Question 7. For the Haber process described by the following reaction.2 NH3(g)N2(g) + 3 H2(g)The equilibrium constants as function of temperature are:Temperature (°C) Ke95227300327427527Determine the temperature at which the reaction become spontaneousa. 754 °Cb. 641 °Cc. 368 °Cd. 638 °Ce. 836 °C1240.10.05

Haber Process is under, N2(g) + 3H2(g) ⇔ 2NH3(g) Determine the temperature at which the reaction…

Answered: Determine the temperature at which the…

Science

Chemistry

Determine the temperature at which the reaction become spontaneous a. 754 °C b. 641 °C C. 368 °C. d. 638 °C e. 836 °C

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

Which process is spontaneous at 298 K?a. H2O(l )--->H2O(g, 1 atm)b. H2O(l )--->H2O(g, 0.10 atm)c. H2O(l )--->H2O(g, 0.010 atm)
Which of the following variables tells us about the extent of a reaction in thermodynamics? a. kforward b. Keq c. RT d. Ea
Which substance has the higher entropy? a. a sample of pure silicon (to be used in a computer chip) or a piece of silicon containing a trace of another element such as boron or phosphorus a piece of silicon containing a trace of another element such as boron or phosphorus a sample of pure silicon b. CO2(g) at 0 °C or CO2 (g) at -50 °C O CO2 (g) at –50 °C O CO2 (g) at 0 °C c. I2 (s) or I2 (g) both at room temperature OL (g) OL (s) d. one mole of CO2(g) at 1 bar pressure or one mole of CO2(g) at 0.01 bar pressure (both at 298 K) one mole of CO2(g) at 0.01 bar pressure one mole of CO2(g) at 1 bar pressure
For: 2 NO (g) + Cl2 (g) → 2 NOCl (g) the ΔHo is −37.78 kJ and ΔSo is −117.03 J/K. As the temperature increases: A. ΔGo increases B. ΔGo decreases C. the reaction becomes more spontaneous D. ΔGo becomes more negative E. nothing happens
Given the following enthalpy and entropy values, determine which reactions would not violate the 2nd law of thermodynamics at 298K. A. Enthalpy = -84 KJ/mole Entropy = 125 J/mol B. Enthalpy = -84 KJ/mol Entropy = -125 J/mol C. Enthalpy = 84 KJ/mol Entropy = 125 J/mol D. Enthalpy = 84 Kj/mol Entropy = -125 J/mol
For a given reaction, ΔH = +35.5 kJ/mol and ΔS = +83.6 J/mol·K. Which of the following is TRUE? a. The reaction is spontaneous at standard conditions. b. The reaction is spontaneous at T > 425 K. c. The reaction is spontaneous at all temperatures. d. The reaction is spontaneous at T < 425 K.
Now calculate the change in entropy (delta S) for the following reaction, using the thermodynamic tables P4 (g) + 10 Cl2 (g) → 4 PCl5 (g) a. 1412 J/K b. – 1.50 x 10^2 J/K c. – 856 J/K d. 2510 J/K e. – 113 J/K f. – 1098 J/K g. 3922 J/K h. 856 J/K i. none of these
Would conditions of +ΔH and -ΔS favor a spontaneous or non-spontaneous reaction? Why? a. Non-spontaneous because energy is absorbed and contained. b. Spontaneous only at low temperatures because energy is released but it is also somewhat concentrated. c. Spontaneous definitely because energy is released and dispersed. d. Spontaneous only at high temperatures because energy is absorbed but it is also dispersed.
Would conditions of +ΔH and -ΔS favor a spontaneous or non-spontaneous reaction? Why? Select one: a.Non-spontaneous because energy is absorbed and contained. b.Spontaneous only at low temperatures because energy is released but it is also somewhat concentrated. c.Spontaneous definitely because energy is released and dispersed. d.Spontaneous only at high temperatures because energy is absorbed but it is also dispersed.
4. Select all that is considered spontaneous a. Cleaning your room b. A piece of bread molding after being left out in the sun c. A bomb exploding d. Pushing a ball up a ramp e. Ice melting f. Frying an egg g. Putting together a puzzle