Part C(c) to N₂ (g), O₂ (g), and H₂O(g)Express your answer in kilojoules per mole to one decimal place.AGIxn=[Π ΑΣΦ?kJ/mol The salt ammonium nitrate can follow three modesof decomposition: (a) to HNO; (g) and NH3(g),(b) to N₂O(g) and H₂O(g), and (c) to N₂ (g),O2 (g) and H₂O(g). Calculate AGixn for eachmode of decomposition at 298 K.Compound AGNH3(g)-16.4NH4NO3(s) -183.9HNO3(g)-73.5N₂O(g)103.7H₂O(g)-228.6(kJ/mol)(b) to N₂O(g) and H₂O(g)Express your answer kilojoules per mole to one decimal place.AGIX =SubmitPart CAGix=IT ΑΣΦ ASubmitRequest Answer(c) to N₂ (g), O₂(g), and H₂O(g)Express your answer in kilojoules per mole to one decimal place.| ΑΣΦ A?Request AnswerkJ/mol?kJ/mol

The information given: The salt ammonium nitrate decomposes to form different products, The change…

The salt ammonium nitrate can follow three modes of decomposition: (a) to HNO3 (g) and NH3(g). (b) to N₂O(g) and H₂O(g), and (c) to N₂ (g). O₂ (g) and H₂O(g). Calculate AGixn for each mode of decomposition at 298 K. Compound AG (kJ/mol) NH3(g) -16.4 NH, NO3(s) -183.9 HNO3(g) -73.5 N₂O(g) 103.7 H₂O(g) -228.6 (b) to N₂O(g) and H₂O(g) Express your answer in kilojoules per mole to one decimal place. AGIX = Submit Part C AGI 195, ΑΣΦ Submit Request Answer (c) to N₂(g), O₂(g), and H₂O(g) Express your answer in kilojoules per mole to one decimal place. 15. ΑΣΦ ? Request Answer kJ/mol ? kJ/mol

The salt ammonium nitrate can follow three modes of decomposition: (a) to HNO3 (g) and NH3(g). (b) to N₂O(g) and H₂O(g), and (c) to N₂ (g). O₂ (g) and H₂O(g). Calculate AGixn for each mode of decomposition at 298 K. Compound AG (kJ/mol) NH3(g) -16.4 NH, NO3(s) -183.9 HNO3(g) -73.5 N₂O(g) 103.7 H₂O(g) -228.6 (b) to N₂O(g) and H₂O(g) Express your answer in kilojoules per mole to one decimal place. AGIX = Submit Part C AGI 195, ΑΣΦ Submit Request Answer (c) to N₂(g), O₂(g), and H₂O(g) Express your answer in kilojoules per mole to one decimal place. 15. ΑΣΦ ? Request Answer kJ/mol ? kJ/mol

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...

See similar textbooks

Similar questions

53. Please show the process of cancelling out the function of ln. thank you
Chemistry
Consider the following reaction: SO((g) + CaO(s) = CasO4(s). If AGº is -345 kJ/mol for this reaction at 298K, what is the Keg at this temperature? Recall that R is 8.314 J mol-1 K-1. A) 3.1 x 1040 B) 3.50 x 1050 c) 2.96 x 1060 D 2.23 x 1070
The synthesis of the pesticide thionyl chloride (OSCI2) proceeds according to the following reaction: SO3(g) + SCI2(e) = OSCl2(e) + SO2(g) If AG° is -106 kJ/mol for this reaction at 298K, what is the Keg at this temperature? Recall that R is 8.314 J mol-1 K-1. A) 7.21 x 1012 B 3.50 x 1014 c) 3.81 x 1018 D) 1.19 x 1020
Calculate AG at 298 K for the following reaction: L(g) + Ch(g) – 2ICI(g), K=81.9 Express your answer in kilojoules to three significant figures. AIO ? kJ AG'm %3D
Consider the following reaction: 2NO2(g) S N204(g) The values of AH° and ASº are -58.03 kJ/mol and -176.6 J/K•mol, respectively. Assuming AH° and AS° are temperature independent, estimate the value of K at 363.2 K. K =
Using H° data, calculate the standard enthalpy change for the reaction at 298K. 2 NH3(g) HNO3(aq) --> NO2(g) 2 H20(1) AH° (KJ/mol) -46.19 -206.6 33.84 -285.83 (Note: the table AH values are located directly below the corresponding compound, this is the number found in the Appendix)
AG° is -32.7 kJ/mol of N2 for the reaction at 100°C N2(g)+3H2(g)=2NH3(g) Calculate AG for the same reaction under the following nonstandard conditions: In which direction must the reaction proceed to reach equilibrium? [N2]= 2.00 M, [H2]= 7.00 M, [NH3] = 0.021 M, and T = 100°C. 2.
Given the dissociation of methane to graphite (C) and hydrogen gas. For the methane at 298K, Given the following data: kJ = -74.85- mol = -80.67 mol · K A,GE.graphite = A,Gån = 0 %3D Solve the following: a. Calculate the equilibrium constant (K) of the dissociation of methane at 298K with the appropriate units. b. Assuming that enthalpy is independent of temperature, Calculate the equilibrium constant (K) of methane dissociation at 1000 K. C. Calculate the ratio between the amounts of methane and hydrogen gas at 298 K and 0.2 bar.
Consider the reaction that happens at -13 °C: 1A + 2B 8C + 6D. Using the data from the table: B C D AH; (kJ mol 1) 309 144.4 149.5 s° (U mol 1 K1) 61.4 33.6 76.4 153.4 calculate AG° (in kJ) of the reaction. (assume that values of AH and S do not change with the temperature) Enter a number with sign (+ or -) to 1 decimal place in kJ.
Consider the system below at equilibrium at 200°C: 2C12 (g) + 2H20 (g) - 98.6KJ = 4HCI (g) + 02 (g) The change listed below would cause more reactants to form when equilibrium is re- established. Write A if true and B if false (Note: Answer is case sensitive) Decreasing the volume at constant temperature
25. H2(g) + I2(g) 2HI(gx Kp = 55.2 AH°rxn = +53 kJ Write the formulas for Kp and Qp of this equation: Kp = Qp = A mixture with 0.22 atm H2(g), 0.05 atm I2(g), and 3.5 atm HI(g) has Qp = and will shift to: (show direction) to reach equilibrium. If the mixture at equilibrium is heated, it will shift to: to reach new equilibrium.