For a particular reaction, AH = -328.21 kJ and AS = 98.7 J/K. Calculate AG for this reaction at 298 K. AG = kJ What can be said about the spontaneity of the reaction at 298 K? The system is at equilibrium. O The system is spontaneous in the reverse direction. The system is spontaneous as written. O O

For a particular reaction, AH = -328.21 kJ and AS = 98.7 J/K. Calculate AG for this reaction at 298 K. AG = kJ What can be said about the spontaneity of the reaction at 298 K? The system is at equilibrium. O The system is spontaneous in the reverse direction. The system is spontaneous as written. O O

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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For a particular reaction, AH = -46.7 kJ and AS =-123.8 J/K. Assuming these values change very little with temperature, at what temperature does the reaction change from nonspontaneous to spontaneous? K. Is the reaction in the forward direction spontaneous at temperatures greater than or less than the calculuted temperature? O greater than O less than
Determine the S'universe at 298 K for the reaction: 31.342 J/mol K 2NO(g) + 20z(g) → 2NO2(g) For the reaction, 4KCIO3(s) → 3KCIO«(s) + KCI(s) Calculate AGʻsys for the process at 298 K if AH'sys =144.3 kJ and AS'sys = -36.8 J/K. 133.33 kJ A key step in the production of sulphuric acid is the oxidation of SO2(g) + Oz(g) → 2SO3(g) At 98K, AGʻsys = - 500.51kJ; AH’sys = - 494.61. kJ; and AS'sys = -60.16 J/K a) Use the data to decide if this reaction is spontaneous at 25°, and predict how AG° will change with increasing T Reaction is spontaneous at lower temperature and vice versa b) Assuming AH´sys and AS'sys are constant with increasing T, is the reaction spontaneous at 900°C? Spontaneous
For each of the following reactions indicate whether as written it will be spontaneous at all temperature only at high enough temperatures only at low temperatures not at any temperatures or if the given information is insufficient to draw a conclu
Consider the reaction shown to answer the following question. 2CO (g) + 2H2 (g) → CO2 (g) + CH4 (g) AH° = - and AS° = - Which statement below is true? O This reaction is spontaneous at relatively higher temperatures and non-spontaneous at lower temperatures. O There is not enough information to make an assessment. O This reaction is spontaneous at relatively lower temperatures and non-spontaneous at higher temperatures. O This reaction is spontaneous at all temperatures. O This reaction is non-spontaneous at all temperatures.
Hint: No calculations are required. For the reaction 2HBr(g) + Cl2(g)- >2HCI(g) + Br2(g) AH° = -81.1 kJ and AS° =-1.20 J/K At standard conditions, this reaction would be product favored O at all temperatures. O at relatively high temperatures. O at no temperature. O at relatively low temperatures.
For a particular reaction at 128.0 °C, AG = 227.67 kJ, and AS = 644.41 J/K. Calculate AG for this reaction at -1.9 °C. AG =
estion 30 of 41 <. Consider an ideal gas enclosed in a 1.00 L container at an internal pressure of 10.0 atm. Calculate the work, w, if the gas expands against a constant external pressure of 1.00 atm to a final volume of 10.0 L. J w = Now calculate the work done if this process is carried out in two steps. 1. First, let the gas expand against a constant external pressure of 5.00 atm to a volume of 2.00 L. 2. From the end point of step 1, let the gas expand to 10.0 L against a constant external pressure of 1.00 atm. J w = とTOOLS x10 Question Source: McQuarrie, Rock, And Gallogly 4e - General Chemsitry| Publisher: University Science Books A étv Aa w MacBook Air DD
Which of the following can NOT be deduced from the value of ArGº for a reaction? Select one: the total energy that is absorbed or released by the system during reaction. the value of the equilibrium constant, K, for the reaction. the amount of work that can be obtained from or is required for a reaction or process under standard conditions. the direction (forwards or reverse) of the spontaneous overall reaction.
A chemical engineer is studying the two reactions shown in the table below. In each case, he fills a reaction vessel with some mixture of the reactants and products at a constant temperature of 74.0 °C and constant total pressure. Then, he measures the reaction enthalpy AH and reaction entropy AS of the first reaction, and the reaction enthalpy AH and reaction free energy AG of the second reaction. The results of his measurements are shown in the table. Complete the table. That is, calculate AG for the first reaction and AS for the second. (Round your answer to zero decimal places.) Then, decide whether, under the conditions the engineer has set up, the reaction is spontaneous, the reverse reaction is spontaneous, or neither forward nor reverse reaction is spontaneous because the system is at equilibrium. AH = 181. kJ AS = -499. K ? 2NO(g) N, (g) + 0, (g) AG = kJ Which is spontaneous? this reaction the reverse reaction neither
For a particular reaction, AH = -238.4 kJ and AS = -80.0 J/K. Calculate AG for this reaction at 298 K. AG = kJ What can be said about the spontaneity of the reaction at 298 K? The system is spontaneous in the reverse direction. The system is at equilibrium. The system is spontaneous as written.
Consider the reaction that happens at -13 °C: 1A + 2B 8C + 6D. Using the data from the table: B C D AH; (kJ mol 1) 309 144.4 149.5 s° (U mol 1 K1) 61.4 33.6 76.4 153.4 calculate AG° (in kJ) of the reaction. (assume that values of AH and S do not change with the temperature) Enter a number with sign (+ or -) to 1 decimal place in kJ.