The compound cyclohexanol, C,H1,0, is a good fuel. It is a liquid at ordinary temperatures. When the liquid is burned, the reaction involved is 2 C,H120(8) + 17 O2(g} →12 CO2(g) + 12 H,0(g) The standard enthalpy of formation of liquid cyclohexanol at 25 °C is -348.2 kJ mol'; other relevant enthalpy of formation values in kJ mol"' are: C,H120(g) = -286.2 ; CO2(g)= -393.5 ; H2O(g) =-241.8 (a) Calculate the enthalpy change in the burning of 5.000 mol liquid cyclohexanol to form gaseous products at 25°C. State explicitly whether the reaction is endothermic or exothermic. AH° = kJ (b) Would more or less heat be evolved if gaseous cyclohexanol were burned under the same conditions? What is the standard enthalpy change for vaporizing 5.000 mol C,H120(,) at 25°C? ΔΗ kJ Calculate the enthalpy change in the burning of 5.000 mol gaseous cyclohexanol to form gaseous products at 25°C. AH° = kJ

The compound cyclohexanol, C,H1,0, is a good fuel. It is a liquid at ordinary temperatures. When the liquid is burned, the reaction involved is 2 C,H120(8) + 17 O2(g} →12 CO2(g) + 12 H,0(g) The standard enthalpy of formation of liquid cyclohexanol at 25 °C is -348.2 kJ mol'; other relevant enthalpy of formation values in kJ mol"' are: C,H120(g) = -286.2 ; CO2(g)= -393.5 ; H2O(g) =-241.8 (a) Calculate the enthalpy change in the burning of 5.000 mol liquid cyclohexanol to form gaseous products at 25°C. State explicitly whether the reaction is endothermic or exothermic. AH° = kJ (b) Would more or less heat be evolved if gaseous cyclohexanol were burned under the same conditions? What is the standard enthalpy change for vaporizing 5.000 mol C,H120(,) at 25°C? ΔΗ kJ Calculate the enthalpy change in the burning of 5.000 mol gaseous cyclohexanol to form gaseous products at 25°C. AH° = kJ

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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Given the standard enthalpies of formation for the following substances, determine the reaction enthalpy for the following reaction. AGran =? kJ 4A (g) + 2B (3) → 1C (g)+ 7D (g) AGi in kJ/mol Substance A (g) B (g) C(g) D (g) 76.34 + 5.24 - 55.86 - 14.55 O - 452.59 kJ/mol O + 452.59 kJ/mol O + 137.17 kJ/mol O - 141.51 kJ/mol O - 137.17 kJ/mol
Butane, C4H10, is widely used as a fuel for disposable lighters When one mole of butane is burned in oxygen, carbon dioxide and steam are formed and 2654.3382 kJ of heat are evolved.. C4H10 (9) + O₂(g) → 4CO₂(g) +5H₂O(1) The standard enthalpies of formation of CO₂ and H₂O are: CO2(g)=-394.87 kJ/mol H₂O(1)=-285.59 kJ/mol Calculate the standard heat of formation of butane. (Round answer to the second decimal place)
2. จงหาค่า AH ของปฏิกิริยานี้ จากข้อมูลที่กำหนดให้ 2C (s) + 2 H,0 (g) → CH, (g) + CO,(g) Determine the standard enthalpy change for this reaction from the following standard enthalpies of reaction: (1) C(s) + H,O (g) → CÓ (g) + H, (g) AH° = 131.3kJ (2) CO (g) + H2O (g) → CO2 (g) + H2 (g) ΔΗΟ = -41.2 kJ (3) CH, (g) + H,O (g) → 3H, (g) + CO (g) AH° = 206.1kJ ชื่อ-สกุล .วันที่ เลขที่ เรหัส.. (0202104) จงหาค่า AH และ As ของปฏิกิริยานี้ จากข้อมูลที่กำหนดให้ 3 ปฏิกิริยาการสังเคราะห์ด้วยแสงเกิดขึ้นดังสมการ 6 CO, (g) + 6 H,0 (1) CH2O6 (S) + 6 0, (g) กำหนดค่าที่สภาวะมาตรฐานของ AH และ S ของสารแต่ละตัว ดังนี้ AH°, (kJ mol-') s° (JK-1 mol-') สาร | CH,206 (s) -1,273 212 O, (g) 205 2/2 CO, (g) -393 214 H,0 (1) -285 70
Calculate the enthalpy for the reaction, BaC₂ (s) + 2 H₂O (l) → Ba(OH)₂ (aq) + C₂H₂ (g) Using the appropriate data from the following reactions, Ba (s) + 2 C (graphite, s) → BaC₂ (g) ∆H° = +437 kJ/mol Ba (s) + 2 H₂O (l) → Ba(OH)₂ +H₂ (g) ∆H° = -374.7 kJ/mol Ba (s) + 1/2 O₂ (g) → BaO (s) ∆H° = -553.5 kJ/mol BaO (s) + H₂O (l) → Ba(OH)₂ (aq) ∆H° = -107 kJ/mol C₂H₂ (g) + 5/2 O₂ (g) → 2 CO₂ (g) + H₂O (l) ∆H° = -1300. kJ/mol C (graphite, s) + O₂ (g) → CO₂ (g) ∆H° = -393.5 kJ/mol H₂ (g) + 1/2 O₂ (g) → H₂O (l) ∆H° = -285.8 kJ/mol
(b) Calculate the enthalpy change for the reaction C(graphite) + 2 H2(g) → CH4(g) with the help of the enthalpy changes of the following reactions: C(graphite) + O2(g) → CO2(g) ∆H= -393.5 kJmol−1 H2(g) +1/2O2(g) → H2O(l) ∆H = -285.8 kJmol−1 CH4(g) + 2 O2(g) → CO2(g) + 2 H2O(l) ∆H = -890.4 kJmol−1 The temperature is 25 ◦C in all instances.
10.00 g of Compound X with molecular formula C4H8 are burned in a constant-pressure calorimeter containing 50.00 kg of water at 25 °C. The temperature of the water is observed to rise by 2.151 °C. (You may assume all the heat released by the reaction is absorbed by the water, and none by the calorimeter itself.) Calculate the standard heat of formation of Compound X at 25 °C. Be sure your answer has a unit symbol, if necessary, and round it to 2 significant digits.
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
Use the standard reaction enthalpies given below to determine ΔH°rxn for the following reaction (show all work): P4(g) + 10 Cl2(g) → 4PCl5(s) ΔH°rxn = ? Given: PCl5(s) → PCl3(g) + Cl2(g) ΔH°rxn = +157 kJ P4(g) + 6 Cl2(g) → 4 PCl3(g) ΔH°rxn = -1207 kJ
55. Does the standard enthalpy of formation of H2O(g) differ from ΔH° for the reaction 2H2(g)+O2(g)⟶2H2O(g)?
1 If the standard enthalpy of cembustion of gaseous cyclopropane, C3H6, is -2091.2 kJ mol- at 25 C, calculate the standard enthalpy of formation of the compound at 298 K. (The standard enthalpy of combustion is the heat of combustion of one mole of a compound to the most stable combustion products, which are CO2(g) and H20(1) in the case of hydrocarbons. The standard enthalpy of formation is the enthalpy of formation of one mole of a compound from its constituent elements, the compound and its constituent elements in their standard states.)
Hydrobromic acid (HBr) is a commonly used acid for adding bromine to organic compounds. As bromine makes for an easily replaceable substituent, these bromine precursors are a necessary part of a vast amount of organic eynthesis, Calculate the reaction enthalpy for the synthesis of HBr according to H2(g) + Bra)2Br(g) Use the following information: NH3(g) +HBr(g) → NHABr(s) AH =-188.32 kJ Na(g) + 3H2(g) → 2NH3(g) AH = -92.22 kJ N2(g) + 4H2(g) + Br2(1) → 2NHABr(s) AH =-541.66 kJ a. AH =-728 kmol b. AH =-1010.52 KJjmol C. AH =-826.08 KJ/mol d. AH =728 kJ/mol e. AH = -257.24 kJ/mol Clear my choice
（1）Consider the reaction: 2A (g) + 3 B (g) → 2 C (g) ΔHrxn = +254.3 kJ What will be the enthalpy change (in kJ) if 0.471 mol B reacts in excess A? （2）Consider the reaction: C (s) + O2 (g) → CO2 (g) ΔHrxn = -393.5 kJ What mass of carbon (in g) must be reacted via this mechanism to release 581.2 kJ of heat?