22. Calculate the enthalpy change of formation of HNO; (aq) in the following reaction:Iultiple CInstruction3NO2 (g) + H2O (I) → 2HNO, (aq)+NO (g); AH,renction-138.4 kJThe enthalpies of formation of NO2 (g), H2O (), and NO (g) are +33.2 kJ, -285.8 kJ, and +90.2 kJ,respectively.1. Heat(A)&(B)(C)(D)(5)2. W

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22. Calculate the enthalpy change of formation of HNO, (aq) in the following reaction: Tultiple C nstruction 3NO; (g) + H,0 (I) → 2HNO, (aq) +NO (g); AHrection=-138.4 kJ The enthalpies of formation of NO, (g), H2O (1), and NO (g) are +33.2 kJ, -285.8 kJ, and +90.2 kJ, respectively. 1. Heat (A)a (B) (C) (D) (5) 2. W

22. Calculate the enthalpy change of formation of HNO, (aq) in the following reaction: Tultiple C nstruction 3NO; (g) + H,0 (I) → 2HNO, (aq) +NO (g); AHrection=-138.4 kJ The enthalpies of formation of NO, (g), H2O (1), and NO (g) are +33.2 kJ, -285.8 kJ, and +90.2 kJ, respectively. 1. Heat (A)a (B) (C) (D) (5) 2. W

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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6 8 7. Consider the following reaction: 2 CH;OH (g) → 2 CH4() O2 (g), AH = + 252.8 kJ a) Is this reaction exothermic or endothermic? b) Calculate the amount of heat transferred when 26.0 g of CH3OH(g) is decomposed by this reaction at constant pressure. Express the heat to three significant digits with the appropriate units. c) For a given sample of CH;OH, the enthalpy change during the reaction is 82.9 kJ. What mass of methane gas is produced? Express the mass to three significant digits with the appropriate units. d) How many kilojoules of heat are released when 38.8 g CH4(g) reacts completely with 02(g) to form CH,OH(g) at constant pressure?
The hypothetical element X and an oxide of X undergo the following reactions with oxygen, with the listed enthalpy changes: 4 X(5) + 3 02(g) – 2 X203(g) AHrxn = -400.0 kJ 4 XO2(g) – 2 X203(g) + O2(g) AHrxn - +200.0 kJ Using the above information, determine AHrxn for the following reaction: X(S) + O2g) – XO22) O -200.0 k) O -600.0 kJ O -150.0 k) O 200.0 kJ
Calculating the heat of reaction from molar reaction enthalpy a... A chemist measures the energy change AH during the following reaction: C,Hg(g)+50,(9) – -3 CO 2(g)+4H,0(1) AH=-2220. kJ Use the information to answer the following questions. endothermic. This reaction is... exothermic Suppose 36.3 g of C,Hg react. O Yes, absorbed. O Yes, released. Will any heat be released or absorbed? No. If you said heat will be released or absorbed in the second part of this question, calculate how much heat will be released or absorbed. Round your answer to 3 significant digits. Elanation Check 2021 McGraw-Hill Education. All Rights Reserved Term
The standard heat of formation, AH: , is defined as the enthalpy change for the formation of one mole of substance from its constituent elements in their Constants I Periodic Table standard states. Thus, elements in their standard states have ΔΗ 0. Heat of formation values can be used Part A to calculate the enthalpy change of any reaction. Consider, for example, the reaction For which of the following reactions is AHn equal to AH: of the product(s)?You do not need to look up any values to answer this question. 2NO(g) + O2 (g) = 2NO2 (g) with heat of formation values given by the following Check all that apply. table: ΔΗ | (kJ/mol) Substance 2Na(s) + F2 (g)–→2NAF(s) NO(g) O H2 (g) + O2(g)→H2O(g) 90.2 O2(g) O H,O2 (g)→O2(g) + H2O(g) NO2 (g) 33.2 O Na(s) + F2(g)→NAF(s) Then the standard heat of reaction for the overall reaction is O Na(s) + F2(1)→NAF(s) AHm= AH¡(products)– AH; (reactants) [2(90.2) + 0] 2(33.2) O 2H2 (g) + O2 (g)→2H2O(g) -114 k.J
dard enthalpy 6.68 (a) What is the value of the standard enthalpy of formation of an element in its most stable form? (b) Write the chemi. cal equation for the reaction whose enthalpy change is the standard enthalpy of formation of sucrose (table sugar), enthalpy of formation? C12H2„O11($), AHf°[C12H22O11(S)]. 6.69 For each of the following compounds, write a balanced ther. mochemical equation depicting the formation of one mole of the compound from its elements in their standard states and then look up AH°r for each substance in Appendix C. (a) NO2(8), (b) SO3(8), (c) NaBr(s), (d) Pb(NO3)2(s). 6.70 Write balanced equations that describe the formation of the following compounds from elements in their standard states, and then look up the standard enthalpy of formation for each substance in Appendix C: (a) H2O2(8), (b) CaCO3(s). (c) POCI3(1), (d) C,H;OH(1). 6.71 The following is known as the thermite reaction:ods 2 Al(s) + Fe2O3(s) Al203(s) + 2 Fe(s) This highly exothermic reaction is…
For which one of the following is the enthalpy of the reaction the same as the enthalpy of formation? A) 2 H (g) + Se (s) → H:Se (g) B) KOH (s) → K*(aq) + OH- (aq) C) 2 Fe (s) + 3 Cl2 (g) → 2 FeCl3 (s) D) Ni (s) + ½ O2 (g)- NiO (s)
3. Calculate the standard enthalpy of formation of acetylene (C2H2) from its elements: C(graphite) + O2(g) → CO2(g) H2(g) + 0,(g) 2C,H2(g) + 502(g) H,O(I) → 4CO2(g) + 2H2O(l) AHn = AHan = -393.5 kJ/mol AHan = -285.8 kJ/mol - 2598.8 kJ/mol %3!
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) $40 D Reaclanis 13:48 SH Products endothermic, A endothermic, B (2) exothermic, A exothermic, B nad W (21 Enthalpy MOMS. Reactants Products (A) (B) Is the reaction endothermic or exothermic, and which of the enthalpy diagrams above represents grow olor and to noin (01 this reaction? SH GH TH A HOMH X HILD 08.10 Page 6 of 8
(c) Consider the following chemical reaction: C;Hs(g) + H2(g) C2H6(g) + CH4(g) ΔΗ? %3D Calculate the enthalpy change for the reaction above using Hess's law. Thermochemical dat: H:(g) + ½O2(g) H2O(1) AH° =-285.8 kJ AH°combustion for CH4(g) AH° =-890.0 kJ/mol %3D CO:(g) C(s. graphite) + O:(g) AH° = +393.5 kJ AH°combustion for C2H6(g) AH = -1560.0 kJ/mol AH°, for C3H$(g) AH° =-103.8 kJ/mol
You wish to know the enthalpy change for the formation of liquid PCI, from the elements. P.()+6 Cl₂(g) →4 PC (6) A, H-7 The enthalpy change for the formation of PCs from the elements can be determined experimentally, as can the enthalpy change for the reaction of PCs (f) with more chlorine to give PCI, (s): P.()+10 Cl₂(g) 4 PCI, () A,H-1774.0 kJ/mol-rxn PCI, ()+ Cl₂(g) → PCI, (s) - A,H-123.8 kJ/mol-rxn Use these data to calculate the enthalpy change for the formation of 2.20 mol of PCs (4) from phosphorus and chlorine. Enthalpy change - k3
O THERMOCHEMISTRY Using Hess's Law to calculate net reaction enthalpy Lindsay Dimethyl ether, a useful organic solvent, is prepared in two steps. In the first step, carbon dioxide and hydrogen react to form methanol and water: CO,(g) + 3 H,(g) → CH;OH(1) + H,0(1) AH=-131. kJ In the second step, methanol reacts to form dimethyl ether and water: 2 CH,OH(1) → CH;OCH,(g) + H,0(1) AH=8. kJ Calculate the net change in enthalpy for the formation of one mole of dimethyl ether from carbon dioxide and hydrogen from these reactions. Round your answer to the nearest kJ. II
15. Using the standard enthalpies of formation for the chemicals involved, calculate the enthalpy change for the following reaction. (Note: Show the math clearly and provide units in your setup) (AH; Values in kJ/mol are as follows: NO, +32, H,0 -286, HNO3 -207, NO +90) 3NO2(8) + H,Oy O 2HNO3(aq) + NO(g) (g),