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AP Intermediate 2nd Year Haloalkanes, Alcohols and Ethers — practice questions

Explore 74 free Haloalkanes, Alcohols and Ethers questions in AP Intermediate 2nd Year Chemistry. Open each question or exercise to read its content, reference answers and available explanation.

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Haloalkanes, Alcohols and Ethers questions and exercises with answers

Showing questions 1–30 of 74.

For a galvanic cell, the standard cell EMF is given by:Read the answer and worked solution →The boiling point elevation $\Delta T_b$ of a dilute solution is:Read the answer and worked solution →For an **ideal** solution, the enthalpy of mixing $\Delta_{mix}H$ is:Read the answer and worked solution →Raoult's law for a volatile component of a solution states $P_i$ equals:Read the answer and worked solution →If 18 g of glucose (M = 180 g/mol) is dissolved in 90 g of water (M = 18 g/mol), the mole fraction of glucose is approximately:Read the answer and worked solution →Which gas does **not** obey Henry's law in water, because it reacts chemically with the solvent?Read the answer and worked solution →The relative lowering of vapour pressure of a dilute solution of a non-volatile solute equals:Read the answer and worked solution →If $K_b$ for water is 0.512 K·kg/mol, the boiling point elevation of a 0.50 molal aqueous urea solution is:Read the answer and worked solution →A solution that shows **positive** deviation from Raoult's law typically has:Read the answer and worked solution →Solutions are homogeneous mixtures of two or more components. In a binary solution, the component present in the largest quantity is termed the:Read the answer and worked solution →An amalgam of mercury with sodium is an example of which type of solution?Read the answer and worked solution →Which of the following concentration units is *temperature-dependent*?Read the answer and worked solution →The sum of mole fractions of all components in a solution equals:Read the answer and worked solution →Molality (m) is defined as:Read the answer and worked solution →Calculate the molality of a solution prepared by dissolving 2.5 g of ethanoic acid (CH₃COOH, M = 60 g mol⁻¹) in 75 g of benzene.Read the answer and worked solution →The molarity of a solution containing 5 g of NaOH (M = 40 g mol⁻¹) in 450 mL of solution is:Read the answer and worked solution →The mole fraction of ethylene glycol (C₂H₆O₂, M = 62) in a 20% by mass aqueous solution is approximately:Read the answer and worked solution →Oxidation state of Cu in [Cu(NH₃)₄]²⁺:Read the answer and worked solution →Carbonyl carbon hybridization:Read the answer and worked solution →Phenol is more acidic than ethanol because:Read the answer and worked solution →The Williamson ether synthesis works best with:Read the answer and worked solution →An ALCOHOL in which the $\mathrm{-OH}$ group is attached to a carbon bonded to ONE other alkyl group is classified asRead the answer and worked solution →The IUPAC name of $\mathrm{(CH_3)_2CHOH}$ isRead the answer and worked solution →The reaction of ethanol with sodium metal producesRead the answer and worked solution →The acidity (Brønsted acidity) order of the following isRead the answer and worked solution →Ethanol heated with concentrated $\mathrm{H_2SO_4}$ at $443\,\text{K}$ (170°C) gives mainlyRead the answer and worked solution →The WILLIAMSON ETHER SYNTHESIS prepares ethers by reactingRead the answer and worked solution →The REIMER-TIEMANN reaction converts phenol to salicylaldehyde. The reagents areRead the answer and worked solution →Phenol reacts with bromine WATER (aqueous $\mathrm{Br_2}$) at room temperature to giveRead the answer and worked solution →Ethanol reacts with $\mathrm{PCl_5}$ to give which set of products?Read the answer and worked solution →

Worked practice questions

For a galvanic cell, the standard cell EMF is given by:

  1. $E^{\circ}_{\text{cell}} = E^{\circ}_{\text{cathode}} + E^{\circ}_{\text{anode}}$
  2. $E^{\circ}_{\text{cell}} = E^{\circ}_{\text{anode}} - E^{\circ}_{\text{cathode}}$
  3. $E^{\circ}_{\text{cell}} = E^{\circ}_{\text{cathode}} - E^{\circ}_{\text{anode}}$
  4. $E^{\circ}_{\text{cell}} = -2 E^{\circ}_{\text{anode}}$
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Correct answer: C. $E^{\circ}_{\text{cell}} = E^{\circ}_{\text{cathode}} - E^{\circ}_{\text{anode}}$

$E^{\circ}_{\text{cell}} = E^{\circ}_{\text{cathode}} - E^{\circ}_{\text{anode}}$, where both potentials are listed as standard *reduction* potentials. For a spontaneous galvanic cell, $E^{\circ}_{\text{cell}} > 0$, which means the cathode has the higher reduction potential. This is just an algebraic restatement of "reduction happens at the cathode".

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The boiling point elevation $\Delta T_b$ of a dilute solution is:

  1. Directly proportional to molality
  2. Independent of molality
  3. Proportional to mole fraction of solvent
  4. Inversely proportional to molality
Show answer and solution

Correct answer: A. Directly proportional to molality

$\Delta T_b = K_b m$, directly proportional to molality $m$. $K_b$ is the ebullioscopic (molal elevation) constant — the BP elevation produced by a 1 molal solution.

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For an **ideal** solution, the enthalpy of mixing $\Delta_{mix}H$ is:

  1. Negative
  2. Equal to T·ΔS
  3. Zero
  4. Positive
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Correct answer: C. Zero

Ideal solutions obey Raoult's law over all compositions. solute–solvent, solute–solute and solvent–solvent interactions are comparable so no heat is released or absorbed on mixing — $\Delta_{mix}H = 0$ (and $\Delta_{mix}V = 0$).

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More Chemistry topics

Amines and BiomoleculesThe d- and f-Block Elements & Coordination CompoundsElectrochemistryChemical KineticsAldehydes, Ketones and Carboxylic AcidsSolutionsHaloalkanes and HaloarenesAlcohols, Phenols and Ethers