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 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

Equilibrium Constant at 25oC is 4.36×10-31 Equilibrium Constant at 1496 oC is 7.68×10-6 Note:-…

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. ) 4.096e-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.) 40 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. ) 4.096e-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.) 40 1.036

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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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(g) + O2(g)=2 NO(g) at 25°C using the data listed in the supporting materials. 4.04.096e-31 X A 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 ArH° and ArS° are temperature independent.) 4.0 1.036
SO₂ reacts with Cl₂ to form SO₂Cl₂. The equilibrium constant, Kp, for this reaction is 0.417 at 373 K. 4 SO₂(g) + Cl₂(g) =SO₂Cl₂(g) The standard enthalpy change for this reaction (AH°) is -67.2 kJ/mol. (a) Predict the effect on the production of SO₂Cl₂ when the temperature of the equilibrium system is increased. (b) Use the van't Hoff equation to estimate the equilibrium constant for this reaction at 449 K. Kat 449 K =
At -9.76 °C the concentration equilibrium constant K = 5.3 × 105 for a certain reaction. Here are some facts about the reaction: • If the reaction is run at constant pressure, the volume increases by 11.%. • If the reaction is run at constant pressure, 64.0 kJ/mol of heat are released. • The net change in moles of gases is - 1. Using these facts, can you calculate K at 15. °C? If you said yes, then enter your answer at right. Round it to 2 significant digits. If you said no, can you at least decide whether K at 15. °C will be bigger or smaller than K at -9.76 °C? O Yes. O No. 0 Yes, and K will be bigger. Yes, and K will be smaller. O No. 0 x10 X
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Given the following equilibrium constants at 700K, 2 N2O(g) (double arrow) 2 N2 (g) + O2(g) K1 = 8.2 x 1033NO2(g) (double arrow) 1⁄2 N2(g) + O2(g) K2 = 2.44 x 108N2O4(g) (double arrow) 2 NO2(g) K3 = 4.6 x 10-3 determine the values of the equilibrium constants for the following reaction. Show your equation-buildingprocess and your calculations. 2 N2O4(g) (double arrow) 2 N2O(g) + 3 O2(g) K =
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Ammonia will decompose into nitrogen and hydrogen at high temperature. An industrial chemist studying this reaction fills a 2.0 L flask with 3.7 atm of ammonia gas, and when the mixture has come to equilibrium measures the amount of nitrogen gas to be 0.74 atm. Calculate the pressure equilibrium constant for the decomposition of ammonia at the final temperature of the mixture. Round your answer to 2 significant digits. K = 0 P X S
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