2022-330-EIII+ans

For each of the following-define a system and its surroundings and give directions ofheat flow. Motivate.i. Propane is burning in a laboratoryii. Two chemicals are mixed in a flask sitting on a laboratory bench

What is the concentration of SO42-ions in the solution of silver sulphate with a Kçç value of 1.1x10-5 at 25 ° C?Silver sulphate dissolves in water according to the following reaction.Ag2SO4  (k)  ...........> 2 Ag+ (aq)  + SO42-(aq) A 1.5 L solution of silver sulfate contains 3 g of dissolved silver sulphate. If extra solid silver sulfate is added to the solution, will it dissolve in the solution? (Ag: 108 g / mol, S: 32 g / mol, O: 16 g / mol)

A novel inorganic compound has two different crystalline forms, namely blue and red crystals. The physical and thermodynamic properties of blue and red crystals are given below. Mw of the novel inorganic compound is 86.54 g mol1. Properties (T = 298 K, P = 1.00 bar) Blue Red AH; (kJ mol 1) -1722.6 -1722.9 AG (KJ mol 1) -1648.5 -1647.1 Sin (U K1 mol 1) 86.4 81.2 CPm (JK1 mol 1) 66.5 65.7 Density (g mL 1) 2.145 2.278 What pressure must be achieved to induce the conversion of blue to red crystal at T = 298 K? Assume both blue and red crystals are incompressible at T = 298 K. Answer in bar to 0 decimal place (e.g. 1762)

Two students prepared aqueous solutions of LiCl and measured the properties, as shown in the table above. Both students observed that the solid LiCl readily dissolved in H2O. The students drew particle diagrams to explain the changes in the enthalpy and entropy of dissolution for LiCl based on their results and observations. Based on this information, the better particle diagram was drawn by which student, and why is that diagram more accurate? (see attached image)   a.) The better particle diagram was drawn by Student 1 because when LiCl dissolves in water, it dissociates into Li+ and Cl− ions causing an increase in entropy.   b.) The better particle diagram was drawn by Student 1 because when LiCl dissolves in water, it dissociates into Li+and Cl−ions indicating that the dissolution of LiCl is exothermic. c.) The better particle diagram was drawn by Student 2 because it shows that LiCl does not dissociate, resulting in a decrease in entropy for the dissolution of LiCl.…

1. Which, if any of the following, constitute a closed system?(a) A sealed container in which a chemical reaction occurs.(b) A dog.(c) An open beaker in the lab, in which a reaction occurs.(d) A mixture of gases inside a sealed impenetrable balloon.   2. What is the definition of an isolated system? How could you approximate anisolated system in the lab?

b) Determine the standard enthalpy change and std. Gibbs free energy change of reaction at 400 k for the reaction СO(g) +2H2(g) — CHОН (g) At 298.15 K, AH.co (0)= -26.41 kcal/mol, AH AG.co (9)= -32.8079 kcal/mol, AG cH,oh(9)= -38.69 kcal/mol, °.CH20H(9)= -48.08 kcal/mol, The standard heat capacity of various components is given by, CO = a + bT + cT² + dT³, where C, is in cal/mol-K and T is in K b x10² с х105 d x10° Соmponent CH3OH а 4.55 2.186 -0.291 -1.92 CO 6.726 0.04 0.1283 -0.5307 H2 6.952 -0.0457 0.09563 -0.2079

The following data was obtained in NASA chemical lab.Temperature (C) Solubility (x 10-21)10 1715 2120 3825 4130 4935 5340 5945 6950 7855 8660 95 Find: the equation Solubility [x10-21] = f(Temperature [K]). Provide the graph withcorresponding labels.

Part C A solution is formed when the solute unilormly disperses throughout (or dissolves in) the solvent The process can be described though three stops A hypothetical solution forms between a solid and a liquid The vakues of the thermodynamic Involved in the process are shown in the following table 1 separation of solvent-solvant particles, 2. breaking of solute-solute particles and 3. formation of solute-solvent interactions Action Enthalpy 145 kJ/mol 21.8 kJ/mol séparation of solute separation of solvent formation of solute-solvent interactions -85.7 kJ/mol solute The overall energy change for the solution process, AHa is the sum of the enthalpies of the threoe stepo. Whether AHs endothermic or exothermic depends on the relative magnitudes of AH, AH, and AH, where the subscript Indicates the step in the process corresponding to the enthalpy value Calculate the enthalpy of solution in kilojoules per mole of solute Enter your answer numerically in kilojoules per mole of solute. > View…

A edu.co g Ce... Aktiv Chemistry $ R F5 Hess's law can be used to solve for reaction enthalpy changes because enthalpy is a function. ► 11 k % 5 F6 6 + A) path B) state C) thermodynamic F7 D) pressure-volume Question 8 of 12 F8 & 7 F9 * 8 P 1 K F10 ( 9 F11 O F12 P PrtScr "Kº ( + Insert 604x Delete O PgUp

In a thermodynamic study, a scientist focuses on the propertiesof a solution in an apparatus as illustrated. A solution iscontinuously flowing into the apparatus at the top and out atthe bottom, such that the amount of solution in the apparatusis constant with time. (a) Is the solution in the apparatusa closed system, open system, or isolated system? (b) If the inletand outlet were closed, what type of system would it be?

C6H12O6(aq) + 6O2(g) 6CO2(g) + 6H2O(l)ΔH = –2802.7 kJ mol –1a) Write an expression for the equilibrium constant for this reaction.b) At equilibrium, the concentration of the reactants and products are determined as [CO2] = 0.30 M, [O2] = 0.040 M and [C6H12O6] = 0.065 M. Determine the value of the equilibrium constant (Kc) and predict the whether the products or reactants will be favoured at equilibrium.c) Given that the concentrations of the reactants and products at a particular time are [CO2] = 0.65 M, [O2] = 0.020 M and [C6H12O6] = 0.055 M, determine the reaction quotient (Qc). Compare the Kc and Qc values and predict the favoured direction of the reaction.d) Explain the effect on equilibrium of:i) Increasing temperatureii) Increasing pressureiii) Decreasing the concentration of oxygeniv) Increasing the concentration of carbon dioxidev) Adding a catalyst

The rise in atmospheric carbon dioxide results in higher concentrations of dissolved carbon dioxide in natural waters. Use Henry's law and Henry's constants found online to calculate the solubility of CO2 in water at 25°C when its partial pressure is 100 kPa.  Ans: 33.9 mmol/dm3

-4 The solubility of Co(OH), in water at 25 °C is measured to be 6.4 x 10 Use this information to calculate K,, for L Co(OH),. Round your answer to 2 significant digits.

The solubility of KNO; (in gr KNO; per 100 gr water) is 155 gr KNO; at 75 °C and 38 gr KNO3 at 25 °C. What mass of KNO; (in grams) will crystallize out of solution if exactly 100 gr of its saturated solution at 75 °C are cooled to 25 °C? О а. 75.4 gr оь. 45.9 gr 110 gr O d. 30.7 gr

The amount of oil and grease from the rivers beside mining sites are quantified by solvent-solvent extraction. The dissolved oil and grease from the organic solvent will then be dried and weighed. What type of gravimetry is described by the statement? O precipitation gravimetry O physical gravimetry thermogravimetry electrogravimetry

In the gas phase reaction 2 A(g) + B(g) 3 C (g) + 2 D (g), it was found that when 1.00 mol A, 2.00 mol B and 1.00 mol D were mixed and allowed to come to equilibrium at 25°C, the resulting mixture contained 0.9 mol C at a total pressure of 1.00 bar. Calculate the mole fractions of each species , Kx is , Kp is and A GO is

Non-Commercial Substances Hypothesis: Soluble in Test Bond Molecular Structure ΔΕΝ H2O? Result: H20 Solubility Result: Hexane Substance Classification Solubility Hexane? H2O: pS Sodium Na--Br lonic Bromide 1.9 Hexane: I |--| lodine NP C 0.0 Ammonium N/A lonic Carbonate NH4* O O NH4* Sodium N/A lonic Acetate C--H NP C 0.4 H-C-OH C--O PC H-C-OH Glycerol 1.0 H-C-OH O--H PC 1.4 HI

Calculate the mean ionic molality for 0.25m LaCls. [Ans. 1.1914 m] 570 nsmer For aqueous HCl solutions, it can be determined: Y- =0.72515 + 0.029188m + 0.055959m Determine the molality at which auCi= 1. (Note: This is the molality for the standard state of HCL in Water; pHCI) [Ans. 1.1914 m] %3D

Lead hydroxide, Pb(0H)2(s) | Pb(0H)2(s)Pb+2(aq)+20H-(aq) | Ksp=1.4x10-20 H2O(aq)H*(aq)+OH-(aq) Pb(OH)2 Water Kw=1.00x10-14 Molar masses 241.21 Pb 207.20 OH- 17.01 If Pb+2(aq) is controlled by the solubility of Pb(OH)2, what Pb+2(aq) concentration is expected if pH=p0H=7.00? b. What pH would be required to lower Pb+2(aq) to 2.07 ppb? a.

You carry out an experiment on the physical properties of 3 organic compounds and observe the following data: Substance Solubility in Water medium Compound A low Compound B high Compound C You know that the 3 organic compounds are an alkene, ketone and alcohol of equal hydrocarbon length. Match the compounds above to their specific organic compound type based upon their solubility. And give a structural reason for the solubility observations that are observed. (I:3) Substance Identity Reason Compound A Compound B Compound C

1. The concept of gas collisions can be applied to the study of metrology. Being the highest composition in atmospheric air (78% by volume), N2 has a collision diameter of 0.369 x 10° m. At 298 K and 1 atm, calculate the single collision frequency of N2 at sea level. The collision frequency of N2 decreases at higher altitude. At 11 km from the sea level, the collision frequency is 3.16 x 10° s-1. Calculate the pressure of the gas at this altitude (T = – 220 K). Determine the mean free path for N2 at the altitude of 11 km (the altitude similar in Question 1.ii.) i. ii. i.

b) Determine the standard enthalpy change and std. Gibbs free energy change of reaction at 400 k for the reaction Co(g) +2H2(g) → CH;OH (g) At 298.15 K, AH?.co )= -26.41 kcal/mol, AH?.CH,OH()= -48.08 kcal/mol, AG.co )= -32.8079 kcal/mol, AG.CH,OH(@)= -38.69 kcal/mol, The standard heat capacity of various components is given by. CS = a + bT + cT2 + dT³, where C is in cal/mol-K and T is in K |Component b x10 e x105 d x10° a -0.291 CH3OH CO 4.55 2.186 -1.92 6.726 0.04 0.1283 -0.5307 H2 6.952 -0.0457 0.09563 -0.2079

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P5B.4* Equation 5B.14 indicates, after it has been converted into an expression for x, that solubility is an exponential function of temperature. The data in the table below gives the solubility, S, of calcium ethanoate in water as a function of temperature. 20 40 60 80 S/(g/100 g solvent) 36.4 34.9 33.7 32.7 31.7 Determine the extent to which the data fit the exponential S= S,e"" and obtain values for S, and r. Express these constants in terms of properties of T/T the solute.

. Complete and balance each of the following equations. If no reaction occurs, enter NOREACTION. tab os lock esc ~ control D S ! 1 FT Q A 1 option Z 2 W S X # 3 command H BO F3 E D $ 4 C Pb(NO3)2(aq) + KCl(aq) → Express your answer as a chemical equation. Enter NOREACTION if no reaction occurs. Identify all of the phases in your answer. FA == | ΑΣΦ R Submit Part B F A chemical reaction does not occur for this question. Nal(aq) + Hg, (C₂H₂O₂)2(aq) → Express your answer as a chemical equation. Enter NOREACTION if no reaction occurs. Identify all of the phases in your answer. — | ΑΣΦ | 4 Request Answer 5 V @ A chemical reaction does not occur for this question. Submit Request Answer X T G 6 MacBook Air B Y ? H & 7 ? 77 U N 8 Dil W I M ( 9 K DO F O . – : ; I { option [ + = = ? 1 11 I 34 F12 } 1 + delet A

For the reaction below, formation salpies at 1 bar and standart entropies are given. Çe te equilibrium constant (Kp) of the reaction at 580 K. X(g) +3 Y,(g) =2XY,(g) For X,(g) AHº,f =0 kJ mol S° = 179 J mol* K For Y(g) AH°f = 0kJ mol* S° = 215 J mol"K** For XY,(g) AH°f = -146 kJ mol" S° = 154 mol K* R = 0.08206 L atm mol-1 K-1 = 8.314 J mol-1 K-1

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?

General Chemistry 4th Edition McQuarrie • Rock • Gallogly University Science Books presented by Macmillan Learning A critical reaction in the production of energy to do work or drive chemical reactions in biological systems is the hydrolysis of adenosine triphosphate, ATP, to adenosine diphosphate, ADP, as described by the reaction АТР(аq) + H,О() — ADP(aq) + HРО (аq) ADP(aq) + HPO, (aq) for which AG;ixn = -30.5 kJ/mol at 37.0 °C and pH 7.0. Calculate the value of AGrxn in a biological cell in which [ATP] = 5.0 mM, [ADP] = 0.10 mM, and [HPO;-] = 5.0 mM. kJ/mol rxn Is the hydrolysis of ATP spontaneous under these conditions? О yes no Question Source: McQuarrie, Rock, And Gallogly 4e - General Chemsitry | Publisher: University Science Books ?

When 50 cm3 of hydrochloric acid of concentration 2.0 mol dm−3 is added to 50 cm3 ofsodium hydroxide solution of concentration 2.0 mol dm−3, the temperature increase is 13.0 qC.HCl(aq) + NaOH(aq) NaCl(aq) + H2O(l) The experiment is repeated using 25 cm3 of the same hydrochloric acid and 50 cm3 ofthe same sodium hydroxide solution. What is the temperature increase?

Using the Kf and Kb equations with electrolytes A certain liquid X has a normal boiling point of 110.90 °C and a boiling point elevation constant K=1.66 °C-kg mol -1 .A solution is prepared by dissolving some ammonium sulfate ((NH SO,) in 150.g of X. This solution boils at 112.2 °C. Calculate the mass of (NH), SO, that was dissolved. Round your answer to 2 significant digits. ? Explanation Check ©2022 McGraw Hill LLC. All Rights Reserved. Terms of Use Privacy Center | étv A

A mixture of isobutylene ((CH3)2CCH2, 0.400 bar partial pressure) and HCI (0.600 bar partial pressure) is heated at 500.0 K. The equilibrium constant K for the gas- phase thermal decomposition of tert- butyl chloride ((CH3)3CCI) is 3.45 at 500.0 K. bar (CH3);CCI(g) = (CH3)2CCH2(g) + HCI(g) 1 3 What is the partial pressure of isobutylene ((CH3)2CCH2) at equilibrium? 4 C 8. 9. +/- х 100

A mixture of isobutylene ((CH3)2CCH2, 0.400 bar partial pressure) and HCI (0.600 bar partial pressure) is heated at 500.0 K. The equilibrium constant K for the gas- phase thermal decomposition of tert- butyl chloride ((CH3)3CCI) is 3.45 at 500.0 K. bar (CH3);CCI(g) = (CH3)2CCH2(g) + HCI(g) 1 3 You have calculated the equilibrium partial pressures to be: 4 C tert-butyl chloride,CH3);CCI = (x) hydrochloric acid, HCI = (0.600 - x) isobutylene, (CH3)2CCH2 = (0.400 - x) What is the partial pressure of tert- butyl chloride ((CH3)3CCI) at equilibrium? 8. 9. +/- х 100

) Determine the standard enthalpy change and std. Gibbs free energy change of reaction at 400 k for the reaction Co(g) +2H2(g) → CH;OH (g) At 298.15 K, AH?,co (»= -26.41 kcal/mol, AH9,cH,0H(0)= -48.08 kcal/mol, AG,co ()= -32.8079 kcal/mol, AG?.cH,oH()= -38.69 kcal/mol, The standard heat capacity of various components is given by, C = a + bT + cT² + dT³, where C§ is in cal/mol-K and T is in K |Component CH;OH CO b x10 с х105 -0.291 0.1283 a d ×10" 4.55 6.726 2.186 0.04 -0.0457 -1.92 -0.5307 -0.2079 6.952 0.09563