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Chapter 4 Solutions
EP ORGANIC CHEMISTRY -MOD.MASTERING 18W
- Using the table of average bond energies below, the AH for the reaction is kJ. ethanol → ethene + water нн нн Н—С—с—0—н → Ć=Ċ + H-0-H Bond сСС-СО-НС-Н СО AH (kJ/mol) 611 348 464 413 360 -6168 6168 -306 63 46 217arrow_forwardWe want to find the enthalpy change (ΔHΔH) for the reaction: 2CH4->C2H6+H2 Given the following reactions: H2+1/2O2→H2O (Given ΔH=−285.8 kJ CH4→2O2->CO2+2H2O (Given ΔH=−890.3 kJ C2H6+7/2O2→2CO2+3H2O (Given ΔH=−1559.9 kJarrow_forwardGiven that ∆H° for the reaction is -42 kcal/mol and the bond dissociation enthalpies for the C - H, C - Cl, and O - H bonds are 101, 85, and 105 kcal/mol respectively, calculate the bond dissociation enthalpy of the O - Cl bond.arrow_forward
- Find the AHn for the following reaction: B2 He (g) + 6 Cl2(9) → 2 RC13(9) + 6 HC(g) given the following reactions and subsequent AH° values $$ BC13 (9) + 3 H2O(1) → H3 BO3(g) + 3 HCl(g) AH° = -113.1 kJ B2 H6 + 6 H2O(l) → 2 H3 BO3(9) + 6 H2 (9) AH° = -496 kJ 1 1 H2 (g) + Cl,(g) 2 HC(g) AH° = -95.5 kJ 2 $$arrow_forwardUse bond-dissociation enthalpies to calculate the AH° for each of the following reactions. CH3CH2CH3+H2 → CH3CH3+CH4 CH3CH2CL+HI → CH3CH2I+HCIarrow_forwardUse the given bond energy values to estimate ΔH for the following gas-phase reaction. (Simple energy units required for the answer.) D-values in kJ/mol DH-H = 432 DH-Br = 363 DH-C = 413 DH-N = 391 DH-O = 467 DC-C = 347 DC=C = 614 DC≡C = 839 DC-N = 305 DC=N = 615 DC≡N = 891 DC-O = 358 DC=O = 745 DC=O (CO2) = 799 DC≡O=1072 DC-Br = 276 DN-N = 160. DN=N = 418 DN≡N = 941 DO-O = 146 DO=O = 495 DN-O = 201 DN=O = 607 DBr-Br = 193 DC-Cl = 339 DH-Cl = 427 DCl-Cl = 239arrow_forward
- Given the following data: 4C(s) + 4H2(g) + O2(g) → CH3CH2OCOCH3(l) ΔH°=-480.0 kJ CH3CH2OH(l) + O2(g) → CH3COOH(l) + H2O(l) ΔH°=-492.0 kJ 2C(s) + 3H2(g) + 1/2O2(g) → CH3CH2OH(l) ΔH°=-278.0 kJ H2(g) + 1/2O2(g) → H2O(l) ΔH°=-286.0 kJ calculate ΔH° for the reaction:CH3COOH(l) + CH3CH2OH(l) → CH3CH2OCOCH3(l) + H2O(l)arrow_forwardCalculate the enthalpy change for the reaction below. Compound Нeat Value -> 3NO(s) ,0,ls) AH +174 k (belONH2 -(aloH (2Fo+ ('N AH -183 k AH =-128 k) 2NO(g) O-137 kJ O-128 kJ -174kJ 270KJarrow_forwardA) Given the standard enthalpy changes for the following two reactions:(1) 2C(s) + H2(g)C2H2(g)...... ΔH° = 226.7 kJ(2) 2C(s) + 2H2(g)C2H4(g)......ΔH° = 52.3 kJwhat is the standard enthalpy change for the reaction:(3) C2H2(g) + H2(g)C2H4(g)......ΔH° = ?------- kJ B) Given the standard enthalpy changes for the following two reactions:(1) 2Pb(s) + O2(g)2PbO(s)...... ΔH° = -434.6 kJ(2) Pb(s) + Cl2(g)PbCl2(s)......ΔH° = -359.4 kJwhat is the standard enthalpy change for the reaction:(3) 2PbCl2(s) + O2(g)2PbO(s) + 2Cl2(g)......ΔH° = ?------ kJarrow_forward
- Now consider the following reaction: C2H5OH + 3O2→2CO2+ 3H2O ,ΔH=−1370 kJ/mol What is the enthalpy for the reaction reversed? reaction 1 reversed: 2CO2 + 3H2O→C2H5OH + 3O2arrow_forwardThe reaction of liquid methyl chloride (CH3Cl) with water produces methanol and hydrogen chloride gas at room temperature, despite the fact that ΔHo rxn = 28.3 kJ/mol. Using thermodynamic arguments, propose an explanation as to why methanol forms. CH3Cl (l) + H2O (l) → CH3OH (l) + HCl (g)arrow_forwardWhen ethene is mixed with hydrogen in the presence of a platinum catalyst, hydrogen adds across the double bond to form ethane. At room temperature, the reaction goes to completion. Predict the signs of ∆H° and ∆S° for this reaction. Explain these signs in terms of bonding and freedom of motion.arrow_forward
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