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:- your data has not provided the standard free energy of formation of NO(g) so I have used data from standard physical chemistry text book the data taken is 86.6 kj/mol

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Chemistry

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
Suppose the following exothermic reaction UO2(s)+4HF(g) UFA(g) + 2H20(g) has already reached equilibrium. Predict the effect that each of the following changes will have on the equilibrium position. State whether the equilibrium will shift to the reactants, will shift to the products, or will not be affected. Explain your answer using Le Chatelier's Principle. a. The system was cooled. b. The reaction vessel was quadrupled. C. Uranium (IV) oxide was added to the reaction. d. The partial pressure of Uranium (IV) fluoride was decreased.
The reaction is at equilibrium at some temperature, T, and the following equilibrium concentrations are measured: [SO2] = 0.90 M, [O2] = 0.35 M, and [SO3] = 1.1 M. Write the equilibrium expression for this reaction. Calculate Keq for the reaction at temperature, T.
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Define equilibrium constant Keq
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Please answer the following questions attached below. Follow the instructions for each given item and provide the complete solution to help me understand the topic. Thank you! P.S. Please do make sure the answers are correct for this items as I only have a few questions left.
A 6.00 mol sample of solid A was placed in a sealed 1.00 L container and allowed to decompose into gaseous B and C. The concentration of B steadily increased until it reached 1.40 M, where it remained constant. A(s)↽−−⇀B(g)+C(g) Then, the container volume was doubled and equilibrium was re‑established. How many moles of A remain? Dont
8.B A certain reaction has an equilibrium constant of K = 8.3×10$ at 25°C with a temperature-independent standard enthalpy of reaction of 34.2 kJ/mol. (a) What is the equilibrium constant at 37°C? (b) Use Le Chatelier's principle to defend your answer.
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
demonstrate an understanding of the concept of dynamic equilibrium and the variables that cause shifts in the equilibrium of chemical systems.