7) Ethanol, is produced by fermentation of the glucose in fruit or grain. The reaction is: C,H1206 (aq) → 2C;H;OH (aq) + 2CO, (g). If AH = -70.8 kJ and AG° = -225.8 kJ at 25°C; a) Calculate entropy change, AS reaction; b) What does the sign of AS° tell us about the reaction? At 25°C, the equilibrium constant for a reaction is 35.0. The equilibrium constant value increases to 2.0 x 10 at 95°C. What is the enthalpy change (kJ/mol) for the reaction? Is it exothermic? 8)

7) Ethanol, is produced by fermentation of the glucose in fruit or grain. The reaction is: C,H1206 (aq) → 2C;H;OH (aq) + 2CO, (g). If AH = -70.8 kJ and AG° = -225.8 kJ at 25°C; a) Calculate entropy change, AS reaction; b) What does the sign of AS° tell us about the reaction? At 25°C, the equilibrium constant for a reaction is 35.0. The equilibrium constant value increases to 2.0 x 10 at 95°C. What is the enthalpy change (kJ/mol) for the reaction? Is it exothermic? 8)

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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If a reaction is exothermic and its entropy change is positive, which statement is true? (a) The reaction is spontaneous at all temperatures (b) The reaction is nonspontaneous at all temperatures (c) The reaction is spontaneous only at higher temperatures (d) The reaction is spontaneous only at lower temperatures
Use the data given here to calculate the values of AGn at 25 °C for the Compound AG; (kJ/mol) reaction described by the equation A +387.7 A + B 2C B - 596.8 C +402.0 543.1 AGixn kJ Incorrect If AHxn and ASxn are both negative values, what drives the spontaneous reaction and in what direction at standard conditions? The spontaneous reaction is enthalpy-driven to the left. entropy-driven to the right. entropy-driven to the left. O enthalpy-driven to the right. Incorrect O O O O
8) Calculate AG for a reaction at -12 ° C if AH is -34.6 kJ and AS is -114 J/K. Is the reaction spontaneous?
For a specific reaction, AH = -25.8 kJ/mol and AS = +45.6 J/K-mol. Which of these statements is true? O The reaction is never spontaneous. O The reaction is only spontaneous at high temperatures. OThe reaction is spontaneous at all temperatures. The reaction is only spontaneous at low temperatures.
Calculate AG for the following reaction at 25°C. Will the reaction occur (be spontaneous)? How do you know? NH(g) + HCI(g) ? NH4CI(s) Also given for this reaction AH =-176.0 kJ AS = -284.8 J-K'
The combustion of acetylene is used in welder's torches because it produces a very hot flame: C,H;(g) + 0;(g) →2CO;(g) + H,O(g) AH° = -1255.5 kJ (a) Use data in Appendix E to calculate AS for this reaction. (b) Calculate AG° and show that the reaction is sponta- neous at 25°C. (c) Is there any temperature range in which this reaction is not spontaneous? (d) Do you think you could use Equation 10.4 to calcu late such a temperature range reliably? Explain yok answer.
Consider the reaction described by the chemical equation shown. C,H,(g) + H,O(1) – C,H,OH(1) AH xn = -44.2 kJ Use the data from the table of thermodynamic properties to calculate the value of ASxn at 25.0 °C. ASixn J.K-! Calculate AGixn ·
18.45 Using enthalpies of formation (Appendix C), calculate AH° for the following reaction at 25°C. Also calculate AS° for this reaction from standard entropies at 25°C. Use these values to calculate AG° for the reaction at this temperature. 2CH3OH(I) + 302(g) 2CO2(g) + 4H,O(l) -
4NH3(g) + 3O2(g) → 2N2(g) + 6H2O(g) ΔrH = -1267 kJ mol-1 For the reaction above, select the correct sign for each of the following: ΔSsurr ΔSsys ΔSuniv Is the reaction spontaneous?
For a particular reaction, ΔH = -32 kJ and ΔS = -98 J/K.Assume that ΔH and ΔS do not vary with temperature.(a) At what temperature will the reaction have ΔG = 0?(b) If T is increased from that in part (a), will the reactionbe spontaneous or nonspontaneous?
For a particular reaction at 180.9 °C, AG = 527.78 kJ/mol, and AS = 953.96 J/(mol · K). Calculate AG for this reaction at -3.7 °C. AG = kJ/mol
AG° is -32.7 kJ/mol of N2 for the reaction at 100°C N2(g)+3H2(g)=2NH3(g) Calculate AG for the same reaction under the following nonstandard conditions: In which direction must the reaction proceed to reach equilibrium? [N2]= 2.00 M, [H2]= 7.00 M, [NH3] = 0.021 M, and T = 100°C. 2.