For each system listed in the first column of the table below, decide (if possible) whether the change described in the second column will increase the entropy Sof the system, decrease S, or leave S unchanged. If you don't have enough information to decide, check the "not enough information" button in the last column.Note for advanced students: you may assume ideal gas and ideal solution behaviour.SystemChangeASAS < 0A mixture of helium (He) gas andArAS = 0An additional 2.0 L ofis added to the mixture, with thepuregasargon (Ar) gas at 5 atm andAS > 0-14°C.pressure kept constant at 5 atm.not enoughinformationAS < 0AS = 0A solution made of sodium iodide50. mL of pure water is added to(Nal) in water, at 92°C.the solution.AS > 0not enoughinformationAS < 0The solution is put into asemipermeable bag immersed in theA 0.35 M solution of sucrose inO AS = 0water, and a beaker of pure water,water, and 50. mL of pure waterAS > 0both at 37.°C.flows through the bag into thesucrose solution.not enoughinformation

Change in Entropy of System is always positive when randomness increases..!

of the system, decrease S, or leave S unchanged. If you don't have enough information to decide, check t Note for advanced students: you may assume ideal gas and ideal solution behaviour. System Change AS O aS < o A mixture of helium (He) gas and O AS = 0 An additional 2.0 L of pure Ar gas is added to the mixture, with the pressure kept constant at 5 atm. argon (Ar) gas at 5 atm and O As > 0 -14°C. not enough information AS < 0 O AS = 0 A solution made of sodium iodide 50. mL of pure water is added to (Nal) in water, at 92°C. O As > 0 the solution. not enough information AS < 0 A 0.35 M solution of sucrose in The solution is put into a semipermeable bag immersed in the O AS = 0 water, and a beaker of pure water, water, and 50. mL of pure water O As > 0 both at 37.°C. flows through the bag into the sucrose solution. not enough information

of the system, decrease S, or leave S unchanged. If you don't have enough information to decide, check t Note for advanced students: you may assume ideal gas and ideal solution behaviour. System Change AS O aS < o A mixture of helium (He) gas and O AS = 0 An additional 2.0 L of pure Ar gas is added to the mixture, with the pressure kept constant at 5 atm. argon (Ar) gas at 5 atm and O As > 0 -14°C. not enough information AS < 0 O AS = 0 A solution made of sodium iodide 50. mL of pure water is added to (Nal) in water, at 92°C. O As > 0 the solution. not enough information AS < 0 A 0.35 M solution of sucrose in The solution is put into a semipermeable bag immersed in the O AS = 0 water, and a beaker of pure water, water, and 50. mL of pure water O As > 0 both at 37.°C. flows through the bag into the sucrose solution. not enough information

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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A solution containing 100 gg of NaNO3NaNO3 in 90.0 gg H2OH2O at 50 ∘C∘C is cooled to 20 ∘C∘C. Use the solubility data from the table below. Solubility (g/100.gH2O)(g/100.gH2O) Substance 20 ∘C∘C 50 ∘C∘C KClKCl 34.0 42.6 NaNO3NaNO3 88.0 114.0 C12H22O11C12H22O11 (sugar) 203.9 260.4 How many grams of NaNO3NaNO3 remain in solution at 20 ∘C∘C? How many grams of solid NaNO3NaNO3 came out of solution after cooling?
5) The volume of several aqueous copper sulfate (CuSO4) solutions was precisely measured at SATP. All of the solutions were made by adding copper sulfate to 100.00 g of water. ncopper sulfate (mol) Vsolution (mL) 0 100.18 0.0330 100.16 0.0696 100.36 0.111 100.81 0.156 101.62 First, estimate the concentration-dependent partial molar volume of copper sulfate in water by taking finite differences. Second, fit the data to a hyperbola and take a derivative of the hyperbola to accurately calculate the partial molar volume of copper sulfate in water at each concentration. Interpret the partial molar volume at infinite dilution - what must copper sulfate be doing to the nearby water molecules?
utions - Homework - 2022.pdf - Adobe Acrobat Pro DC (32-bit) E-Sign Window Help ols Chapter 14 - Soluti. x 2 / 3 135% 8) Determine the freezing point of a solution that contains 63.8 g of naphthalene (C10H8, molar mass = 128.16 g/mol) dissolved in 275. mL of benzene (d = 0.877 g/mL). Pure benzene has a melting point of 5.50°C and a freezing point depression constant of 4.90°C/m. d fliv ebruogrnos sniwollot srb lo rdairlW (1 (EelD) onimaly tomit (I acorous (CH3COCH?) stuloe slitslovn qps adnoone B) O 300 CISO Inioq anilam omce ori overl ls verdT (3 D)0 100 a VICI oqmot eirs s ) vilidulce ort oninnsis (E 0.26 gnivlozaib yd bonisido pexsue Ce ylienob e 26rd noituloe adt it DH arlo inalom srb noituloe 1 MS.0lo (J) omulov torW
4) In class, we derived the condition for equilibrium between a gas and the same chemical dissolved in solution Peap Poop YAXA (4) where Prap is the equilibrium pressure of the vapor, Pp, is the vapor pressure of the pure substance, 74 is the activity coefficient of A in the solution, and XA is the mole fraction of A in solution. We can define a constant, called the Henry's Law coefficient ka, such that kA = PopYA. Note that ka is a property of both the chemical A (Pp) and solvent (which determines YA). Then Equation 4 can be rewritten as Poop = KAXA (5) 1 Note that Equation 5 is essentially the same as Equation 4, but now it's easier to tabulate one constant, and values of ka can be found in tables such as Table 6.1 of Tinoco. Note that ka has units of bar, since XA is unitless (mole fraction). Using Henry's Law constants in Table 6.1 of Tinoco, calculate the solubility in M of each gas in water at 298 K if P(O2)= 0.2 bar, P(N2)= 0.75 bar, P(CO2)= 0.05 bar.
Part A - Using the definition for mole fraction. A solution was prepared by dissolving 160.0 g of KCl in 235 g of water. Calculate the mole fraction of KCl. (The formula weight of KCl is 74.6 g/mol. The formula weight of water is 18.0 g/mol) Express the mole fraction of KCl to two decimal places. ▸ View Available Hint(s) x = Submit Η ΕΕ ΑΣΦ 0 Previous Answers
A sodium sulfate solution is measured at 2.2 molal in pure water at a source company. (sodium sulfate molar mass = 142.05 g mol) The lab needs to report the concentration in molarity. What is the final molarity of the sodium sulfate solution? (density of water = 1.0 g mL¯' ; density of the solution = 1.2 g uestion 4 %3D mL-1). (the answer should be entered with 3 significant figures; do not enter units; give answer in normal notation--examples include 1.23 and 120. and -123 and 123. and 12.3) Question 4 of 29> AMoving to another question will save this response. 888. P11 64 F12 eIC " 24 4 & 7\ 3 5 6. 8. %3D dele E R T Y A S D L F G K Z C N alt alt option command command option
Air is a mixture of several gases. The 10 most abundant of these gases are listed here along with their mole fractions and molar masses. Molar mass Component Mole fraction (g/mol) 28.013 31.998 39.948 44.0099 20.183 4.003 16.043 83.80 2.0159 Nitrogen 0.78084 Oxygen 0.20948 Argon 0.00934 Carbon dioxide 0.000375 Neon 0.00001818 Helium 0.00000524 Methane 0.000002 0.00000114 Krypton Hydrogen 0.0000005 Nitrous oxide 0.0000005 44.0128 Part A What mass of carbon dioxide is present in 1.00 m³ of dry air at a temperature of 19 °C and a pressure of 687 torr? Express your answer with the appropriate units. ▸ View Available Hint(s) 0 Value Submit Part B μᾶ O Submit μÀ Value 3 Calculate the mass percentage of oxygen in dry air. Express your answer with the appropriate units. ▸ View Available Hint(s) B Units ? Units ?
The solvent for an organic reaction is prepared by mixing 70.0 mL of acetone (C3H6OC3H6O) with 56.0 mL of ethyl acetate (C4H8O2C4H8O2). This mixture is stored at 25.0 ∘C∘C. The vapor pressure and the densities for the two pure components at 25.0 ∘C∘C are given in the following table. What is the vapor pressure of the stored mixture? Compound Vapor pressure(mmHg) Density(g/mLg/mL) acetone 230.0 0.791 ethyl acetate 95.38 0.900
Given these values, find the initial mole fraction and initial mass % of the solute (sucrose) Solvent (water) weight: 200g Solute (NaCl) weight: 232g Solute (NaCl) Molar mass=342.3 moles of solute (NaCl) = .678
A solution is prepared by adding 425g of AgNO3 to 0.150L of water at 40.0∘C. The solubility of AgNO3 at 40.0∘C is 311g100.mL. How many grams of AgNO3 are expected to precipitate if the temperature is dropped to 0.00∘C where the solubility of AgNO3 is only 122g100.mL? Give the answer with three significant figures.
b Success Confirmation of Qu X < + с app.101edu.co Aktiv Chemistry X D2L Bar Graph Report - Spring x G The let-down reflex allows XCA. Fill words to blanks: Lon X Time's Up! The enthalpy of solution (AH) of KOH is -57.6 kJ/mol. If 1.56 g KOH is dissolved in enough water to make a 150.0 mL solution, what is the change in temperature (°C) of the solution? (The specific heat capacity of the solution is 4.184 J/g °C and the density of the solution is 1.02 g/mL). 1 4 7 +/- Untitled document - Google + 2 5 8 | °℃ 3 6 9 0 Update: Submit X C x 100
Use the T-xy diagram for mixtures of benzene (Mbenzene-78.11 kg/kmol) and toluene (Mtoluene-92.13 kg/mol) at 1 atm to answer the following question. Temperature (°C) 20 15 10 115 110 105 5 85858KOS 100 95 90 80 75 70 65 Vapor A mixture consisting of 15 moles of 60 mol% benzene and 40 mol% toluene at 90 °C, how much benzene (in moles) would need to be added to make the mixture all vapor? Liquid 0.6 0.8 1.0 0.2 0.4 Mole fraction benzene P = 1 atm