Which of the following would be immiscible

1 of 20Which of the following would be immiscible (NOT soluble) with water?NH3Which intermolecular force or bond is primarily responsible for the solubility of NaCl inwater?Hydrogen bondingIonic bondingCovalent bondingIon-dipole forceDipole-dipole forceThe solubility of CO2 gas in water ________ with ________ gas pressure.increases; increasingincreases; decreasingdecreases; increasingdecreases; decreasingis not dependent on pressure4 of 20The solubility of calcium chloride is 74.5 g per 100.0 g of water at 20°C. The amount ofwater needed to dissolve 271 g of calcium chloride at 20°C is202 g255 g345 g364 g446 g5 of 20If 4.49 g NaNO3 (FW = 85.0 g/mol) is dissolved in enough water to make 250.0 mL ofsolution, what is the molarity of the sodium nitrate solution?1.32 x 10–2 M1.80 x 10–2 M2.11 x 10–1 M5.28 x 10–2 M18.0 M6 of 20What is the chloride ion concentration in a 1.7 M calcium chloride solution?0.85 M1.7 M3.4 M4.3 M5.1 M7 of 20The weight percent of concentrated HClO4(aq), molar mass = 100.5 g/mol, is 70.5% and itsdensity is 1.67 g/mL. What is the molarity of concentrated HClO4?4.20 M7.18 M11.7 M14.2 M39.7 M8 of 20How many liters of 0.1107 M KCl contain 15.00 g of KCl (FW = 74.6 g/mol)?0.02227 L0.5502 L1.661 L1.816 L18.16 L9 of 20A solution is prepared by dissolving 2.0 g NaOH (FW = 40.0 g/mol) to 255 mL of solution. Ifthe density of the solution is 1.15 g/mL, what is the mass percent NaOH in the solution?0.68 %0.78 %0.90 %6.8 %7.8 %10 of 20What is the percent CsCl by mass in a 0.711 M CsCl solution that has a density of 1.091g/mL?3.87 x 10-1 %3.87 x 10-4 %6.5 x 10-2 %1.1 %11.0 %11 of 20In how many grams of water should 25.31 g of potassium nitrate (KNO3; FW=101.1 g/mol)) be dissolved to prepare a 0.1982 m solution?250.0 g792 g1,000 g1,263 g7,917 g12 of 20The density of a 20.3 M CH3OH (methanol); MW=32.0 g/mol; solution is 0.858 g/mL. Whatis the molality of this solution? H2O is the solvent.17.4 m20.8 m23.7 m70.0 m97.6 m13 of 20How much water would be needed to prepare 500.0 mL of a 0.100 M NaOH solution from a2.0 M NaOH solution?2.0 mL25.0 mL50.0 mL475.0 mL500.0 mL14 of 20If 5.00 mL of 0.314 M KOH is diluted to exactly 125 mL with water, what is the masspercent concentration of the resulting solution?1.26 x 10-2 %5.02 x 10-4 %0.127 %0.281 %Can’t determine the concentration because you need the density of the solution15 of 20Arrange the following aqueous solutions in order of increasing boiling points.0.050 m Mg(NO3)2; 0.100 m ethanol; 0.090 m NaClEthanol < Mg(NO3)2 < NaClMg(NO3)2 < NaCl < ethanolMg(NO3)2 < ethanol < NaClNaCl < ethanol < Mg(NO3)2Ethanol < NaCl < Mg(NO3)216 of 20What is the boiling point of a solution containing 2.33 g of caffeine, C8H10N4O2; MW=194.0g/mol; dissolved in 15.0 g of benzene? The boiling point of pure benzene is 80.1 °C and theboiling point elevation constant, Kb is 2.53 °C/m.2.02 °C78.1 °C80.2 °C82.1 °C83.3 °C17 of 20What is the molar mass of toluene if 0.85 g of toluene depresses the freezing point of 1.00 x102 g of benzene by 0.47°C? Kf of benzene is 5.12°C/m.10.7 g/mol78.0 g/mol81.8 g/mol92.6 g/mol927 g/mol18 of 20The percent composition by mass of a compound is 76.0% C, 12.8% H, and 11.2% O. Asolution of 1.18 g of this compound dissolved in 10.0 g of benzene freezes at 3.37 °C. Whatis the molecular formula of this compound? The normal freezing point of benzene is 5.50°C and it has a Kf of 5.12 °C/m.C9H18OC10H6OC16H28O4C18H36O2C20H12O219 of 20A solution of ethylene glycol in water such as in an antifreeze solution has a boiling point> 100°C and a freezing point > 0°C.> 100°C and a freezing point < 0°C.> 100°C and a freezing point = 0°C.< 100°C and a freezing point > 0 °C.and a freezing point close to that of ethylene glycol.20 of 20The osmotic pressure of blood is 7.65 atm at 37 °C. What mass of glucose C6H12O6, molarmass = 180.2 g/mol is needed to prepare 5.00 L of solution for intravenous injection? Theosmotic pressure of the glucose solution must equal the osmotic pressure of blood.(π = MRT; R=0.082 L atm/mol K)1.50 g54.2 g126 g271 g2270 g1 of 10According to collision theory, which condition(s) must be met in order for molecules toreact?1. The reacting molecules must collide with sufficient energy to initiate the process ofbreaking and forming bonds.2. A catalyst must be in contact with the reacting molecules for a reaction to occur.3. The reacting molecules must collide with an orientation that can lead to rearrangementof the atoms.1 only2 only3 only1 and 21 and 32 of 10For the reaction 2A + B –> C, the rate law isWhich of the factors will affect the value of the rate constant for this reaction?1. decreasing the temperature2. adding a catalyst3. decreasing the concentration of reactant A1 only2 only3 only1 and 22 and 33 of 10A catalystincreases the activation energyincreases the average kinetic energy of the reactantsincreases the collision frequency of reactant moleculesincreases the concentration of reactantsalters the reaction mechanism4 of 10For the reaction below, if the rate of appearance of Br2 is 0.180 M/s, what is the rate ofdisappearance of NOBr?2 NOBr(g) –> 2 NO(g) + Br2(g)–0.360 M/s–0.090 M/s0.090 M/s0.180 M/s0.720 M/s5 of 10Ammonium ion (NH4+) reacts with nitrite ion (NO2-) to yield nitrogen gas and liquid water.The following initial rates of reaction have been measured for the given reactantconcentrations:Which of the following is the rate law (rate equation) for this reaction?rate = k [NH4+][NO2-]4rate = k [NH4+][NO2-]2rate = k [NH4+]1/2[NO2-]1/4rate = k [NH4+][NO2-]rate = k [NH4+]2[NO2-]6 of 10The first-order reaction SO2Cl2 –> SO2 + Cl2 is 10% complete in 80 min. How long would ittake for the reaction to be 95% complete?1.8 min104 min530 min990 min2300 min7 of 10The decomposition of hydrogen peroxide follows first order kinetics and has a rate constantof 2.54 x 10-4 s-1 at a certain temperature. If the concentration of hydrogen peroxide is 0.321M after 855 s , what was the initial concentration of hydrogen peroxide at thistemperature?0.258 M0.399 M0.538 M0.677 M1.48 M8 of 10What is the half-life of a first-order reaction if the rate constant is 6.2 x 10–3 s–1?0.097 s5.77 s1.0 x 102 s1.6 x 102 s8.9 x 10–3 s9 of 10For the second-order reaction below, the initial concentration of reactant A is 0.24 M. If therate constant for the reaction is 1.5 x10–2 M–1s–1, what is the concentration of A after 265seconds?2A –> B + Crate = k[A]20.12 M0.19 M0.95 M4.0 M5.2 M10 of 10The decomposition of nitrogen dioxide2 NO2(g) –> 2 NO(g) + O2(g)is second order with a rate constant of 0.790s -1. It takes 125 seconds for the concentrationof NO2(g) to go from an initial concentration 0.800 M to 0.010 M. What is the half-life forthis reaction?0.790 s0.913 s1.58 s2.64 s125 s1 of 10Which of the following statements is/are CORRECT?1. For a chemical system, if the reaction quotient (Q) is greater than K, reactant must beconverted to products to reach equilibrium.2. For a chemical system at equilibrium, the forward and reverse rates of reaction areequal.3. For a chemical system at equilibrium, the concentrations of products divided by theconcentrations of reactants equals one.1 only2 only3 only1 and 21, 2, and 32 of 10Indicate the expression for Kp for the reaction below.MgCO3(s)MgO(s) + CO2(g)3 of 10Indicate a balanced chemical equation that corresponds to the following equilibriumconstant expression.H+(aq) + OH–(aq)H2O( )HNO2(aq) + H2O( )NO2–(aq) + H3O+(aq)HNO2(aq)NO2–(aq) + H3O+(aq)HNO2(aq)NO2–(aq) + H3O+(aq)NO2–(aq) + H3O+(aq)HNO2(aq) + H2O( )4 of 10The following reactions occur at 500 K. Arrange them in order of increasing tendency toproceed to completion (least completion –> greatest completion).2<1<3<43<1<4<23<4<1<24<3<1<24<3<2<15 of 10At 700 K, the reaction2SO2(g) + O2(g)2SO3(g)has the equilibrium constant Kc = 4.3 x 106, and the following concentrations are present:[SO2] = 0.10 M; [SO3] = 10. M; [O2] = 0.10 M.Is the mixture at equilibrium? If NOT at equilibrium, in which direction (as the equation iswritten), left to right or right to left, will the reaction proceed to reach equilibrium?Yes, the mixture is at equilibrium.No, left to right.No, right to left.There is not enough information to be able to predict the direction.6 of 10At a high temperature, equal concentrations of 0.160 mol/L of H2(g) and I2(g) are initiallypresent in a flask. The H2 and I2 react according to the balanced equation below.H2(g) + I2(g)2 HI(g)When equilibrium is reached, the concentration of H2(g) has decreased to 0.036 mol/L.What is the equilibrium constant, Kc, for the reaction?3.44.01222487 of 10For the reactionSO2(g) + NO2(g)SO3(g) + NO(g), the equilibrium constant is 18.0 at 1,200ºC. If 2.0moles of SO2 and 2.0 moles of NO2 are placed in a 20. L container, what concentration ofSO3 will be present at equilibrium?0.081 mol/L0.019 mol/L0.11 mol/L1.00 mol/L18 mol/L8 of 10The equilibrium constant (Kc) for the following reaction is 6.7 x 10–10 at 630 °C.N2(s) + O2(g)2 NO(g)What is the equilibrium constant for the reaction below at the same temperature?1/2 N2(g) + 1/2 O2(g)NO(g)1.3 x 10-91.8 x 10-52.6 x 10-53.4 x 10-104.5 x 10-199 of 10For the following reaction at equilibrium, which one of the changes below would cause theequilibrium to shift to the left?2NOBr(g) ↔ 2NO(g) + Br2(g), Hºrxn = 30 kJ/molRemove some NO.Remove some Br2.Add more NOBr.Increase the container volume.Decrease the temperature.10 of 10For the systemSiO2(s) + 4 HF(g) ↔ 4 SiF4(g) + 2 H2O(g) ΔH = 156 kJa shift to produce more SiF4(g) would occur ifthe concentration of H2O(g) is increasedthe concentration of HF(g) is increasedsome SiO2(s) is removedthe volume of the container is decreasedthe temperature of the container is decreased1 of 20Which is NOT a characteristic property of acids?Neutralizes basesTurns litmus from blue to redTastes sourReacts with metals to yield CO2 gasReacts with carbonates to yield CO2 gas2 of 20Identify the major ions present in an aqueous HNO3 solution.OH-, NOOH-, NO3H+, NO3HN+, O2H+, N3-, O23 of 20According to the Arrhenius concept, which of the following substances is NOT a base inaqueous solutions?H2ONH3Ca(OH)2LiOHNaOH4 of 20All of the following acids are weak EXCEPTNaH2PO4H2CO3HNO2HNO3H3PO45 of 20Arrange the following compounds in increasing order of pH. Assume all are 1.0 Msolutions. (Ka HNO2 = 3.7 x 10-4; Kb NH3 = 1.8 x 10-5)NaClNaOHHNO3NH4ClNaNO2HNO3, NaNO2, NaCl, NH4Cl, NaOHHNO3, NaNO2, NaCl, NaOH, NH4ClHNO3, NH4Cl, NaCl, NaNO2, NaOHNaCl, NaOH, HNO3, NH4Cl, NaNO2NaCl, HNO3, NH4Cl, NaNO2, NaOH6 of 20Arrange the acids H2Se, H2Te, and H2S in order of increasing acid strength.H2S < H2Se < H2TeH2S < H2Te < H2SeH2Te < H2S < H2SeH2Se < H2S < H2TeH2Se < H2Te < H2S7 of 20Identify the conjugate base of HClO3 in the reactionClO3- + HSO4- ↔ HClO3 + SO42OHH3O+HSO4SO42ClO38 of 20Seawater has a hydroxide ion concentration of 2.0 x 10-6 M. What is the pH of seawater?-8.30-5.705.708.305.00 x 10-99 of 20The pOH of a solution is 10.40. Calculate the hydrogen ion concentration in the solution.3.6 M1.8 x 10-4 M2.5 x 10-4 M4.0 x 10-11 M4.0 x 10-10 M10 of 20What is the pH of 0.250 M HCl?0.6001.202.5012.013.411 of 20What is the pH of a 0.014 M Ca(OH)2 solution?1.551.8512.1512.4515.8512 of 20A 0.10 M NH3 solution is 1.3% ionized. Calculate the H+ ion concentration.NH3 + H2ONH4+ + OH0.10 M0.13 M1.3 x 10-3 M7.7 x 10-12 M7.7 x 10-2 M13 of 20What is the pH of 0.30 M aqueous formic acid? (Ka of HCO2H = 1.8 x 10–4)0.521.612.143.744.2414 of 20A tablet of a common over-the-counter drug contains 2.00 x 102 mg of caffeine (C8H10N4O2;molar mass = 194.0 g/mol). What is the pH of the solution resulting from the dissolution oftwo of these tablets in 225. mL of water at 25oC? (For caffeine, Kb = 4.1 x 10-4.)2.766.337.6710.9611.2415 of 20What is the chemical formula of the salt produced by the neutralization of nitric acid withcalcium hydroxide?CaNO3Ca(NO3)2Ca2NO3Ca2(NO3)3Ca3(NO3)216 of 20Predict the direction in which the equilibrium will lie for the reactionC6H5COO- + HFC6H5COOH + F-.Ka(C6H5COOH) = 6.5 x 10-5; Ka(HF) = 7.1 x 10-4To the rightIn the middleTo the left17 of 20For H3PO4, Ka1 = 7.3 x 10-3, Ka2 = 6.2 x 10-6, and Ka3 = 4.8 x 10-13. An aqueous solution ofNaH2PO4 therefore would bebasicacidicneutral18 of 20Which of these salts will form a neutral solution on dissolving in water?NH4NO3NaCNFeCl3NaClKNO219 of 20What mass of sodium fluoride (FW=42.0 g/mol) must be added to 3.50 x 102 mL of water togive a solution with pH = 8.40? [Ka(HF) = 7.1 x 10-4]0.039 g6.6 g24 g68 g1.7 x 10-4 g20 of 20What is the pH of 0.50 M NaOCl if the Ka for HOCl is 3.5 x 10-8?3.47.07.2810.61 of 10Which of the following combinations CANNOT function as a buffer solution?HCl and NaOHH2CO3 and NaHCO3HF and NaFNH3 and (NH4)2SO4HCN and KCN2 of 10Which of the following combinations of acids and conjugate bases would be the best tocreate a pH = 7.0 buffer?H2PO4- (Ka = 6.2 x 10-8) and HPO4-2HNO2 (Ka = 4.5 x 10-4) and NO2NH4+ (Ka = 5.7 x 10-10) and NH3H3PO4 (Ka = 7.5 x 10-3) and H2PO4Equal amounts of HCl and NaCl3 of 10Calculate the pH of a buffer solution that contains 0.25 M benzoic acid (C 6H5CO2H) and0.15 M sodium benzoate (C6H5CO2Na). [Ka = 6.5 x 10-5 for benzoic acid]3.403.974.194.414.834 of 10The Ka of hydrofluoric acid, HF, is 7.2 x 10-4. What [F-]/[HF] ratio is necessary to make abuffer of 2.84?0.502.02.51.4 x 10-37.1 x 1025 of 10Hydrofluoric acid has a pKa value of 3.14. What is the value of pKb for fluoride ion?3.1410.8617.141.4 x 10–117.2 x 10–46 of 10Which of the following equations represents the reaction of a weak acid with a strong base?H+(aq) + OH-(aq) H2O(aq)H+(aq) + CH3NH2(aq) CH3NH3+(aq)OH-(aq) + HCN(aq) H2O(aq) + CN-(aq)HCN(aq) + CH3NH2(aq) CH3NH3+(aq) + CN-(aq)7 of 10What is the pH of the solution that results from mixing 75 mL of 0.50 M NH3(aq) and 75mL of 0.50 HCl(aq) at 25 xC? (Kb for NH3 = 1.8 x 10–5)0.602.674.744.939.268 of 10A volume of 25.0 mL of 0.100 M C6H5CO2H(aq) is titrated with 0.100 M NaOH(aq). What isthe pH after the addition of 12.5 mL of NaOH? (Ka of benzoic acid = 6.3 x 10–5)2.604.205.407.008.609 of 10Which one of the following conditions is always true for a titration of a weak acid with astrong base?If a colored indicator is used, it must change color rapidly in the weak acid’s bufferregion.Equal volumes of weak acid and strong base are required to reach the equivalencepoint.A colored indicator with a pKa less than 7 should be used.The equivalence point occurs at a pH equal to 7.The equivalence point occurs at a pH greater than 7.10 of 10A 5.95 g sample of an acid, H2X requires 45.0 mL of a 0.500 M NaOH solution for completereaction (removing both protons). The molar mass of the acid is132 g/mol178 g/mol264 g/mol529 g/mol735 g/mol1 of 10A central metal atom bonded to surrounding ions or molecules is called acoordination compoundchelateligandLewis baseLewis acid2 of 10In the reaction CaO(s) + SO2(g) ↔ CaSO3(s),SO42- acts as a Lewis base, and SO2 acts as a Lewis acidO2- acts as a Lewis base, and SO2 acts as a Lewis acidCa2+ acts as a Lewis base, and SO42- acts as a Lewis acidSO2 acts as a Lewis base, and O2- acts as a Lewis acidSO2 acts as a Lewis base, and Ca2+ acts as a Lewis acid3 of 10All of the following species can behave as Lewis bases EXCEPTOHAl+3NH3FH2O4 of 10What is the coordination number of chromium in the following complex?[Cr(C2O4)2(H2O)2]+2245685 of 10What is the ionic charge of cobalt ion in [Co(en)2(OH)2]Cl?-1+1+3+4+66 of 10In the coordination compound [Cr(NH3)2(en)Cl2]Br2, the coordination number (C.N.) andoxidation number (O.N.) of the metal atom areC.N. = 4; O.N. = +3C.N. = 5; O.N. = +2C.N. = 5; O.N. = +4C.N. = 6; O.N. = +3C.N. = 6; O.N. = +47 of 10What is the percent copper in the sulfate salt of [Cu(NH3)4]2+?12.6%19.6%24.3%27.9%48.3%8 of 10The formula for the complex formed by Cr+3 with two ethylenediamine molecules (en) andtwo sulfate ions would be[Cr(en)2(SO4)2]3+[Cr(en)2(SO3)2][Cr(en)2(SO4)2][Cr(en)2(SO4)2][Cr(en)2(SO3)2]9 of 10The best name for [Co(en)2Br2]Br isdibromodiethylenediaaminecobalt(III) bromidedibromobis(ethylenediamine)cobalt(III) bromidedibromidedi(ethylenediamine)cobalt(III) bromidecobalt(III)bis(ethylenediamine) bromidetribromobis(ethylenediamine)cobalt(III)10 of 10What is the formula for dicyanobis(ethylenediamine)zirconium(IV) nitrate?[Zr(NO3)2(en)2](CN)2[Zr(CN)2(en)2](NO3)2[Zr(CN)2(NO3)2(en)2]Zr[(CN)2(NO3)2(en)2](NO3)2[Zr(CN)2(en)2]Question1 of 10What is the equilibrium constant expression for dissolving iron (III) hydroxide in water?Ksp = [Fe+3] + [OH-]3Ksp = [Fe+3] [OH-]3Ksp = [Fe+3] [OH-]2Ksp = [Fe+3]3 [OH-]Ksp = [Fe+3] [OH-]2 of 10The following anions can be separated by precipitation as silver salts: Cl–, Br –, I–, CrO42–. IfAg+ is added to a solution containing the four anions, each at a concentration of 0.10 M, inwhat order will they precipitate?CompoundKspAgCl1.8 x 10–10Ag2CrO41.1 x 10–12AgBr5.4 x 10–13AgI8.5 x 10–17AgCl ® Ag2CrO4 à AgBr à AgIAgI à AgBr à AgCl à Ag2CrO4AgI à AgBr à Ag2CrO4 à AgClAg2CrO4 à AgCl à AgBr à AgIAg2CrO4 à AgI à AgBr à AgCl3 of 10Consider the equilibrium of Mg(OH)2(s) in water:Mg(OH)2(s) ↔ Mg+2 + 2 OHWhat is the effect of lowering the pH of the solution?Mg(OH)2 precipitates.Mg+2 is reduced to Mg.The concentration of hydroxide ion increases.The concentration of Mg+2 decreases.None of the above4 of 10The solubility of strontium carbonate (FW=147.6 g/mol) is 0.0011 g/100 mL at 20°C.Calculate the Ksp value for this compound.1.5 x 10-31.5 x 10-45.6 x 10-97.5 x 10-57.5 x 10-65 of 10The molar solubility of silver sulfate Ag2(SO4) is 1.5 x 10-2 mol/L. What is the Ksp for thiscompound?1.4 x 10-51.5 x 10-22.3 x 10-42.8 x 10-143.5 x 10-66 of 10Calculate the silver ion concentration in a saturated solution of silver(I) carbonate (Ksp =8.1 x 10-12).1.3 x 10-4 M2.0 x 10-4 M2.5 x 10-4 M5.0 x 10-5 M8.1 x 10-4 M7 of 10The Ksp for silver(I) phosphate is 1.8 x 10-18. Calculate the molar solubility of silver(I)phosphate.1.6 x 10-5 M1.8 x 10-1 M2.1 x 10-5 M3.7 x 10-5 M7.2 x 10-1 M8 of 10What is the molar solubility of Mn(OH)2(s) in a solution that is buffered at pH 8.00 at25°C? The Ksp of Mn(OH)2 is 1.9 x 10–13 at 25°C.1.9 x 10–7 mol/L1.9 x 10–1 mol/L1.9 x 103 mol/L3.6 x 10–8 mol/L3.6 x 10–5 mol/L9 of 10At what pH will a 0.15 M Cu+2 begin to precipitate as Cu(OH)2? The Ksp for Cu(OH)2 is 1.6x 10-19 M.5.017.007.537.838.9910 of 10What mass of KCl (molar mass = 74.55 g/mol) must be added to 1.0 L of 0.0180 M Pb2+(aq)to initiate precipitation of PbCl2(s)? The Ksp of PbCl2 is 1.7 x 10–5. Assume no volumechange occurs upon addition of KCl.0.041 g0.070 g2.3 g2.5 g6.6 x 10–5 g1 of 10Thermodynamics can be used to determine all of the following EXCEPTthe entropy change of a reactionthe temperature at which a reaction is spontaneousthe rate of reactionthe direction in which a reaction is spontaneousthe extent to which a reaction occurs2 of 10Which of the following statements is/are CORRECT?1. Spontaneous changes only occur in the direction that leads to equilibrium.2. Exothermic reactions are always spontaneous.3. In any chemical reaction, energy must be conserved.1 only2 only3 only1 and 31, 2, and 33 of 10Which of the following processes is/are exothermic?1. the reaction of butane with oxygen2. the melting of gold3. cooling copper from 225°C to 65°C1 only2 only3 only1 and 31, 2, and 34 of 10If a cube of ice at 0oC is placed outside on a warm summer day, the ice will meltspontaneously. What are the signs of ΔH, ΔS, and ΔG for this process?ΔH < 0, ΔS > 0, ΔG > 0ΔH < 0, ΔS > 0, ΔG < 0ΔH < 0, ΔS < 0, ΔG < 0ΔH > 0, ΔS > 0, ΔG < 0ΔH > 0, ΔS < 0, ΔG > 05 of 10Which of these species has the highest entropy (So) at 25oC?CH4(g)NaCl(s)CO(g)Fe(s)H2O(l)6 of 10Without reference to a table, arrange these reactions according to increasing S.1<3<22<1<32<3<13<1<23<2<17 of 10Calculate the standard entropy change for the combustion of ethanol at 25°C.CH3CH2OH( ) + 3 O2(g) D 2 CO2(g) + 3 H2O(g)SpeciesCH3CH2OH( )O2(g)CO2(g)H2O(g)S° (J/K mol)160.7205.1213.7188.8–35.9 J/K+35.9 J/K+217.8 J/K+422.9 J/K+833.1 J/K8 of 10For a particular chemical reaction∆H = 5.5 kJ and ∆S = -25J/KUnder what temperature condition is the reaction spontaneous?When T < -220 KWhen T < 220 KWhen T > 220 KAt all temperaturesNot at any temperature9 of 10Determine G° for the following reaction:CH4(g) + O2(g) à CO2(g) + 2 H2O(g)given fG° [CH4(g)] = –50.7 kJ/mol, fG° [H2O((g)] = –237.4 kJ/mol,fG° [O2(g)] = 0.0 kJ/mol, and fG° [CO2(g)] = –394.4 J/mol.106.3 kJ130.4 kJ207.7 kJ818.5 kJ943.1 kJ10 of 10Sodium carbonate can be made by heating sodium bicarbonate:2 NaHCO3(s) Na2CO3(s) + CO2(g) + H2O(g)Given that Ho = 128.9 kJ/mol and So = 321.0 J/K at 25oC, above what minimumtemperature will the reaction become spontaneous under standard state conditions?4.0 K25.0°C128.9°C273.0°C402°C1 of 10Assuming the following reaction proceeds in the forward direction:3 Sn4+(aq) + 2 Cr(s) D 3 Sn2+(aq) + 2 Cr3+(aq)Sn4+(aq) is the reducing agent and Cr(s) is the oxidizing agentSn4+(aq) is the reducing agent and Sn2+(aq) is the oxidizing agentCr(s) is the reducing agent and Cr3+(aq) is the oxidizing agentCr(s) is the reducing agent and Sn2+(aq) is the oxidizing agentCr(s) is the reducing agent and Sn4+(aq) is the oxidizing agent2 of 10Indicate a balanced half-reaction for the reduction of NO3–(aq) to NO(g) in an acidicsolution.NO3–(aq) + 4 H+(aq) à NO(g) + 2 H2O( )NO3–(aq) + 4 H+(aq) à NO(g) + 2 H2O( ) + 2 e–NO3–(aq) + 4 H+(aq) + 3 e– à NO(g) + 2 H2O( )NO3–(aq) + 3 e– à NO(g) + O2(g)NO3–(aq) + 4 e– à NO(g) + O2(g)3 of 10Indicate a balanced chemical equation for the following reaction in an acidic solution:Cr2O72–(aq) + Ni(s) à Cr3+(aq) + Ni2+(aq)Cr2O72–(aq) + 3 Ni(s) + 14 H+(aq) à 2 Cr3+(aq) + 3 Ni2+(aq) + 7 H2O( )Cr2O72–(aq) + 3 Ni(s) + 7 H+(aq) à 2 Cr3+(aq) + 3 Ni2+(aq) + 7 OH–(aq)Cr2O72–(aq) + 3 Ni(s) à 2 Cr3+(aq) + 3 Ni2+(aq) + O2–(aq)Cr2O72–(aq) + Ni(s) + 14 H+(aq) à 2 Cr3+(aq) + Ni2+(aq) + 7 H2O( )Cr2O72–(aq) + Ni(s) + 14 H+(aq) à 2 Cr3+(aq) + Ni2+(aq) + 7 H2O( )4 of 10All of the following statements concerning voltaic cells are true EXCEPToxidation occurs at the anodeelectrons flow from the cathode to the anode in the external circuita salt bridge allows cations and anions to move between the half-cellsa voltaic cell can be used as a source of energya voltaic cell consists of two-half cells5 of 10Use the standard reduction potentials below to determine which element or ion is the bestreducing agent.NO3–(aq) + 4 H+(aq) + 3 e– à NO(g) + 2 H2O( )E° = +0.955 VPd2+(aq) + 2 e– à Pd(s)E° = +0.90 V2 H+(aq) + 2 e– à H2(g)E° = 0.00 VPd2+(aq)Pd(s)H+(aq)H2(g)NO3–(aq)6 of 10Consider the following standard reduction potentials in acid solution:Which is the weakest oxidizing agent in this list?Al3+(aq)Al(s)I-(aq)I2(s)Sn4+(aq)7 of 10What is a correct cell notation for a voltaic cell based on the reaction below?Cu2+(aq) + Pb(s) + SO42–(aq) à Cu(s) + PbSO4(s)Cu(s) | Cu2+(aq) || SO42–(aq) | PbSO4(s) | Pb(s)Cu(s) | Cu2+(aq), SO42–(aq) | PbSO4(s) | Pb(s)Cu(s) | Cu2+(aq), SO42–(aq) || PbSO4(s) || Pb(s)Pb(s) | PbSO4(s) || Cu2+(aq) || Cu(s)Pb(s) | PbSO4(s) | SO42–(aq) || Cu2+(aq) || Cu(s)8 of 10Calculate Eocell for the electrochemical cell below:Ag(s) | AgCl(s) | Cl–(aq) || Cu2+(aq) | Cu(s)given the following standard reduction potentials:Cu2+(aq) + 2 e– à Cu(s)E° = +0.337 VAgCl(s) + e– à Ag(s) + Cl–(aq)E° = +0.222 V–0.115 V–0.107 V+0.115 V+0.452 V+0.559 V9 of 10The reduction potentials for Au+3 and Ni+2 are as follows:Au+3 + 3e- à AuNi+2 + 2e- à NiEo = +1.50 VEo = -0.23 VCalculare ∆Go for the spontaneous reaction.-2140 kJ-5.00 x 102 kJ+5.00 x 102 kJ-1.00 x 103 kJ+1.00 x 103 kJ10 of 10In an electrolytic cell, 10.0 amps is passed through a magnesium chloride solution for 3.0hours. How many moles of Mg(s) are produced?0.370.570.741.12.2