Part ACalculate AS; for the reaction 3H₂(g) +N2(g) → 2NH3(g) at 715 K. Omit terms in thetemperature-dependent heat capacities greater than T²/K².Cp,m(H2, g) = 22.66 +0.0438-1.0835 × 10-4²J.K-¹.mol-¹Cp,m (N2, g) = 30.81 -0.01187+2.3968 × 10-5.<10-5²J.K-¹.mol-¹Cp,m (NH3, g) = 29.29 +0.01103+4.2446 × 10-5²J.K-¹.mol-¹H2(g) N2(g) NH3(g)S° (J. mol-¹.K-¹) 130.7 191.6 192.8Express your answer to four significant figures and include the appropriate units.AS; =HAValueSubmit Request AnswerUnits?T2

The reaction is given to us as This can also be written as

Calculate AS for the reaction 3H₂(g) +N2(g) → 2NH3(g) at 715 K. Omit terms in the temperature-dependent heat capacities greater than T²/K². Cp,m (H2, 8) = 22.66+0.0438-1.0835 × 10-4 J.K-¹.mol-¹ Cp,m (N2, g) = 30.81 -0.01187+2.3968 × 10-5J.K-¹.mol-¹ Cp,m (NH3, 8) = 29.29 +0.01103+4.2446 × 10-5 J.K-¹.mol-¹ H2(g) N2(g) NH3(g) S° (J. mol-¹.K-¹) 130.7 191.6 192.8

Calculate AS for the reaction 3H₂(g) +N2(g) → 2NH3(g) at 715 K. Omit terms in the temperature-dependent heat capacities greater than T²/K². Cp,m (H2, 8) = 22.66+0.0438-1.0835 × 10-4 J.K-¹.mol-¹ Cp,m (N2, g) = 30.81 -0.01187+2.3968 × 10-5J.K-¹.mol-¹ Cp,m (NH3, 8) = 29.29 +0.01103+4.2446 × 10-5 J.K-¹.mol-¹ H2(g) N2(g) NH3(g) S° (J. mol-¹.K-¹) 130.7 191.6 192.8

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter7: Chemical Energy

Section: Chapter Questions

Problem 62E: In a coffee-cup calorimeter, 1.60 g NH4NO3 is mixed with 75.0 g water at an initial temperature of...

See similar textbooks

Similar questions

When 1.000 g of ethylene glycol, C2H6O2, is burned at 25C and 1.00 atmosphere pressure, H2O(l) and CO2(g) are formed with the evolution of 19.18 kJ of heat. a Calculate the molar enthalpy of formation of ethylene glycol. (It will be necessary to use data from Appendix C.) b Gf of ethylene glycol is 322.5 kJ/mol. What is G for the combustion of 1 mol ethylene glycol? c What is S for the combustion of 1 mol ethylene glycol?
Benzoic acid, C6H5COOH, is a common standard used in bomb calorimeters, which maintain a constant volume. If 1.20 g of benzoic acid gives off 31, 723 J of energy when burned in the presence of excess oxygen and in a water bath having a temperature of 24.6 C, calculate q, w, H, and U for the reaction.
For the process A(l) A(g), which direction is favored by changes in energy probability? Positional probability? Explain your answers. If you wanted to favor the process as written, would you raise or lower the temperature of the system? Explain.
What are the two ways that a final chemical state of a system can be more probable than its initial state?
A 220-ft3 sample of gas at standard temperature and pressure is compressed into a cylinder, where it exerts pressure of 2000 psi. Calculate the work (in J) performed when this gas expands isothermally against an opposing pressure of 1.0 atm. (The amount of work that can be done is equivalent to the destructive force of about 1/4 lb of dynamite, giving you an idea of how potentially destructive compressed gas cylinders can be if improperly handled!)
The octane number of gasoline is based on a comparison of the gasolines behavior with that of 2,2,4-trimethylpentane, C8H18(), which is arbitrarily assigned an octane number of 100. The standard enthalpy of combustion of this compound is 5456.6 kJ/mol. (a) Write the thermochemical equation for the combustion of 2,2,4-trimethylpentane. (b) Use the standard enthalpies of formation in Appendix G to calculate the standard enthalpy of formation of 2,2,4-trimethylpentane.
Consider the reaction 2HCl(aq)+Ba(OH)2(aq)BaCl2(aq)+2H2O(l)H=118KJ Calculate the heat when 100.0 rnL of 0.500 M HCl is mixed with 300.0 mL of 0.100 M Ba(OH)2 Assuming that the temperature of both solutions was initially 25.0C and that the final mixture has a mass of 400.0 g and a specific heat capacity of 4.18 J/C g, calculate the final temperature of the mixture.
If the heat capacity varies withtemperature, abetter form ofequation 2.9 isto solve q=TiTfnCT-t A 50.0-g sample of white phosphorus is heated from 298 K to 350K. If its molar heat capacity is CT- = 56.990.1202T J/mol.K, how much heat is needed?