Mixed Practice

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Showing 1101 to 1125 of 3046 questions (page 45 of 122).

1101. The bond angle in water is about 104.5 degrees rather than 109.5 degrees because

A. hydrogen atoms repel each other B. the two lone pairs repel the bonding pairs more strongly C. of hydrogen bonding within the molecule D. the molecule is linear E. oxygen is sp2 hybridized

1102. A sigma bond is stronger than a pi bond because

A. it involves fewer electrons B. it involves sideways overlap C. it involves head on overlap giving greater electron density between the nuclei D. it is formed later E. it uses unhybridized orbitals

1103. The bond order in a nitrogen molecule is

A. 3 B. 2.5 C. 1.5 D. 1 E. 2

1104. Which of the following molecules is polar?

A. boron trifluoride B. carbon tetrachloride C. carbon dioxide D. methane E. hydrogen chloride

1105. Metallic bonding is best described as

A. the transfer of electrons from metal to non-metal B. hydrogen bonding between metal atoms C. the sharing of electron pairs between two atoms D. the electrostatic attraction between cations and a sea of delocalized electrons E. dipole induced dipole attraction

1106. The standard conditions for reporting thermochemical data are

A. 298 K and 10 atm B. 0 K and 1 atm C. 273 K and 1 atm D. 373 K and 1 atm E. 298 K and 1 atm

1107. The enthalpy of combustion of a substance is always

A. zero B. negative C. equal to the lattice energy D. equal to the enthalpy of formation E. positive

1108. In calorimetry, the heat exchanged is calculated from

A. q = m c delta T B. q = m/c delta T C. q = nRT D. q = P delta V E. q = c delta T / m

1109. A bomb calorimeter measures the heat of combustion at constant

A. pressure B. entropy C. temperature D. enthalpy E. volume

1110. Internal energy is a state function, which means it depends on

A. the path taken B. only the initial and final states C. the container shape D. the catalyst used E. the time taken

1111. A reversible reaction never goes to completion because

A. the pressure drops B. the temperature falls C. the reverse reaction becomes appreciable as products accumulate D. the reactants are impure E. the catalyst is exhausted

1112. Raising the temperature of an exothermic reaction at equilibrium

A. increases Kc B. has no effect C. stops the reaction D. shifts it towards the products E. shifts it towards the reactants

1113. The pH of pure water at 25 degrees Celsius is

A. 14 B. 8 D. 7 E. 6

1114. A larger value of the acid dissociation constant Ka indicates

A. a weaker acid B. a neutral solution C. a stronger acid D. a stronger base E. a buffer solution

1115. An aqueous solution of sodium acetate is

A. neutral B. basic C. a buffer on its own only at pH 7 D. amphoteric E. acidic

1116. The solubility product expression for silver chloride is

A. [Ag+][Cl-] B. [AgCl]/[Ag+][Cl-] C. [Ag+]2[Cl-] D. [Ag+][Cl-]2 E. [Ag+]/[Cl-]

1117. Dissolving 0.5 mol of solute in enough water to make 250 cm3 of solution gives a molarity of

A. 1 M B. 0.5 M C. 5 M D. 2 M E. 0.125 M

1118. The osmotic pressure of a dilute solution is given by

A. pi V = n/RT B. pi V = nRT C. pi = n/V D. pi = nRTV E. pi = RT/nV

1119. Molarity changes with temperature but molality does not, because molarity depends on

A. the volume of solution B. the mass of solvent C. the number of moles of solute D. the mass of solute E. the nature of the solute

1120. The solubility of most gases in water

A. is independent of temperature B. increases with decreasing pressure C. decreases with temperature D. increases with temperature E. is unaffected by pressure

1121. An oxidizing agent is a species that

A. donates protons B. gains electrons C. always contains oxygen D. increases its own oxidation number E. loses electrons

1122. The oxidation number of sulphur in sulphuric acid is

A. +4 C. +2 D. -2 E. +6

1123. The standard cell potential is calculated as

A. the sum of the two reduction potentials B. the average of the two potentials C. anode potential minus cathode potential D. cathode potential minus anode potential E. always zero

1124. The products of the electrolysis of concentrated aqueous sodium chloride using inert electrodes are

A. oxygen and hydrogen only B. sodium and oxygen C. hydrogen, chlorine and sodium hydroxide D. chlorine and oxygen only E. sodium and chlorine

1125. The function of the salt bridge in a galvanic cell is to

A. prevent oxidation B. maintain electrical neutrality in the two half cells C. supply electrons to the circuit D. act as the cathode E. increase the cell voltage

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