4.8 A phenol can be prepared from benzene using correct reaction schemes. Choosecorrect scheme for the synthesis of phenol from benzene from the options givenA.B.C.D.SO₂H₂SO4HNO3H₂SO4SO3H₂SO4SO₂H₂SO4ProductProductProductProduct1. NaOH, 300 °C2. H₂O*1. NaOH, 300 °C2. H₂O*1. SnCI,, HyO*2. HO1. NaOH, 200 °C2. H₂O*PhenolPhenolPhenolPhenolInn.

For the product of phenol from benzene first of all we introduce a sulfonic acid group on the…

4.8 A phenol can be prepared from benzene using correct reaction schemes. Choose correct scheme for the synthesis of phenol from benzene from the options given A. B. C. D. SO₂ H₂SO4 HNO₂ H₂SO4 SO₂ H₂SO4 SO₂ H₂SO4 Product - Product Product Product 1. NaOH, 300 °C 2. H₂0* 1. NaOH, 300 °C 2. H₂O* 1. SnCl, HyO* 2. HO 1. NaOH, 200 °C 2. H₂O* Phenol Phenol Phenol Phenol I POVE

4.8 A phenol can be prepared from benzene using correct reaction schemes. Choose correct scheme for the synthesis of phenol from benzene from the options given A. B. C. D. SO₂ H₂SO4 HNO₂ H₂SO4 SO₂ H₂SO4 SO₂ H₂SO4 Product - Product Product Product 1. NaOH, 300 °C 2. H₂0* 1. NaOH, 300 °C 2. H₂O* 1. SnCl, HyO* 2. HO 1. NaOH, 200 °C 2. H₂O* Phenol Phenol Phenol Phenol I POVE

Organic Chemistry

8th Edition

ISBN:9781305580350

Author:William H. Brown, Brent L. Iverson, Eric Anslyn, Christopher S. Foote

Publisher:William H. Brown, Brent L. Iverson, Eric Anslyn, Christopher S. Foote

Chapter5: Alkenes: Bonding, Nomenclature, And Properties

Section: Chapter Questions

Problem 5.31P

See similar textbooks

Similar questions

Hexanoic acid was added to an immiscible biphasic solvent system, water and CCl4 at 20.0OC and the equilibrium concentrations of hexanoic acid were determined to be 3.66 g/L in H2O and 67.0 g/L in CCl4. Caluclate the distrubution coeffiecent (D2) of hexanoic acid in water with respect to CCl4.
At constant pressure and 25°C, what is ΔrH° for the following reaction2C2H6(g) + 7O2(g) → 4CO2(g) + H2O(l)if the complete consumption of 14.5 g of C2H6 liberates 752.3 kJ of heat energy?
Hexanoic acid was added to an immiscible biphasic solvent sysem, water and CCl4 at 20.0OC and the equilibrium concentrations of hexanoic acid were determined to be 3.66 g/L in H2O and 67.0 g/L in CCl4. Caluclate the distrubution coeffiecent (D1) of hexanoic acid in CCl4 with respect to water.
Determine AGrxn for 2 A(g) + B₂(g) → 2 AB(g) A. -400 kJ B. -250 kJ C. -200 kJ D. -100 kJ E. -50 kJ Compound(state) AG (kJ/mol) A(g) B₂(g) AB(g) 0 -100 -150
COMPOUND ∆Hf (kJ/mole) S° (J/K mole) MgCO3 –1111 65.86 BaCO3 –1213 112.1 MgO –601.6 27.0 BaO –548 72.1 CO2 –393.5 213.8 Calculate ∆G° for the reaction of MCO3 ---> MO + CO2 at 25°C for the alkaline earth compounds Mg and Ba
Develop a general equation for the standard heat of reaction as a function of temperature for one of the reactions given in parts (a), (b), (c) a. CH3CHO(g) + H2(g) → C2H5OH(g) b. C2H5CH:CH2(g) → CH2:CHCH:CH2(g) + H2(g) c. C4H10(g) → CH2:CHCH:CH2(g) + 2H2(g)
Calculate ∆Hrxn for the reaction of MgO(s) with HCl(g): 2 MgO(s)+ 4 HCl(g)⟶⟶ 2 MgCl2(s) + 2 H2O(l) ∆Hrxn = ? using the following equations: Mg(s) + 2HCl(g)⟶⟶ MgCl2(s) + H2(g) ∆Hrxn = -456.9 kJ 2Mg(s) + O2(g) ⟶⟶2MgO(s) ∆Hrxn = -1203.2 kJ 2H2O(l) ⟶⟶2H2(g) + O2(g) ∆Hrxn = 571.6 kJ
For the reaction 2 H2S(g) <==> 2 H2(g) + S2(g) the value of Kc = 1.6e-2 Calculate the value of Kc for this second reaction below: 8 H2(g) + 4 S2(g) <==> 8 H2S(g)
Be sure to answer all parts. Use the table to calculate ΔG for the following reactions at 25°C. Species Δ G o f (kJ/mol) Mg(s) 0 O2(g) 0 MgO(s) −255.0 SO2(g) −300.57 SO3(g) −370.53 C2H2(g) 168.43 CO2(g) −394.65 H2O(l) −237.35 H2O(g) −228.77 (a) 2 Mg(s) + O2(g) → 2 MgO(s) kJ (b) 2 SO2(g) + O2(g) → 2 SO3(g) kJ (c) 2 C2H2(g) + 5 O2(g) → 4 CO2(g) + 2 H2O(l) kJ
When butanoic acid (7.0 mL) is dissolved in methanol (20 mL) and heated with a catalytic amount of concentrated sulfuric acid, methyl butanoate (6.5 mL) is isolated. Calculate the per cent yield for the formation of this product. (Use a mole for the process)
1.1The Ksp of Ca3 (PO4 ) 2 is 1.3 × 10−26 . Estimate the solubility of this salt in units of g. L −1 . You must show any reaction equation(s) that you may think are necessary. 1.2 If a sample of solid Ca3(PO4)2 is stirred into exactly one litre of a 0.550M solution of Na3PO4, how will the solubility of the salt compare with the answer that you have obtained in question 1.1? Explain you answer in a short sentence.
Develop a general equation for the standard heat of reaction as a function of temperature for one of the reactions given in parts (a), (b), (c) a. C2H5CH:CH2 (g) → CH2:CHCH:CH2 (g) + H2 (g) b. 2H2S(g) + 3O2 (g) → 2H2O(g) + 2SO2 (g) c. CH3OH(g) +1/2O2 (g) → HCHO(g) + H2O(g)