Chemistry

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Showing 126 to 150 of 1398 questions (page 6 of 56).

126. Extrapolation of the volume against temperature graph for a gas gives absolute zero at

A. 0 degrees Celsius B. -100 degrees Celsius C. -273.16 degrees Celsius D. -373 degrees Celsius E. 100 degrees Celsius

127. The value of the gas constant R in dm3 atm mol-1 K-1 is

A. 8.314 B. 0.0821 C. 1.987 D. 62.4 E. 0.083

128. According to Graham's law, the rate of diffusion of a gas is

A. proportional to its molar mass B. proportional to the square of its molar mass C. inversely proportional to the square root of its molar mass D. independent of molar mass E. proportional to the square root of its molar mass

129. In the van der Waals equation, the constant b accounts for

A. intermolecular attraction B. the volume occupied by the gas molecules C. the kinetic energy of the molecules D. the temperature correction E. the number of moles

130. A gas cannot be liquefied by pressure alone above its

A. boiling point B. melting point C. critical temperature D. inversion temperature E. transition temperature

131. The average kinetic energy of gas molecules is directly proportional to

A. pressure B. volume C. absolute temperature D. molar mass E. density

132. Dalton's law of partial pressures does not apply to gases that

A. are monatomic B. have different molar masses C. react chemically with each other D. are at high temperature E. are at low pressure

133. The abnormally high boiling point of water compared with hydrogen sulphide is due to

A. its low molar mass B. hydrogen bonding C. London dispersion forces D. its ionic character E. covalent network bonding

134. The boiling point of a liquid at reduced external pressure

A. increases B. decreases C. remains unchanged D. becomes zero E. doubles

135. The coordination number of each ion in a sodium chloride crystal is

A. 4 B. 6 C. 8 D. 12 E. 2

136. The existence of a substance in more than one crystalline form is called

A. isomorphism B. polymorphism C. isotopy D. allotropy in solutions only E. anisotropy

137. Which type of solid has the highest melting point?

A. molecular B. ionic C. metallic D. covalent network E. amorphous

138. The maximum number of electrons that can occupy the shell with n = 3 is

A. 8 B. 10 C. 18 D. 32 E. 6

139. For an electron in a 3d orbital, the azimuthal quantum number l is

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

140. The ground state electronic configuration of chromium (Z = 24) is

A. [Ar] 3d4 4s2 B. [Ar] 3d5 4s1 C. [Ar] 3d6 D. [Ar] 4s2 4p4 E. [Ar] 3d3 4s3

141. Rutherford's gold foil experiment established the existence of

A. the electron B. the neutron C. a small dense positively charged nucleus D. energy levels E. orbitals

142. The energy of a photon of frequency nu is given by

A. h/nu B. h nu C. nu/h D. h nu2 E. h/nu2

143. The shape of a p orbital is

A. spherical B. dumb bell C. double dumb bell D. tetrahedral E. planar triangular

144. Hund's rule requires that

A. electrons pair up before occupying empty degenerate orbitals B. degenerate orbitals are singly occupied with parallel spins before pairing C. the lowest energy orbital is filled last D. no two electrons can have the same spin E. d orbitals fill before s orbitals of the same shell

145. The bond angle in a molecule with sp3 hybridization and no lone pairs is

A. 90 degrees B. 104.5 degrees C. 107 degrees D. 109.5 degrees E. 120 degrees

146. The dipole moment of carbon dioxide is zero because the molecule is

A. non-polar in its bonds B. linear and symmetrical C. angular D. tetrahedral E. ionic

147. The shape of the ammonia molecule according to VSEPR theory is

A. trigonal planar B. tetrahedral C. trigonal pyramidal D. linear E. bent with 104.5 degrees

148. As bond order increases, the bond length

A. increases B. decreases C. remains constant D. first increases then decreases E. becomes zero

149. A coordinate covalent bond is present in

A. methane B. the ammonium ion C. sodium chloride D. chlorine E. ethene

150. The ionic character of a bond increases with

A. decreasing electronegativity difference B. increasing electronegativity difference C. increasing bond order D. decreasing atomic size only E. increasing covalent radius

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