Calculate Section in J/mol at 298.15 K givenCH (g) + N₂(g) → HCN(g) + NH3(g)AS reaction - Ens Products - En SoAG (kJ/mol)-50.50SubstanceCH (9)N₂(9)HCN (9)124.7NH:(g) -16.5O none of theseO-134:38O24.80 16.7O-2149Renetan to04430 29.500088601770886AH (kJ/mol)-74.60135.5-45.9SK (V/mol K)186.3191.6201.8192.8Question 31Calculate T (in K) given AG 44 kymol and AH-28.1 kJ/mol and AS-814 /mol KAG AH TAS

Answered: Image /qna-images/answer/a59620cc-d0a5-444f-9e5d-c6074fa93938.jpg

Calculate A Section in J/mol at 298.15 K given CH (g) + N₂(g) → HCN(g) + NH3(g) AS reaction = nS Products - En AG (kJ/mol) -50.5 0 Substance CH (9) N₂(9) HCN (9) 124.7 NH:(9) -16.5 O none of these O-13438 0 24.8 016.7 O-2149 Renetan to 0443 0 29.5 00.0886 0177 0886 AH (kJ/mol) -74.6 0 135.5 -45.9 S8K (V/mol K) 186.3 191.6 201.8 192.8 Question 31 Calculate T (in K) given AG-44 kymol and AH-28.1 kJ/mol and AS-814 /mol K AG AH TASⓇ

Calculate A Section in J/mol at 298.15 K given CH (g) + N₂(g) → HCN(g) + NH3(g) AS reaction = nS Products - En AG (kJ/mol) -50.5 0 Substance CH (9) N₂(9) HCN (9) 124.7 NH:(9) -16.5 O none of these O-13438 0 24.8 016.7 O-2149 Renetan to 0443 0 29.5 00.0886 0177 0886 AH (kJ/mol) -74.6 0 135.5 -45.9 S8K (V/mol K) 186.3 191.6 201.8 192.8 Question 31 Calculate T (in K) given AG-44 kymol and AH-28.1 kJ/mol and AS-814 /mol K AG AH TASⓇ

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

6.69. Adding 2.00 g of Mg metal to 95.0 mL of 1.00 M HCl in a coffee-cup calorimeter leads to a temperature increase of 9.2°C. 01 020072 Ha. b. 10 (lom. Write a balanced net ionic equation for the reaction. If the molar heat capacity of 1.00 M HCl is the same as that for water [cp = 75.3 J/(mol °C)], what is AHxn? ·C 11°
and 2 Enthalpy #1.30 enoindice pled TT 2010 2D49.bs 22) When 1 mole of Fe2O3(s) reacts with H₂(g) to form Fe(s) and H2O(g) according to the following equation, 98.8 kJ of energy are absorbed. (6 Fe2O3(s) + 3 H2(g) → 2 Fe(s) + 3 H₂O(g) (pp) (20/d4 (pm) $40 D Reaclanis 13:48 SH Products endothermic, A endothermic, B (2) exothermic, A exothermic, B nad W (21 Enthalpy MOMS. Reactants Products (A) (B) Is the reaction endothermic or exothermic, and which of the enthalpy diagrams above represents grow olor and to noin (01 this reaction? SH GH TH A HOMH X HILD 08.10 Page 6 of 8
Methane-producing bacteria convert liquid acetic acid (CH3CO₂H) into CO₂(g) and CH₂(g). AS° ΔΗ, Ο (kJ/mol) (J/mol.K) CH3CO₂H (1) -484.5 159.8 CO₂(g) -393.5 213.8 CH₂(g) -74.8 186.2 Calculate AHOrxn = kJ Calculate AG rxp = (round to 3 sig figs) Is this process endothermic or exothermic under standard conditions? Is the reaction spontaneous under standard conditions? kJ (round to 3 sig figs)
(D 263 kJ/mol P. 22. Using the following thermochemical equations: C(s) + O,(g) → CO,(g) ΔΗΟ. rxn 1 =-394 kJ/mol,Txn C(s) + CO,(g) → 2 CO(g) AH°. Ixn 2 =+173 kJ/mol,xa Determine the enthalpy of the reaction represented below: 2 C(s) + 0,(g) → 2 CO(g) ΔΗ Txn 3 = ? 1> (A) ΔΗ. :-567 kJ/molxn rxn (В) ДН =-221 kJ/mol,xn (С) ДН =+221 kJ/molpxn (D) AH°. +567 kJ/molpxn %3D Ixn qt ian od geind hw qua boalunai na cop d ofiosa orb d A 100--32 HO0-02 X convinn or rmrainn an nart of this nanA iR llanal.
One of the reactions that destroys ozone in the upper atmosphere is NO(g) + 03 (g) ⇒ NO2 (g) + O₂(g) Substance and State ▲Gƒ° (kJ/mol) NO(g) 87 NO₂(g) 52 0₂ (9) 0 03 (9) 163 a Calculate AG (at 298 K) for this reaction. l\G° = Submit KJ
4) Consider the thermochemical equation below. What mass of HgO must decompose to consume 400.0 kJ of heat? 2 HgO (s) → 2 Hg (1)+ O2(g) AH°rxn =+ 181.4 kJ (1) 5) Write the standard formation reaction for KAI(SO4)2(s). (1) 3 CO2 (g). (1) -393.5 kJ/mol 2 Cr (s) + 3 CO (ag) -110.5 kJ/mol Cr2O3 (s) 6) Consider the reaction 0.0 kJ/mol AH°f = -1139.7 kJ/mol Calculate AH°rxn.
Given the following reactions: N2 (g) + O2 (g) → 2NO (g) AH = +180.7 kJ 2N20 (g) → O2 (g) + 2N2 (g) AH = -163.2 kJ the enthalpy of reaction for 2N20 (g) → 2NOo (g) + N2 (g) is kJ. -343.9 343.9 -145.7 145.7 O 17.5
Cl2 (g) + H2 (g) → 2 HCl (g) ΔH0rxn = ‒184.6 kJ 8. What is ΔH0rxn when 4.50 mol HCl (g) forms? (Slides 17 – 18: Stoichiometry of Thermochem. Eq.) Group of answer choices A.‒831 kJ B.‒415 kJ C.‒207 kJ D.831 kJ E.415 kJ
1) From the following data, C(graphite) + O2(g) à CO2(g) = -393.5 kJ/mol H2(g) + 1/2O2(g) = H2O(l) delta H = -285.8 kJ/mol 2C2H6(g) + 7O2(g) = 4CO2(g) + 6H2O(l) delta H = -3119.6 kJ/mol calculate the enthalpy change for the reaction 2C(graphite) + 3H2(g) =C2H6(g) a) –2417.2 kJ b) –84.6 kJ c) 2417.2 kJ d) –3204.2 kJ
4) Given the reactions (1) and (2) below, determine a) A,H and A.U for reaction (3); b) AH® for both HCl(g) and H₂O(g). Assume all gases are perfect and T= 298 K. (1 point) (1) H₂(g) + Cl2(g) → 2HCl(g) AH +52.96 kJ/mol (2) 2H2(g) + O2(g) → 2H₂O(g) A.HⓇ -483.64 kJ/mol (3) 4HCl(g) + O2(g) → 2Cl2(g) + 2H₂O(g) =
A chemist measures the enthalpy change AH during the following reaction: COCL,(9) + 4 NH,(g)–+cO(NH,),(s) + 2 NH,Cl(s) AH=-559. kJ Use this information to complete the table below. Round each of your answers to the neare reaction AH co(NH,),(-) + NH,CI(3) - coC, () + 2NH, (2) 3coCI, (3) + 12NH, (3) - 3c0(NH,), (-) + 6NH,CI(s) co(NH,),() + 2NH,C1(«) → COCI, (3) + 4NH, (2) Explanation Check MacBook Air 20 F1 F3 F4 F5 F6 F @ & くC
Given the following enthalpy change values for the reactions below: A + B → 2C; AH = -485.1 kJ mol-¹ C + 2D + E +F; AH = 251.4 kJ mol-¹ ½E + G +H; AH = 471.1 kJ mol-¹ Calculate A,H for the following reaction (in kJ mol-¹) using Hess's Law: A + B + 4D + 4G → 4H + 2F Answer: