The standard molar entropy of NH3 is 192.45 J K1 mol at 298K, and its heat capacity is given by the equation Coma +bT +c/T2 with the coefficients given in the table below. Calculate the standard molar entropy of NH3 at 100 °C p,m Please explain as much as possible. Why did you use the equation? Or what conditions did you see from the question? etc. Table 1: Temperature variation of molar heat capacities, Cp,m/U K-1mol-1) a + bT + c/T2 b/(10-3 K-) 25.1 c/(10 K2) a NH3 29.75 -155

The standard molar entropy of NH3 is 192.45 J K1 mol at 298K, and its heat capacity is given by the equation Coma +bT +c/T2 with the coefficients given in the table below. Calculate the standard molar entropy of NH3 at 100 °C p,m Please explain as much as possible. Why did you use the equation? Or what conditions did you see from the question? etc. Table 1: Temperature variation of molar heat capacities, Cp,m/U K-1mol-1) a + bT + c/T2 b/(10-3 K-) 25.1 c/(10 K2) a NH3 29.75 -155

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

For the reaction 2BrF3 (g) → Br₂(g) + 3F₂ (g) AGO 471 kJ and AH° 542 kJ at 264 K and 1 atm. This reaction is reactant favored under standard conditions at 264 K. The entropy change for the reaction of 2.39 moles of BrF3 (g) at this temperature would be = J/K.
An organic compound CXH,O is a liquid at room temperature. The normal freezing point of this compound is -30 °C, and its molar enthalpy of fusion is AH = 4.73 kJ/mol. What is the entropy change in unit of J/K when 0.29 mole of liquid CyHyO freezes at the normal freezing point? fus Please keep your answer to one decimal place.
Calculate the standard molar entropy of vaporization of water at 40.0 °C, given that its standard molar entropy of vaporization at 100.0 °C is 109.0 J-K-¹ mol and the molar heat capacities at constant pressure for liquid water and water vapor are 75.3 J-K-¹-mol-¹ and 33.6 J-K-¹-mol-¹, respectively, in this temperature range. A.Svap 145.96 Incorrect J.K-¹.mol-¹
Solve the following and provide the complete solution: Calculate the change in entropy experienced by 2 moles of an ideal gas onbeing heated from a pressure of 5 atm at 50 °C to a pressure of 10 atm at100 °C. For the gas CP = 9.88 cal mole–1degree–1
Consider the reaction 4-entro 4HС(g) + O2(g)- →2H2O(g) + 2Cl2(g) Using standard thermodynamic data at 298K, calculate the entropy change for the surroundings when 1.50 moles of HCl(g) react at standard conditions. AS surroundings J/K
A chem V ngineer is studying the two reactions shown in the table below. In each case, he fills a reaction vessel with some mixture of the reactants and products at a constant temperature of 90.0 °C and constant total pressure. Then. he measures the reaction enthalpy AH and reaction entropy AS of the first reaction, and the reaction enthalpy AH and reaction free energy AG of the second reaction. The results of his measurements are shown in the table. Complete the table. That is, calculate AG for the first reaction and AS for the second. (Round your answer to zero decimal places.) Then, decide whether, under the conditions the engineer has set up, the reaction is spontaneous, the reverse reaction is spontaneous, or neither forward nor reverse reaction is spontaneous because the system is at equilibrium. AH = 2220, kJ J AS = 6113. K AG = kJ 3co,() + 4H,0(1) → C,H,(g) + 50,(g) Which is spontaneous? O this reaction O the reverse reaction O neither AH = -951. kJ J AS = AG = – 14. kJ 2A1(s)…
4) The heat capacity of CO2(g) between 30 C and 100 C is given by the following equation Cp = 26.65+ 42.3x10-3 T/K-142.4X10 -7 T 2/K 2 in J K -1 mol -1 . a )Calculate the enthalpy change and b) the entropy change between 30C and 100 C.
Consider the reaction: 6CO2(g) + 6H₂O(l) → C6H12O6 + 602 (9) Using standard thermodynamic data at 298 K, calculate the entropy change for the surroundings when 1.87 moles of CO₂ (g) react at standard conditions. AS⁰ Substance AH (kJ/mol) CO₂ (g) -393.5 H₂O(1) -285.8 C6H12O6 -1275.0 O₂(g) 0.0 surroundings J/K
D. 12.5% 46. What is the binding energy (in J per nucleus) for the nuclide 1.43 x 10¹3 J/nucleus 1.43 x 10-12 J/nucleus A. B. 19 F 9 C. 2.38 x 10-11 J/nucleus D. 7.53 x 10¹¹ J/nucleus ini below the band of stability can increase their neutron-to
A chem.. ngineer is studying the two reactions shown in the table below. In each case, he fills a reaction vessel with some mixture of the reactants and products at a constant temperature of 52.0 °C and constant total pressure. Then, he measures the reaction enthalpy AH and reaction entropy AS of the first reaction, and the reaction enthalpy AH and reaction free energy AG of the second reaction. The results of his measurements are shown in the table. Complete the table. That is, calculate AG for the first reaction and AS for the second. (Round your answer to zero decimal places.) Then, decide whether, under the conditions the engineer has set up, the reaction is spontaneous, the reverse reaction is spontaneous, or neither forward nor reverse reaction is spontaneous because the system is at equilibrium. AH = 181. kJ J AS = 557. K N, (g) + 0, (g) → 2NO (g) AG = N, (g) + 0,(8) kJ Which is spontaneous? this reaction the reverse reaction neither ΔΗ - - 1353. kJ J AS = K 2CH,OH (g) + 30,(g)…
Consider the reaction HCI(g) + NH3(g)- →NH4Cl(s) Using standard thermodynamic data at 298K, calculate the entropy change for the surroundings when 2.34 moles of HCI(g) react at standard conditions. ASO surroundings = J/K
A chemical engineer is studying the two reactions shown in the table below.. In each case, he fills a reaction vessel with some mixture of the reactants and products at a constant temperature of 124.0 °C and constant total pressure. Then, he measures the reaction enthalpy AH and reaction entropy AS of the first reaction, and the reaction enthalpy AH and reaction free energy AG of the second reaction. The results of his measurements are shown in the table. Complete the table. That is, calculate AG for the first reaction and AS for the second. (Round your answer to zero decimal places.) Then, decide whether, under the conditions the engineer has set up, the reaction is spontaneous, the reverse reaction is spontaneous, or neither forward nor reverse reaction is spontaneous because the system is at equilibrium. CC14 (8)→ C(s) + 2Cl₂ (g) TICI (g) + 2H₂O(g) → TiO₂ (s) + 4HCl(g) ΔΗ = 107. kJ AS = 310. AG= kJ Which is spontaneous? O this reaction. O the reverse reaction Oneither ΔΗ = -70. KJ…