Please use the values in the resources listed below instead of the textbook values.Nitric oxide (NO) from car exhaust is a primary air pollutant. Calculate the equilibrium constant for the reactionN2(g) + O2(g)=2 NO(g)at 25°C using the data listed in the supporting materials.4.04.096e-31 XA 4e-31Calculate the equilibrium constant at 1496°C, which is a typical temperature inside the cylinders of a car's engine after it has been running for some time. (Assume that both ArH° and ArS° are temperature independent.)4.0 1.036 KNO2(s)KNO3(s)-369.8152.1-415.1N2(g)191.6-57.1-494.6133.1-394.9N2H4(g)95.4238.524.3KOH(s)N2H4(g)N,H¾(1)-424.878.9-379.195.40KO,(s)K2CO3(s)-284.9116.7-319.750.63149.4149.4-1150.2155.4-1196.5N2H4(1)50.6K202(s)N20(g)N203(g)N204(g)N204(1)-494.1102.1-524.581.56220.0103.6314.7Kr(g)Li(g)164.186.6-7.2159.3138.8117.99.7304.398.3Li(s)28.03-19.5209.297.5LiBr(s)-351.2-373.4Na(g)Na(s)74.3107.5153.777.0LİCI(s)LiF(s)-408.659.3-426.351.21-616.035.7-626.6NaBr(s)-361.0686.82-348.98NaCl(s)NaCIO3(s)Lil(s)-270.486.8-296.3-411.272.13-384.1LIOH(s)-487.250.21-443.9-365.8123.4-402.6Li,0(s)-597.937.6-609.1NaCIO4(s)-383.3142.3-425.7147.1102.8NaF(s)NaHCO3(s)Mg(g)148.6-576.651.1-546.3102.1Mg(s)MgBr2(s)32.68-947.7-851.9-524.3117.2-559.2Nal(s)NaNO2(s)-287.898.53-286.1MgCO3(s)-1095.865.7-1012.1-358.7103.8-389.6MgCl2(s)-641.389.62-591.8NaNO3(s)-467.9116.5-502.6Mg0(s)-601.826.78-569.6NaOH(s)-425.664.46-379.5Mn(g)280.7173.7228.9NaO2(s)-260.2115.9-294.8Mn(s)32.0-9.5Na,CO3(s)-1130.9135.98-1047.7Na20(s)Na202(s)MnCl2(s)-481.3118.2-516.5-414.275.1-436.6MnO(s)MnO2(s)-385.259.7-403.0-510.995.0-539.2-520.053.1-535.8Na,S(s)-364.883.7-389.8N(g)NH2CH2CO2H(s)Na,SO3(s)Na,SO4(s)470.7153.3455.5-1100.8145.9-1144.3-527.5103.5-558.4-1387.1149.6-1431.7NH3(g)-46.3192.5-16.6Ne(g)146.3TITStandard State Thermodynamic DataformulaAH º (kJ/mol)s° J/mol·K)AG° (kJ/mol)formulaAHº (kJ/mol)s° J/mol·K)AG° (kJ/mol)Ni(g)Ni(s)NiCl2(s)429.7182.2375.4SF.(g)-1209291.8-1105.3SO(g)SOCI2(g)SO2(g)29.9-8.96.3222.0-59.9-305.397.7-334.4-212.5309.8-304.9O(g)02(g)249.4161.0231.7-296.1248.5-300.1205.0SO2C12(g)-364.0311.9-457.0

When the rate of the forward and the backward reaction proceeds equally, then the reaction is said…

Please use the values in the resources listed below instead of the textbook values. Nitric oxide (NO) from car exhaust is a primary air pollutant. Calculate the equilibrium constant for the reaction N2(9) + O2(9)=2 NO(g) at 25°C using the data listed in the supporting materials. 04.096e-31 x 4e-31 Calculate the equilibrium constant at 1496°C, which is a typical temperature inside the cylinders of a car's engine after it has been running for some time. (Assume that both A,H° and A,S° are temperature independent.) D 1.036

Please use the values in the resources listed below instead of the textbook values. Nitric oxide (NO) from car exhaust is a primary air pollutant. Calculate the equilibrium constant for the reaction N2(9) + O2(9)=2 NO(g) at 25°C using the data listed in the supporting materials. 04.096e-31 x 4e-31 Calculate the equilibrium constant at 1496°C, which is a typical temperature inside the cylinders of a car's engine after it has been running for some time. (Assume that both A,H° and A,S° are temperature independent.) D 1.036

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter13: Chemical Equilibrium

Section: Chapter Questions

Problem 90AE: Methanol, a common laboratory solvent, poses a threat of blindness or death if consumed in...

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Lexan is a plastic used to make compact discs, eyeglass lenses, and bullet-proof glass. One of the compounds used to make Lexan is phosgene (COCl2), an extremely poisonous gas. Phosgene decomposes by the reaction COCl2(g)CO(g)+Cl2(g) for which Kp 6.8 109 at 100C. If pure phosgene at an initial pressure of 1.0 atm decomposes, calculate the equilibrium pressures of all species.
Consider the equation G = G + RT ln(Q). What is the value of G for a reaction at equilibrium? What does Q equal at equilibrium? At equilibrium, the previous equation reduces to G = RT ln(K). When G 0, what does it indicate about K? When G 0, what does it indicate about K? When t G = 0, what does it indicate about K? G predicts spontaneity for a reaction, whereas G predicts the equilibrium position. Explain what this statement means. Under what conditions can you use G to determine the spontaneity of a reaction?
Methanol, a common laboratory solvent, poses a threat of blindness or death if consumed in sufficient amounts. Once in the body, the substance is oxidized to produce formaldehyde (embalming fluid) and eventually formic acid. Both of these substances are also toxic in varying levels. The equilibrium between methanol and formaldehyde can be described as follows: CH3OH(aq)H2CO(aq)+H2(aq) Assuming the value of K for this reaction is 3.7 1010, what are the equilibrium concentrations of each species if you start with a 1.24 M solution of methanol? What will happen to the concentration of methanol as the formaldehyde is further converted to formic acid?
. Many sugars undergo a process called mutarotation, in which the sugar molecules interconvert between two isomeric forms, finally reaching an equilibrium between them. This is true for the simple sugar glucose, C6H12O6, which exists in solution in isomeric forms called alpha-glucose and beta-glucose. If a solution of glucose at a certain temperature is analyzed, and it is found that the concentration of alpha-glucose is twice the concentration of beta-glucose, what is the value of K for the inter-conversion reaction?
The reaction, 3 H2(g) + N2(g) (g), has the fol lowing equilibrium constants at the temperatures given: atT=25°C,K= 2.8 X 104 at T = 500°C, A = 2.4 X IO"7 At which temperature are reactants favored? At which temperature are products favored? YVhat can you say about the reaction if the equilibrium constant is 1.2 at 127°C?
Hydrogen and carbon dioxide react at a high temperature to give water and carbon monoxide. H2(g) + CO2(g) H2O(g) + CO(g) (a) Laboratory measurements at 986 C show that there are 0.11 mol each of CO and H2O vapor and 0.087 mol each of H2 and CO2 at equilibrium in a 50.0-L container. Calculate the equilibrium constant for the reaction at 986 C. (b) Suppose 0.010 mol each of H2 and CO2 are placed in a 200.0-L container. When equilibrium is achieved at 986 C, what amounts of CO(g) and H2O(g), in moles, would be present? [Use the value of Kc from part (a).]
12.101 An engineer working on a design to extract petroleum from a deep thermal reservoir wishes to capture toxic hydrogen sulfide gases present by reaction with aqueous iron(II) nitrate to form solid iron(II) sulfide. (a) Write the chemical equation for this process, assuming that it reaches equilibrium. (b) What is the equilibrium constant expression for this system? (c) How can the process be manipulated so that it does not reach equilibrium, allowing the continuous removal of hydrogen sulfide?
Sulfur oxychloride, SO2Cl2, decomposes to sulfur dioxide and chlorine gases. SO2Cl2(g)SO2(g)+Cl2(g) At a certain temperature, the equilibrium partial pressures of SO2, Cl2, and SO2Cl2 are 1.88 atm, 0.84 atm, and 0.27 atm, respectively. (a) What is K at that temperature? (b) Enough Cl2 condenses to reduce its partial pressure to 0.68 atm. What are the partial pressures of all gases when equilibrium is reestablished?
12.108 A nuclear engineer is considering the effect of discharging waste heat from a power plant into a lake and estimates that this may warm the water locally to 25 °C. One question to be considered is the effect of this temperature change on the uptake of CO2 by the water. The equilibrium constant for the reaction CO2+H2OH2CO3 ; is K=1.7103 at 25 °C. Because bonds form, the reaction is exothermic. (a) Will this reaction progress further toward products at higher temperatures near the water discharge with its warmer water than it would in the cooler lake water? Explain your reasoning. (b) Carbonic acid has a Kaof 2.5104 at 25 °C. What is the equilibrium constant for the CO2+2H2OHCO3+H3O+? (c) What additional factor should the engineer be considering about CO2 gas, probably before considering this reaction chemistry?