Try this as often as you like. You will get a different set of questions each time you attempt this quiz.
In the experiment showing the diffusion between ammonia (NH3) and hydrogen chloride (HCl), which of the following statements is FALSE?
Hydrogen chloride travels the furthest because it is less dense.
A white cloud of ammonium chloride is formed when the two gases mix.
The reaction takes place at the end nearest the hydrochloric acid.
Both ammonia and Hydrogen chloride must be very concentrated solutions.
Which one of the following statements best describes Boyle's Law?
For a fixed mass of gas at a constant temperature, the pressure of the gas is inversely proportional to its volume.
For a fixed mass of gas at a constant pressure, its temperature is proportional to its volume.
For a fixed volume of gas at a constant temperature, the pressure of the gas is inversely proportional to its mass.
The temperature of a fixed mass of gas at a constant pressure is inversely proportional to its volume.
Which one of the following does NOT express Boyle's Law?
Which one of the following expresses Charles' Law?
The graph shows the volume left in a glass container after 60 ml of hydrogen chloride gas reacts with 40 ml of ammonia gas. Ammonia + hydrogen chloride → ammonium chloride NH3 + HCl → NH4Cl Ammonia and hydrogen chloride are both gases, ammonium chloride is a solid. The total volume at the start is 100 ml. After reacting, there are 20 ml of gas left in the container because
when all of the ammonium chloride is formed, there is still some unreacted hydrogen chloride gas left in the container.
there is an excess of ammonia gas left in the container.
the two gases do not react in a 1:1 ratio.
the product of the reaction, ammonium chloride has a volume of 20 ml.
Which scientist is credited with the Law of Combining Volumes
Gay-Lussac
Boyle
Avogadro
Charles
Which law states that "equal volumes of gases under the same conditions of temperature and pressure contain equal numbers of molecules"?
Avogadro's
Gay-Lussac's
Boyle's
Charles'
80 ml of carbon monoxide (CO) are reacted with 40 ml of oxygen (O2). What volume of carbon dioxide (CO2) is formed? 2CO + O2 → 2CO2
80 ml
120 ml
40 ml
200 ml
If the volume of a fixed mass of gas is doubled while its temperature remains constant, what change will there be in its pressure?
The pressure will be halved.
The pressure remains the same.
The pressure will double.
The pressure will increase by four times.
The temperature of a fixed mass of gas increases from 100K to 400K. What will happen to its volume?
It will increase by a factor of four (four times its original volume).
It will decrease to a quarter of its original volume.
It will double.
It will stay the same.
If 4 litres of nitrogen gas at a temperature of 300K is expanded to 8 litres at the same pressure, what will the new temperature of the gas be?
600 K
150 K
300 K
37.5 K
A gas has a volume of 250 cm3 at a pressure of 100 kPa. What will the new volume of the gas be at a pressure of 200 kPa if the temperature remains constant?
125 cm3
500 cm3
150 cm3
2.5 cm3
An ideal gas occupies a volume V at an absolute temperature T. If the volume is halved and the pressure kept constant, what will happen to it's temperature?
It will halve to T/2.
It will increase to 2T.
It will remain the same.
It will increase to 3T.
A sample of air has a volume of 150 cm3 at a temperature of 57oC. At what temperature will this volume be 250 cm3?
277oC or 550 K.
4oC or 281 K.
95oC or 368 K.
198oC or 471 K.
The temperature of an ideal gas in a sealed container of volume V is increased from T to 3T. What will happen to the pressure, P of this gas?
It increases from P to 3P.
It decreases from P to P/3.
There is no change.
It increases from P to 2P.
Separate samples of methane and nitrogen gas have the same volume and each gas is at the same temperature and pressure. Which of the following statements is correct?
Both gases have the same number of molecules.
Each gas has the same mass.
The densities of both gases are the same.
Molecules of each gas have the same number of atoms.
A mole of a substance is defined as
the amount of substance that contains as many particles as there are in 12 grams of the C-12 isotope.
the amount of substance contained in 12 grams of carbon.
the amount of substance in 16 grams of oxygen.
the number of atoms in 12 grams of carbon.
The sum of the relative atomic masses of all the atoms in a molecule is known as
its relative molecular mass
the Avogadro number
a mole
its molar volume
One mole of a substance contains
6.0 x 1023 particles of that substance.
6.2 x 1032 particles of that substance.
6.23 x 10 particles of that substance.
10 x 623 particles of that substance.
The equation of state for an ideal gas is expressed as
PV = nRT
nPV = RT
P1V1 = P2V2
V/T = constant
For the chemical reaction shown, how many moles of NH3 are formed when 2 moles of N2 react with 8 moles of H2? N2 + 3H2 ⇌ 2NH3
4 moles
1 mole
3 moles
2 moles
How many atoms are there in 2.5 moles of Gold (Au)?
1.5 x 1024
1.5 x 1023
3.0 x 1023
3.0 x 1024
There are 3 x 1023 molecules in a sample of hydrogen (H2) gas. How many moles of H2 are there in this sample?
0.5 mole
3 moles
5 moles
0.3 mole
How many atoms are there in 1.5 moles of sulfur dioxide (SO2)?
2.7 x 1024
9.0 x 1023
9.0 x 1024
2.7 x 1023
If the molar volume of a gas at STP is 22.4 litres, how many moles are there in 112 litres of hydrogen gas?
5 moles
10 moles
2 moles
20 moles
The average mass of a molecule of a substance relative to one-twelfth the mass of a carbon-12 atom is known as
the relative molecular mass.
the relative atomic mass.
a mole of a that substance.
the molar mass of that substance.
The mass in grams of a mole of a substance is known as
molar mass.
molar volume.
relative molecular mass.
a mole.
The relative atomic mass of hydrogen is 1, and that of oxygen is 16, and that of sulfur is 32. What is the relative molecular mass of sulfuric acid (H2SO4)?
98
49
66
96
There are 22,400 cm3 in a mole of any gas at STP. How many cm3 are there in 0.05 mole of a gas at STP?
1,120 cm3
112 cm3
44,800 cm3
448 cm3
The relative atomic masses of sodium, oxygen and hydrogen are 23, 16 and 1 respectively. How many grams are there in 0.5 mole of sodium hydroxide (NaOH)?
20 grams
40 grams
38 grams
17 grams.
Which one of the following instruments is used for determining the relative molecular mass of a substance?
Mass spectrometer
Hofmann voltameter
Cathode ray tube
Geiger-Muller tube
The molar mass of a substance is defined as
the mass in grams of 1 mole of that substance.
the mass in grams of 1 litre of that substance.
the number of moles in 1 litre of that substance.
the number of moles in 1 kilogram of that substance.
If Avogadro's Number is 6 x 1023, then how many atoms are there in 2.5 moles of hydrogen gas (H2)?
3.0 x 1024
3.0 x 1023
1.5 x 1023
1.5 x 1024
If the molar volume of methane (CH4) is 22,400 cm3 and its molar mass is 16 grams, then how many grams of methane are there in 112 cm3 of methane gas?
0.08 gram
0.8 gram
1400 grams
20 grams
What will the mass of 5,600 cm3 of nitrogen gas (N2) be at STP? {Mr(N2) = 28 and molar volume at stp = 22,400 cm3}
7 grams
14 grams
28 grams
112 grams
Which of the following expressions is that of the combined gas law?
Under what two conditions will a real gas behave like an ideal gas?
High temperature and low pressure.
Low temperature and low pressure.
High temperature and high pressure.
Low temperature and high pressure.
Which one of the following is NOT an assumption of the Kinetic Theory of Gases?
Van Der Waals forces exist between particles in a gas.
The average kinetic energy of the particles in a gas is proportional to its absolute temperature.
All collisions between particles in a gas are perfectly elastic.
The diameters of the gas particles are negligible compared to the distances between the particles.
A gas that obeys all of the assumptions of the Kinetic Theory of Gases under all conditions of temperature and pressure is known as
an ideal gas
a real gas
a diatomic gas
a Noble Gas
In the equation of state for an ideal gas, which term represents the Universal Gas Constant?
R
P
n
T
V
The temperature of 1 dm3 of a gas is increased from 2oC to 64oC at constant pressure. What is the new volume in dm3?C
1.2
1.3
1.6
2.0
gas sample occupies a volume V1 at a pressure P1 and a Kelvin temperature T1. What would be the temperature of the gas, T2, if both its pressure and volume are doubled?
T2 = 4T1
T2 = ½T1
T2 = T1
T2 = 2T1
What will happen to the volume of a fixed mass of gas if the pressure and the Kelvin temperature are both doubled?
It will remain the same.
It will be double its initial volume.
It will be one-half its initial volume.
It will be four times its initial volume.
A cylinder of gas is at a pressure of 40 kPa. The volume and temperature (in K) are both doubled. What is the pressure of the gas after these changes?
40 kPa
10 kPa
20 kPa
80 kPa
For which set of conditions does a fixed mass of an ideal gas have the greatest volume?
High temperature and low pressure
Low temperature and high pressure
High temperature and high pressure
Low temperature and low pressure
The temperature in Kelvin of 2.0 dm3 of an ideal gas is doubled and its pressure is increased by a factor of four. What is the final volume of the gas?
1.0 dm3
2.0 dm3
3.0 dm3
4.0 dm3
Which change in conditions would increase the volume of a fixed mass of gas?
Halve the pressure and double the temperature
Halve the pressure and halve the temperature
Double the pressure and halve the temperature
Double the pressure and double the temperature
In gas laws, the conditions of S.T.P. are
0 °C and 1 atm pressure.
0 °C and 76 mm Hg pressure.
25 °C and 1 atm pressure.
25 °C and 76 mm Hg pressure.
According to Dalton’s Law of Partial Pressure, in a mixture of gases each gas
exerts a pressure equal to the pressure it would exert if it alone occupied the total volume.
exerts a pressure equal to the total pressure of the mixture.
The graph shows the volume left in a glass container after 60 ml of hydrogen chloride gas reacts with 40 ml of ammonia gas. 
