Consider the following reaction at 25 °C: 5 SO(g) + 2 NH»(g) → 2 NO(g) + 5 SO2(g) + 3 H₂O(g) If AG = -125 kJ/mol, AH = 42.4 kJ/mol and AS = 562.3 J/mol-K, is this reaction spontaneous as written under standard conditions? A) No, it is not spontaneous because enthalpy and entropy are positive. B) No, it is not spontaneous because the free energy is negative. C) Yes, it is spontaneous because the free energy is negative. D) Yes, it is spontaneous because the entropy

Consider the following reaction at 25 °C: 5 SO(g) + 2 NH»(g) → 2 NO(g) + 5 SO2(g) + 3 H₂O(g) If AG = -125 kJ/mol, AH = 42.4 kJ/mol and AS = 562.3 J/mol-K, is this reaction spontaneous as written under standard conditions? A) No, it is not spontaneous because enthalpy and entropy are positive. B) No, it is not spontaneous because the free energy is negative. C) Yes, it is spontaneous because the free energy is negative. D) Yes, it is spontaneous because the entropy

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

The element oxygen was prepared by Joseph Priestley in 1774 by heating mercury(II) oxide: HgO(s) → Hg() + 1/2O2(g), AH = 90.84 kJ/mol. Estimate the temperature at which this reaction will become spontaneous under standard state conditions. S'(Hg) = 76.02 J/K mol S(O2) = 205.0 J/K mol C S(HgO) = 70.29 J/K mol 11
Please report in correct sigfigs and in units of kJ/mol
Σ *00 For a particular reaction, AH = 81.95 kJ and AS = 27.0 J/K. Calculate AG for this reaction at 298 K. AG = %3D What can be said about the spontaneity of the reaction at 298 K? O The system is spontaneous in the reverse direction. O The system is at equilibrium. O The system is spontaneous as written. 8:12 PH (口四< 11/8/20 F5 F8 F12 PrtScr Insert Delete Backspace $4 % 8. 5. 7. 24 Alt Ctri
Gibbs free E 1
In the decomposition of H2O2(l) to H2O(l) and O2(g) the resulting ΔSuniv is 454.3 J/K; a spontaneous process. TRUE OR FALSE
) A chemical reaction that has a positive Δ G is correctly described as A) endergonic. B) endothermic. C) enthalpic. D) spontaneous. E) exothermic.
Calculate ΔHf for HCN(g) at 25°C, given the following related reaction at 25°C, 2 NH3(g) + 3 O2(g) + 2 CH4(g) ---> 2 HCN(g) + 6 H2O(g); ΔHrxn = -870.8 kJ and the heats of formation of some species are ΔHf = -80.3 kJ/mol for NH3(g), -74.6 kJ/mol for CH4, and -241.8 kJ/mol for H2O(g). Answers are in kJ/mol.
Combustion of C12H22O11(s) (sucrose or "table sugar") produces CO2(g) and H2O(l). When 3.96 g of sucrose is combusted in a constant volume (bomb) calorimeter, 65.3 kJ of heat is liberated. Calculate ΔE for the combustion of 2.75g of sucrose. Calculate ΔH for the combustion of 2.75 g of sucrose.
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 63.0 °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.
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
The standard state Gibb's energy and entropy changes are known for the reaction: 2H, S(g) + 30,(g)=2H20(g) + 2SO2(g) What is the standard state enthalpy change for the reaction at 25 C? 120 kJ 52 J AGº ASº Mole Mole K -68 kJ/mol 154 kJ/mol 104 kJ/mol O -119 kJ/mol
Consider the following reaction: Sr(OH)2(s) → Sr2+(aq) + 2 OH-(aq) ΔHorxn = -19.3 kJ/ mol Sorxn = -218.3 J/ K mol Which of the following statements is true? Group of answer choices: - the reaction is always non-spontaneous - The reaction is nonspontaneous at all temperatures - The reaction is spontaneous only at high temperature - The reaction is spontaneous only at low temperature - ΔG < 0 and the reaction is always spontaneous