Question :
1.Which statement concerning the three states of matter FALSE?
A) Particles : 1318393
1.Which statement concerning the three states of matter is FALSE?
A) Particles of a gas are well separated, have no regular arrangement, and move at high speeds.
B) Particles of a solid have low kinetic energy, and are held close together by strong attractive forces.
C) Particles of a liquid have a rigid, ordered arrangement due to the high speeds of the liquid particles.
D) Gases have low densities and high compressibility due to the large amount of space between gas particles.
E) Phase changes between the three states of matter are physical changes; no change in the identity or composition of the substance occurs.
2.Gas pressure is a result of which of the following?
A) collisions of gas particles with each other
B) expansion of gas particles in an open container
C) the resistance of gas particles to flow
D) collisions of gas particles with the walls of the container
E) compressibility of gas particles
3.Which of the following statements correctly describes Boyle’s Law?
A) The volume of a gas is directly proportional to the number of moles of the gas, if the pressure and temperature remain constant.
B) The volume of a gas is directly proportional to the Kelvin temperature of the gas, if the pressure and amount of gas remain constant.
C) The pressure of a gas is inversely proportional to the volume of the gas, if the temperature and amount of gas remain constant.
D) The pressure of a gas is directly proportional to the Kelvin temperature of the gas, if the volume and amount of gas remain constant.
E) The total pressure exerted by a mixture of gases in a container is the sum of the partial pressures that each gas would exert alone.
4.Which of the following statements correctly describes Charles’s Law?
A) The volume of a gas is directly proportional to the number of moles of the gas, if the pressure and temperature remain constant.
B) The volume of a gas is directly proportional to the Kelvin temperature of the gas, if the pressure and amount of gas remain constant.
C) The pressure of a gas is inversely proportional to the volume of the gas, if the temperature and amount of gas remain constant.
D) The pressure of a gas is directly proportional to the Kelvin temperature of the gas, if the volume and amount of gas remain constant.
E) The total pressure exerted by a mixture of gases in a container is the sum of the partial pressures that each gas would exert alone.
5.Which of the following statements correctly describes Avogadro’s Law?
A) Equal volumes of any ideal gas contain the same number of moles, if measured at the same temperature and pressure.
B) The volume of a gas is directly proportional to the Kelvin temperature of the gas, if the pressure and amount of gas remain constant.
C) The pressure of a gas is inversely proportional to the volume of the gas, if the temperature and amount of gas remain constant.
D) The pressure of a gas is directly proportional to the Kelvin temperature of the gas, if the volume and amount of gas remain constant.
E) The total pressure exerted by a mixture of gases in a container is the sum of the partial pressures that each gas would exert alone.
6.Which of the following represent STP (Standard Temperature and Pressure) conditions?
A) T = 0 K and P = 1 atm
B) T = 273 K and P = 0 atm
C) T = 1 K and P = 1 atm
D) T = 273 K and P = 1 atm
E) T = 0°C and P = 760 atm
7.Dalton’s Law of Partial Pressures states which of the following?
A) The total pressure exerted by a mixture of gases in a container is equal to the highest partial pressure exerted by any of the gases in the container.
B) The total pressure exerted by a mixture of gases in a container is the sum of the pressures that each gas would exert if present alone under similar conditions.
C) The total pressure exerted by a mixture of gases in a container is the average of the pressures that each gas would exert if present alone under similar conditions.
D) The total pressure exerted by a mixture of gases in a container is inversely proportional to the pressure that each gas would exert if present alone under similar conditions.
E) The total pressure exerted by a mixture of gases in a container is equal to the range of partial pressures of each gas in the container.
8.Which statement INCORRECTLY describes what happens to a sample of gas when it experiences an increase in temperature?
A) The volume of the gas increases, as long as the pressure remains constant.
B) The pressure of the gas increases, if the volume remains constant.
C) The kinetic energy of the gas particles increases.
D) The number of gas particles increases.
E) The gas particles move with increased speed.
9.Which gas under the specified conditions would come closest to exhibiting ideal gas behavior?
A) H2 at low pressure and high temperature
B) NH3 at low pressure and high temperature
C) H2 at high pressure and low temperature
D) NH3 at low pressure and low temperature
E) NH3 at high pressure and low temperature
10.At 100°C, which gas sample exerts the greatest pressure?
A) A
B) B
C) C
D) D
E) They would all exert the same pressure.
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