2) (3 pts) Classify each of the following reactions as one of the four possible type: i) spontaneous at all temperatures; ii) not spontaneous at any temperatures; iii) spontaneous at Low To, but not spontaneous at High T° and; iv) spontaneous at High T°, but not spontaneous at Low T°. A) NH4Cl (s) - t NH3 (g) + HCl (g) ; an endothermic reaction B) 2 C4H10 (g) + 13 O2 (g) → 8 CO2 (g) + 10 H2O (g) -> ; an exothermic reaction C) 2SO2 (g) + O2 (g) → 2SO3 (g) ; an exothermic reaction Page

2) (3 pts) Classify each of the following reactions as one of the four possible type: i) spontaneous at all temperatures; ii) not spontaneous at any temperatures; iii) spontaneous at Low To, but not spontaneous at High T° and; iv) spontaneous at High T°, but not spontaneous at Low T°. A) NH4Cl (s) - t NH3 (g) + HCl (g) ; an endothermic reaction B) 2 C4H10 (g) + 13 O2 (g) → 8 CO2 (g) + 10 H2O (g) -> ; an exothermic reaction C) 2SO2 (g) + O2 (g) → 2SO3 (g) ; an exothermic reaction Page

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...

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der the following reaction: 2NO2(g) N₂O4 (9) Part A Part B Calculate AG at 298 K if the partial pressures of NO₂ and N₂O4 are 0.36 atm and 1.64 atm, respectively. Express the free energy in kilojoules to two decimal places. |ΨΕΙ ΑΣΦ AG= -6288.99 Submit Previous Answers Request Answer ? Review I Consta kJ X Incorrect; Try Again; 4 attempts remaining This value of free energy is more negative than AG for the reaction (i.e., more spontaneous), but the partial pressure of ta about four times greater than that of the reactant, so the free-energy change is expected to be more positive than AG (i.e spontaneous). Given that AG = AG + RTln Q, calculate the value of Q (it should be greater than 1 for the specified conditions), and free energy from Part A to find the free-energy change at the given partial pressures. Make certain values are expressed in before summing them.
Consider the following reaction: E 2NO₂(g) N₂O4(9) -> Type here to search Q W S E Bi C R Part B F Calculate AG at 298 K if the partial pressures of NO₂ and N₂O4 are 0.38 atm and 1.63 atm, respectively. Express the free energy in kilojoules to two decimal places. AG= -6 Submit VΞΑΣΦ h a xa xô x + √x √xxx Provide Feedback Previous Answers Request Answer T P B 1X1 H X Incorrect; Try Again; 3 attempts remaining This value of free energy is more negative than AG for the reaction (i.e., more spontaneous), but the partial pressu times greater than that of the reactant, so the free-energy change is expected to be more positive than AG (Le., les N Given that AG-AG + RTIn Q, calculate the value of Q (it should be greater than 1 for the specified conditions) energy from Part A to find the free-energy change at the given partial pressures. Make certain values are expressed in summing them LOWE O ? M X.10n F20 kJ 4 90°F Clear
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Be sure to answer all parts. From the following combinations of AH and AS, predict if a process will be spontaneous at a high or low temperature: (a) both AH and AS are negative Process is spontaneous at high and low temperatures. Process is spontaneous at high temperatures and nonspontaneous at low temperatures. Process is nonspontaneous at high and low temperatures. Process is nonspontaneous at high temperatures and spontaneous at low temperatures. (b) AH is negative and AS is positive Process is spontaneous at high and low temperatures. Process is spontaneous at high temperatures and nonspontaneous at low temperatures. Process is nonspontaneous at high and low temperatures. Process is nonspontaneous at high temperatures and spontaneous at low temperatures. (c) both AH and AS are positive Process is spontaneous at high and low temperatures. Process is spontaneous at high temperatures and nonspontaneous at low temperatures. Process is nonspontaneous at high and low temperatures.…
I need help with this pratice problem: will the reaction be spontaneous? If not write thespontaneous direction, and calculate the Ecell. Sketch thecell and write the line notation of the spontaneous reaction. Zn + Ca2+ → Zn2+ + Ca