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Showing 2701 to 2725 of 3046 questions (page 109 of 122).

2701. Standard temperature and pressure are defined as

A. 273 K and 760 mm of mercury only at the equator B. 0 K and zero pressure C. 298 K and 1 atm D. 373 K and 1 atm E. 273.15 K and 1 atm

2702. The volume occupied by 0.5 mol of any ideal gas at STP is

A. 22.4 dm3 B. 11.2 dm3 C. 2.24 dm3 D. 44.8 dm3 E. 5.6 dm3

2703. A hydrogen bond is typically

A. weaker than a covalent bond but stronger than a London force B. weaker than a London dispersion force C. of zero energy D. stronger than a covalent bond E. identical to an ionic bond

2704. Ice floats on water because

A. water is denser at 0 degrees Celsius than at 4 degrees Celsius B. it contains dissolved air only C. hydrogen bonding gives ice an open structure of lower density D. ice is amorphous E. it is warmer

2705. Molecular solids are generally

A. good conductors of electricity B. hard with high melting points C. soft with low melting points D. network covalent E. ionic in character

2706. Ionic solids conduct electricity

A. only when molten or dissolved B. only as vapours C. in the solid state D. only at absolute zero E. never

2707. Cleavage of a crystal along definite planes shows that

A. the crystal contains water B. the crystal is ionic C. the crystal is amorphous D. the particles are arranged in an ordered pattern E. the crystal is anisotropic in colour only

2708. The three isotopes of hydrogen are

A. hydride, proton and hydronium B. protium, deuterium and tritium C. ortho, meta and para hydrogen D. alpha, beta and gamma hydrogen E. hydrogen, helium and lithium

2709. The maximum number of electrons that a d subshell can hold is

A. 10 B. 2 C. 18 D. 6 E. 14

2710. The wave mechanical model of the atom is based on the equation formulated by

A. Bohr B. Rutherford C. Schrodinger D. Chadwick E. Planck

2711. The existence of discrete spectral lines rather than a continuous spectrum shows that atomic energy is

A. continuous B. quantized C. zero D. independent of the electron E. infinite

2712. The number of lone pairs on the oxygen atom in a water molecule is

A. 3 C. 4 D. 1 E. 2

2713. The shape of the phosphorus pentachloride molecule is

A. tetrahedral B. see saw C. trigonal bipyramidal D. square planar E. octahedral

2714. The number of sigma bonds in an ethyne molecule is

A. 4 B. 3 C. 1 D. 2 E. 5

2715. The number of pi bonds in a benzene molecule, on the Kekule representation, is

A. 3 B. 2 C. 6 D. 1

2716. The specific heat capacity of water is about

A. 1.0 J g-1 K-1 B. 4.18 J g-1 K-1 C. 2.09 J g-1 K-1 D. 336 J g-1 K-1 E. 8.314 J g-1 K-1

2717. The dissolution of ammonium chloride in water lowers the temperature, so the process is

A. endothermic B. exothermic C. isothermal D. spontaneous only above 100 degrees Celsius E. adiabatic

2718. The imaginary surface separating a system from its surroundings is called the

A. phase B. meniscus C. medium D. interface E. boundary

2719. Enthalpy changes of reaction are normally quoted in

A. kJ K-1 B. J K-1 mol-1 C. kJ mol-1 D. J E. mol kJ-1

2720. The enthalpy of formation of a compound can be found from enthalpies of combustion using

A. Raoult's law B. Le Chatelier's principle C. Graham's law D. Hess's law E. Dalton's law

2721. Chemical equilibrium is described as dynamic because

A. the temperature keeps changing B. the concentrations keep changing C. the reaction has stopped D. both forward and reverse reactions continue at equal rates E. the catalyst is consumed

2722. The pH of a 0.01 mol dm-3 solution of sodium hydroxide at 25 degrees Celsius is

A. 12 B. 14 C. 7 D. 2 E. 10

2723. Phenolphthalein is a suitable indicator for the titration of

A. two neutral solutions B. a weak acid with a strong base C. a strong acid with a weak base D. a strong acid with a strong acid E. a weak acid with a weak base

2724. The volume of 0.1 mol dm-3 hydrochloric acid needed to neutralize 25 cm3 of 0.1 mol dm-3 sodium hydroxide is

A. 2.5 cm3 B. 50 cm3 C. 12.5 cm3 D. 25 cm3 E. 100 cm3

2725. A concentration of one part per million corresponds to

A. 1 mol of solute in 10^6 dm3 B. 1 mg of solute in 1 kg of solution C. 1 cm3 of solute in 1 dm3 D. 1 g of solute in 1 g of solution E. 1 g of solute in 1 kg of solution

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