Answered: Practice: will the reaction be…

Practice: will the reaction be spontaneous? If not write the spontaneous direction, and calculate the Ecell. Sketch the cell and write the line notation of the spontaneous reaction.

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

2. Calculate AGº and Kc for the following reaction at 298K: Br₂(1) + 21 (aq) (R:8.314J/mol.K, 96500 J/V.mol) 2Br (aq) + I₂(s)
A eq req E Consider the reaction: 2SO₂(g) + O2(g) → 2SO3(g) Using standard thermodynamic data at 298 K, calculate the free energy change when 1.57 moles of SO₂(g) react at standard conditions. AG = Substance AG (kJ/mol) SO3(g) SO₂(g) 0₂ (9) Submit Answer $ R % k] 5 Show Hint Use the References to access important values if needed for this question. T -371.1 -300.2 0.0 Retry Entire Group B Cengage Learning Cengage Technical Support ^ 6 9 more group attempts remaining H & 7 N J * 8 M 1 K ( 1 O P Previous Next> D ㅈ R 7 Save and Exit
Why is this incorrect and what is the right response?
Consider the reaction: 2C,H6(g) - 702(3)4CO2(g) + 6H,0(g) Using standard thermodynamic data at 298K, calculate the free energy change when 1.77 moles of C,H(g) react at standard conditions. AG kJ
13) Calculate the AGᵒrxn at 298 K using the following information. 2 H2S(g) + 3 O2(g) → 2 SO2(g) + 2 H₂O(g) - 33.4 -300.1 -228.6 AG°f (kJ/mol) A) -990.6 kJ B) +112.4 kJ C) +66.8 kJ 2A1 (s) + 312 (s) AG°r rxn ? D) -528.7 kJ 14) The standard cell potential for the cell using the overall cell reaction below is +2.20 V: 2A13+ (aq) + 61- (aq) The voltage generated by the cell when [A13+] = 4.5 × 10-3 M and [I-] = 0.15 Mis A) 2.32 B) 2.10 C) 2.39 D) 2.20 E) -495.3 kJ V. E) 2.23
Q17.24 A 3.5 mol sample of an ideal gas is compressed from 20.8 L to 12.5 L. What is its change in entropy (in J/K)? Give only the numerical part of your answer.
Consider the reaction: 2C₂H6(g) + 70₂(g) 4CO₂(g) + 6H₂O(g) Using standard thermodynamic data at 298K, calculate the free energy change when 2.42 moles of C₂H6(g) react at standard conditions. AG = rxn kJ
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.…
(Q74) A certain process is nonspontaneous at low temperatures. Given that AHX = 201.2 kJ and ASPxn = 876 J/K, at what temperature (in °C) will the process become spontaneous? %3D (Report your Celsius temperature to one decimal place --> if your answer has a decimal place of "O" and Canvas chops it off, don't worry about it).