For the following reactions at constant pressure, choose the correct relationship between AH and AE. 2HF(g) → H2(g) + F2(g) ΔΗ>ΔΕ ΔΗ <ΔΕ ΔΗ-ΔΕ depends on the conditions N2(g) + 3H2(g) → 2NH3(g) ΔΗ > ΔΕ Ο ΔΗ< ΔΕ ΔΗ- = AE depends on the conditions 4NH3(g) + 502(g) → 4NO(g) + 6H,O(g) ΔΗ > ΔΕ ΔΗ<ΔΕ ΔΗ-ΔΕ depends on the conditions

For the following reactions at constant pressure, choose the correct relationship between AH and AE. 2HF(g) → H2(g) + F2(g) ΔΗ>ΔΕ ΔΗ <ΔΕ ΔΗ-ΔΕ depends on the conditions N2(g) + 3H2(g) → 2NH3(g) ΔΗ > ΔΕ Ο ΔΗ< ΔΕ ΔΗ- = AE depends on the conditions 4NH3(g) + 502(g) → 4NO(g) + 6H,O(g) ΔΗ > ΔΕ ΔΗ<ΔΕ ΔΗ-ΔΕ depends on the conditions

Introduction to General, Organic and Biochemistry

11th Edition

ISBN:9781285869759

Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres

Publisher:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres

Chapter7: Reaction Rates And Chemical Equilibrium

Section: Chapter Questions

Problem 7.17P: 7-17 If a certain reaction takes 16 h to go to completion at 10°C, what temperature should we run it...

See similar textbooks

Similar questions

Table 17-1 lists common half-reactions along with the standard reduction potential associated with each half-reaction. These standard reduction potentials are all relative to some standard. What is the standard (zero point)? lf is positive for a half-reaction, what does it mean? If is negative for a half-reaction, what does it mean? Which species in Table 17-1 is most easily reduced? Least easily reduced? The reverse of the half-reactions in Table 17-1 are the oxidation half-reactions. How are standard oxidation potentials determined? In Table 17-1, which species is the best reducing agent? The worst reducing agent? To determine the standard cell potential for a redox reaction, the standard reduction potential is added to the standard oxidation potential. What must be true about this sum if the cell is to be spontaneous (produce a galvanic cell)? Standard reduction and oxidation potentials are intensive. What does this mean? Summarize how line notation is used to describe galvanic cells.
7-17 If a certain reaction takes 16 h to go to completion at 10°C, what temperature should we run it if we want it to go to completion in 1 h?
What is a nonspontaneous reaction?
Which of the following quantities can be taken to be independent of temperature? independent of pressure? (a) H for a reaction (b) S for a reaction (c) G for a reaction (d) S for a substance
What characterizes an electrolytic cell? What is an ampere? When the current applied to an electrolytic cell is multiplied by the time in seconds, what quantity is determined? How is this quantity converted to moles of electrons required? How are moles of electrons required converted to moles of metal plated out? What does plating mean? How do you predict the cathode and the anode half-reactions in an electrolytic cell? Why is the electrolysis of molten salts much easier to predict in terms of what occurs at the anode and cathode than the electrolysis of aqueous dissolved salts? What is overvoltage?
The expression for ∆H° of formation of CO2 as a function of temperature is ∆Ho = -93480–0.603T–0.675x10-4T2-1.091x105/T. Find the ∆Cpo for this reaction as a function of T.
The value of delta G at 281.0oC for the formation of phosphorous trichloride from its constituent elements, P2 (g) + 3CI2 (g) ---> 2PCI3 (g) is _____ kJ/mol. At 25.0oC for this reaction delta H is -720.5kJ/mol, delta G is -642.9 kJ/mol, and delta S is -263.7 J/K.
The value of Delta G at 261.0oC for the formation of phosphorous trichloride from its constituent elements, P2 (g) +3Cl2 (g) -> 2PCI3 (g) is ___ kJ/mol. at 25.0oC for this reaction, delta H is -720.kJ/mol, Delta G is -642.9kJ/mol and delta s is -263.7 J/K
For the reaction 4HCl(g) +O2(g) == 2Cl2(g) + H2O (g), Keq =889 at 480 o If 0.03 mole HCl , 0,02 mole O2 , 0.08 mole Cl2 and 0.07 mole H2O were mixed in 1 liter container, in what direction will the reaction proceed. Support your answer.
Urea, CO(NH2)2 is slowly converted to ammonia (NH3) at 25.0 °C according to the following reaction. CO(NH2)2 (aq) + H2O (l) → CO2 (aq) + NH3 (aq) The following data were obtained for this reaction Compound ∆H°f (kJ/mol) CO(NH2)2 (aq) -319.2 H2O (l) -412.9 CO2 (aq) -285.8 NH3 (aq) -80.3 A) Calculate ∆H° for the reaction B) What type of reaction is this (endothermic, exothermic, neither) c)Calculate the change in enthalpy (∆H°) for the decomposition of 2.00 g of urea.
For the reaction 2 C6H5COOH(s) + 15 O2(g) → 14 CO2(g) + 6 H2O(g), ΔrU⦵ = −772.7 kJ mol−1 at 298 K. Calculate ΔrH⦵
Find ∆H as a function of T for the reaction: CO2 (g) + C (s, graphite) = CO Given that ∆H 293= 41,400 cal Cp CO2= 5.166+15.77×10^-3 T - 95.78×10^-3 T² + 2.260×10^-9 T³ Cp CO= 6.6 + 2×10^-3 T Cp C (s, graphite)= 2.673 + 2.617×10^-3 T - 1.169×10^-5 T^-2