nts (Hint: how many different arrangements of particles could produce a state with the same overall energyl? 3 ok 2. 1 B Meou The sample with the greatest entropy is Select

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...

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Which statement is true of the internal energy of the system and its surroundings following a process in which ΔEsys = +65 kJ? Explain.a. The system and the surroundings both lose 65 kJ of energy.b. The system and the surroundings both gain 65 kJ of energy.c. The system loses 65 kJ of energy and the surroundings gain 65 kJ of energy.d. The system gains 65 kJ of energy and the surroundings lose 65 kJ of energy.
If a reaction does not move forward and backward (meaning only move to one direction; could be product favored, could be reactant favored under these conditions), what is true about entropy and enthalpy? a. ΔH°rxn < 0 and ΔS°rxn > 0. b. ΔH°rxn < 0 and ΔS°rxn < 0. c. ΔH°rxn > 0 and ΔS°rxn < 0. d. ΔH°rxn > 0 and ΔS°rxn > 0. e. both a and c are correct
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)
One mole of an ideal gas is contained in a cylinder with a movable piston. The temperature is constant at 78°C. Weights are removed suddenly from the piston to give the following sequence of three pressures. a. P₁ b. P2 c. P3 = 5.20 atm (initial state) = 2.53 atm = 1.00 atm (final state) What is the total work (in joules) in going from the initial to the final state by way of the preceding two steps? J What would be the total work if the process were carried out reversibly? J
estion 30 of 41 <. Consider an ideal gas enclosed in a 1.00 L container at an internal pressure of 10.0 atm. Calculate the work, w, if the gas expands against a constant external pressure of 1.00 atm to a final volume of 10.0 L. J w = Now calculate the work done if this process is carried out in two steps. 1. First, let the gas expand against a constant external pressure of 5.00 atm to a volume of 2.00 L. 2. From the end point of step 1, let the gas expand to 10.0 L against a constant external pressure of 1.00 atm. J w = とTOOLS x10 Question Source: McQuarrie, Rock, And Gallogly 4e - General Chemsitry| Publisher: University Science Books A étv Aa w MacBook Air DD
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.
Compare what will happen to the entropy of the whole system in the following two scenarios: A) if the oil molecules are all clumped together and the clump is surrounded by water and B) if the oil molecules are spread out evenly throughout the water, each individual oil molecule surrounded by water?
Which of the following best defines molar heat capacity. a. The quantity of heat required to raise the temperature of 1 mole of a substance by 1K b. The quantity of heat required to lower the temperature of 1 liter of a substance by 1°C c. The quantity of heat required to raise the temperature of 1 gram of a substance by 1°C d. The quantity of heat required to raise the temperature of 1 gram of a substance by 1°F
What of the following options describes the term "entropy, S"? O a. If a process or reaction is carried out in multiple steps, the sum of the enthalpy changes for these steps is the same as the enthalpy change if the entire reaction was carried out in a single step. O b. An indication that a process is capable of proceeding in a given direction without needing to be driven by an outside source of energy. O c. A thermodynamic function which measures the dispersal of energy amongst the particles in a substance. O d. The substances or material being studied in an experiment. For a chemical reaction, the system is all of the atoms in the substances undergoing the reaction. O e. Everything outside of the system.
Consider the following chemical reaction. 2CH,(g) +30,(g) – 2CO(g) + 4H,O() Select all the statements that are correct. The potential energy of the reactants is higher than the potential energy of the products. O The reactants can adopt a larger number of configurations than the products. The reaction should become more product favored at hiph temperatures. IThe reactants can adopt a fewer number of confipurations than the products. I The potential energy of he reactants is lower than the potential energy of the products. The reaction should become more product lavored at low temperatures.
In a reaction similar to Reaction 1, 3.2 g of sodium hydroxide (NaOH) is added to 100.0 g of water. A rise in temperature of 2.9 °C was noted. Assume the solution formed is water and c= 4.184 J/ (g °C). a. Calculate the heat, q, evolved for this reaction. b. How many moles of NaOH were reacted? c. Using the answers to a and b, what is the H for this reaction in kJ/mol?