The standard molar entropy of NO is 211 J K-1 mol-1. What is the standard entropy...

The standard molar entropy of NO is 211 J K-1 mol-1. What is the standard entropy of 3 moles of NO at 10 bar?

Solutions

Expert Solution

Comment in case of any doubt.

queen_honey_blossom answered 1 year ago

Next > < Previous

Related Solutions

The entropy of sublimation of a certain compound is 20.7 J K–1 mol–1 at its normal...

The entropy of sublimation of a certain compound is 20.7 J K–1 mol–1 at its normal sublimation point of 101 °C. Calculate the vapour pressure (in torr) of the compound at 9 °C. Assume that the enthalpy of sublimation is constant.

The standard molar entropies of water ice, liquid, and vapor are $37.99, 69.91$, and $188.83 \mathrm{~J} \mathrm{~K}^{-1} \mathrm{~mol}^{-1}$,

The standard molar entropies of water ice, liquid, and vapor are $37.99, 69.91$, and $188.83 \mathrm{~J} \mathrm{~K}^{-1} \mathrm{~mol}^{-1}$, respectively. On a single graph, show how the Gibbs energies of each of these phases vary with temperature.

The molar enthalpy of fusion of solid copper is 13.0 kJ mol-1, and the molar entropy...

The molar enthalpy of fusion of solid copper is 13.0 kJ mol-1, and the molar entropy of fusion is 9.58 J K-1 mol-1. (a) Calculate the Gibbs free energy change for the melting of 1.00 mol of copper at 1.39×103 K. kJ (b) Calculate the Gibbs free energy change for the conversion of 4.27 mol of solid copper to liquid copper at 1.39×103 K. kJ (c) Will copper melt spontaneously at 1.39×103 K? _____Yes No (d) At what temperature are...

At 100. oC, the constant-volume molar heat capacity of water vapor is 27.5 J mol-1 K-1;...

At 100. oC, the constant-volume molar heat capacity of water vapor is 27.5 J mol-1 K-1; this value rises to 33.1 J mol-1 K-1at 1000. oC. Based on these experimental values, what types (and how many) of degrees of freedom are contributing to the heat capacity of water vapor at each of these two temperatures? Clearly distinguish which degrees of freedom are fully or partially accessible. Do you expect the specific heat value to increase significantly as the T is...

Estimate Keq for the following equilibria at 350 K. R = 8.3145 J/(molK). Substance ΔHo(kJ/mol) So(J/(molK))...

Estimate Keq for the following equilibria at 350 K. R = 8.3145 J/(mol*K). Substance ΔHo(kJ/mol) So(J/(mol*K)) SnO2(s) -577.6 49.0 H2(g) 0 130.680 CO(g) -110.5 197.7 Sn(s, white) 0 51.2 H2O(l) -285.83 69.95 Fe(s) 0 27.3 Fe3O4(s) -1118.4 146.4 Correct answer. Correct. SnO2(s) + 2H2(g) ⇄ Sn(s, white) + 2H2O(l) The number of significant digits is set to 2; the tolerance is +/-3% LINK TO TEXT Incorrect answer. Incorrect. 3Fe(s) + 4H2O(l) ⇄ Fe3O4(s) + 4H2(g) Entry field with incorrect answer...

10. The initial and final entropy of a system are 42.9 J/moleK and 267.2 J/moleK, respectively....

10. The initial and final entropy of a system are 42.9 J/mole*K and 267.2 J/mole*K, respectively. At a temperature of 86.3oC, the enthalpy associated with this process was +68.6 KJ/mole. (a) Calculate the number of configurations that the system can assume finally. (b) Calculate the change of entropy for the system, in J/mole*K. Also, state whether the system became more or less disorderly. (c) Calculate the Gibb’s free energy for the process, in KJ/mole (d) State whether the process above...

For a hypothetical reaction, ΔrHθ = 89.1 kJ/mol and ΔrSθ = 364 J/mol/K. What is the...

For a hypothetical reaction, ΔrHθ = 89.1 kJ/mol and ΔrSθ = 364 J/mol/K. What is the total standard entropy of the reaction, ΔrStotθ, at 343 K?

The value of the universal gas constant is 0.082 (L atm)/(mol K) or 8.31 J/(mol k)...

The value of the universal gas constant is 0.082 (L atm)/(mol K) or 8.31 J/(mol k) and 1.00 atm = 760 mmHg or 760 torr. When a sample of H2O2 is decomposed, 350 mL of O2 gas is collected at 20 °C and at a partial pressure of 695 torr. How many moles of O2 gas were collect The value of the universal gas constant is 0.082 (L atm)/(mol K) or 8.31 J/(mol k) and 1.00 atm = 760 mmHg...

Cgas = 1.3 J/g×K Hvap = 38.56 kJ/mol Cliq = 2.3 J/g×K Hfus = 5.02 kJ/mol ...

Cgas = 1.3 J/g×K Hvap = 38.56 kJ/mol Cliq = 2.3 J/g×K Hfus = 5.02 kJ/mol Csolid = 0.97 J/g×K Condensation Temp = 78.0oC Freezing Pt = -114.0oC Calculate the amount of heat required toconvert 92.6 mL of ethanol, C2H6O, from 110.0oC to -98.0oC.

Please explain in detail "Biochemistry" Given: [R= 8.315 J/mol . K] Consider the reaction at standard...

Please explain in detail "Biochemistry" Given: [R= 8.315 J/mol . K] Consider the reaction at standard temperature: glucose-1-P -> glucose-6-P This reaction has a K' eq = 21 Answer the following questions: a. Is the concentration of glucose-6-P equal, higher or lower than that of glucose-1-P at equilibrium? Justify your answer using the expression for K' eq. b. What is ∆G'° for the reaction? Write down the equation used in the calculations and the units in your answer. c. If...

Subjects