Calculate temperature at which AG" changes sign. Calculate the temperature (in kelvins) at which the sign of AG° changes from positive to negative for the reaction below. This corresponds to the temperature at which K1. Assume that AH and AS are constant and do not change with temperature. 2HBr(g) + Cl(g)-2HCI(g) + Bry(g) AH= 81.1 kJ/mol and AS =-1.20 J/K mol T= K.

Calculate temperature at which AG" changes sign. Calculate the temperature (in kelvins) at which the sign of AG° changes from positive to negative for the reaction below. This corresponds to the temperature at which K1. Assume that AH and AS are constant and do not change with temperature. 2HBr(g) + Cl(g)-2HCI(g) + Bry(g) AH= 81.1 kJ/mol and AS =-1.20 J/K mol T= K.

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter16: Spontaneity Of Reaction

Section: Chapter Questions

Problem 83QAP

See similar textbooks

Similar questions

Suppose you have an endothermic reaction with H = + 15 kJ and a S of 150 J/K. Calculate G and Keq at 10, 100, and 1000 K.
Calculate K at 25°C for each of the reactions referred to in Question 32. Assume smallest whole-number coefficients.
Consider the reaction low at 25°C: 3SO42(aq)+12H+(aq)+2Cr(s)3SO2(g)+2Cr3+(aq)+6H2O Use Table 17.1 to answer the following questions. Support your answers with calculations. (a) Is the reaction spontaneous at standard conditions? (b) Is the reaction spontaneous at a pH of 3.00 with all other ionic species at 0.100 M and all gases at 1.00 atm? (c) Is the reaction spontaneous at a pH of 8.00 with all other ionic species at 0.100 M and all gases at 1.00 atm? (d) At what pH is the reaction at equilibrium with all other ionic species at 0.100 M and all gases at 1.00 atm?
Suppose you have an exothermic reaction with H = 15 kJ and a S of +150 J/K. Calculate G and Keq at 10, 100, and 1000 K.
Consider the reaction NH4+(aq) H+(aq)+NH3(aq) Use G f for NH3(aq) at 25C=26.7 kJ/mol and the appropriate tables to calculate (a) G at 25C (b) Ka at 25C
Consider the reaction below at 25°C: 2MnO4(aq)+16H+(aq)+10Br(aq)2Mn2+(aq)+5Br2(l)+8H2O Use Table 17.1 to answer the following questions. Support your answers with calculations. (a) Is the reaction spontaneous at standard conditions? (b) Is the reaction spontaneous at a pH of 2.00 with all other ionic species at 0.100 M? (c) Is the reaction spontaneous at a pH of 5.00 with all other ionic species at 0.100 M? (d) At what pH is the reaction at equilibrium with all other ionic species at 0.100 M?
Use Table 17.1 to find Kffor AuCl4- (aq) at 25°C.
The equilibrium constant for a reaction decreases as temperature increases. Explain how this observation is used to determine the sign of either H or S.
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.
10. For the reaction A(aq) + B(aq) <---> C(aq) + D(aq), the equilibrium constant is 20.3 at 25oC and 36.8 at 50oC. What is the value of the standard Gibbs free energy change (in kJ) of this reaction at 75oC?
For the reaction A(aq) ---> B(aq) the change in the standard free enthalpy is 3.39 kJ at 25 oC and 5.43 kJ at 45 oC. Calculate the value of this reaction's equilibrium constant at 75 oC. (I have already sent it once but the answer was 0.883 and its incorrect)
For the reaction A(aq) + B(aq) <---> C(aq) + D(aq), the equilibrium constant is 24.8 at 25oC and 37.5 at 50oC. What is the value of the change in the standard Gibbs free enthalpy (in kJ) of this reaction at 75oC?