2C2H2(g) + 502ig) →4CO2(g) + 2H2O» Using the following data at 298K to answer the questions: Substance ΔΗ kJ/mol AS J/K•mol C2H2g) 227 201 O2ig) 205 -393.5 214 H2O) -286 70 What is the enthalpy change for the reaction? [ Select ] What is the entropy change for the reation? [Select] What is the Gibb's Free energy for the reaction? [ Select] Is the reaction spontaneous? [ Select] > >

2C2H2(g) + 502ig) →4CO2(g) + 2H2O» Using the following data at 298K to answer the questions: Substance ΔΗ kJ/mol AS J/K•mol C2H2g) 227 201 O2ig) 205 -393.5 214 H2O) -286 70 What is the enthalpy change for the reaction? [ Select ] What is the entropy change for the reation? [Select] What is the Gibb's Free energy for the reaction? [ Select] Is the reaction spontaneous? [ Select] > >

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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The value of AHT for the following reaction is 169.5 kJ. The value of AH for CaO(s) s kmd. CaCO3 (s)- Cao (s) * CO2 ) Standard Enthalpies of Formation of Some Inorganic Substances at 25'C TABLE 6.4 Subatance A mol) Substance A /mo) -1876 Ag(s) AgC) AKS) 127.0 ALO) "1669.8 Mg(s) MgO) Br() HBrg Cigraphite) Cidiamond) -36.2 -S01.S -11129 1.90 NH4 NO) -110.5 463 904 33.35 Cas) 35.6 NO) CCO(s) 966 Og) HCKg Car) 92.3 Sirhombic Scenonocinic) so-co so Fig) -716 Hg) Hg) 20.15 2418
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4. The standard enthalpies of combustion reaction at 25 °C of H2i9) , n-butane, C«H10(9) , 1- butene, C4H8(g) , and 1,3 -butadiene, C4H6(g) are -285.84 kJ/mol, -2878.6 kJ/mol, - 2718.8 kJ/mol and -2543.5 kJ/mol, respectively. Calculate AH° for the following reactions. a) C4H8(q) + H2(g). CẠH10(9) b) C4H6(a) + 2 H2(a) C4H10(a) c) CO(g)+H20(g)→CO2(g)+H2(g)
4. Use Hess's Law and the following data; CHale) + 202) CO2le) + 2H,0(g) AH = - 802 KJ + CO2(e) 2C0 + 2H2g) AH = + 247 KJ CH416) + H,0e) + 3H2(e) AH = + 206 KJ + To determine AH for reaction: CH4le) + % Ozle) » COe) + 2H2e)
& Moving to another question will save this response. Question 13 Calculate the work w, gained or lost by the system when a gas shrinks from 23.4 L to 119 Lagainst a constant external pressure of 1.3 atm. (1 Latm-1013 (1.5kJ 280 kJ 360 kJ 0.15 kJ -13k
# Consider the reaction 20 E D 2NH3(g) + 3N₂O(g) → 4N2(g) + 3H₂O(g) for which AH = -879.5 kJ and AS = 288.1 J/K at 298.15 K. 1. Calculate the entropy change of the UNIVERSE when 1.642 moles of NH3 (9) react under standard conditions at 298.15 K. $ Submit Answer 4 ASuniverse J/K 2. Is this reaction reactant or product favored under standard conditions? 3. If the reaction is product favored, is it enthalpy favored, entropy favored, or favored by both enthalpy and entropy? If the reaction is reactant favored, choose 'reactant favored'. 000 000 R F do L % [Review Topics] [References] Use the References to access important values if needed for this question. 5 O Retry Entire Group T Cengage Learning Cengage Technical Support G ‹ 6 8 more group attempts remaining Y H & 7 U 8 J 1 ( 9 K O O L P > Previous Email Instructor Save and Exit + 11 ( Next ? 11 } ] d
Mark the correct statements. (Select all that apply.) O [The reaction 2H20(g) → 2H2(g) + O2(g) is expected to have a positive value of ASº.] O [If a sample of pure ozone changed to oxygen at constant T and P, the entropy of the sample would decrease.] O [For the process H20(1) → H20(s) occurring at 0°C and 1 atm, the sign of AS is negative.] O [The value of AS for the process CHC13(1) – CHC13(g) is negative.] O [The reaction CH4(g) + 202(g) → CO2(g) + 2H2O(g) has a negative value of ASsurr-]
Calculate AGran in kJ, at 298K for the following reaction using the conditions given below. R = 8.314 J/mol.K SO3 (g) + H₂O (9) H₂SO4 (1) AGran = -90.5 (A) mol Pso3 = 0.20 atm, Pu,o = 0.88 atm Express your answer to one decimal place.
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
lp acellus_engine.html?ClassID=1246112631# Student Orie. Using the data below, calculate the enthalpy for the decomposition of sodium bicarbonate. 2NaHCO3(s) → Na,CO3(s) + H2O(g) + CO2(g) Compounds S (J/mol-K) AHF° (kJ/mol) NaHCO,(s) Na,CO,(s) CO,(g) H,O(g) 102 -948 136 -1131 214 -394 189 -242 AHxn = [ ? ] kJ %3D Enter either a + or - sign AND the magnitude. Enthalpy (kJ) Enter
O-234 kJ 234 kJ -150. kJ -117 kJ Given: -1835kJ AH°, AHᵒf (kJ/mol) -941 -840 QUESTION 12 Use the standard reaction enthalpies given below to determine AH°rxn for the following reaction: P4(g) + 10 Cl₂(g) → 4 PC|5(s) PC15(s) → PC13(g) + Cl₂(g) P4(g) + 6 Cl₂(g) → 4 PCl3(g) rxn IF7(g) IF 5(9) 2(g) 62.42 = ? ΔΗ° rxn AH°rxn = +157 kJ = -1207 KJ QUESTION 13 Use the AH°f and AH°rxn information provided to calculate AH°f for IF: IF7(9) + 12(g) → IF5(g) + 2 IF(g) AH°rxn = -89 kJ
Estimate the entropy change for the reaction: 2NO2 (g) + N204 (g) Standard entropy and enthalpy of formation S (U/mol K) Species H>(8) H(g) O:(8) O(g) N:(g) N(g) NO(g) H,O (g) H;0 (1) N,0 (g) NO2 (g) N2O N,Os(g) N20s(s) NHANO,(s) AH", (kJ/mol) 130.6 114.6 218.0 205 161 249.2 191.5 153.2 472.7 210.7 90.25 188.7 -241.8 69.91 -285.8 219.7 82.05 240.0 33.2 304.2 9.2 356 11 178 -43.1 151.1 -365.6