Try this as often as you like.

You will get a different set of questions each time you attempt this quiz.

You will get a different set of questions each time you attempt this quiz.

- In the experiment showing the diffusion between ammonia (NH
_{3}) 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

NH_{3}+ HCl → NH_{4}Cl

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 (O
_{2}). What volume of carbon dioxide (CO_{2}) is formed?

2CO + O_{2}→ 2CO_{2}- 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 cm
^{3}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 cm
^{3} - 500 cm
^{3} - 150 cm
^{3} - 2.5 cm
^{3}

- 125 cm
- 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 cm
^{3}at a temperature of 57^{o}C. At what temperature will this volume be 250 cm^{3}?- 277
^{o}C or 550 K. - 4
^{o}C or 281 K. - 95
^{o}C or 368 K. - 198
^{o}C or 471 K.

- 277
- 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 10
^{23}particles of that substance. - 6.2 x 10
^{32}particles of that substance. - 6.23 x 10 particles of that substance.
- 10 x 6
^{23}particles of that substance.

- 6.0 x 10
- The equation of state for an ideal gas is expressed as
- PV = nRT
- nPV = RT
- P
_{1}V_{1}= P_{2}V_{2} - V/T = constant

- For the chemical reaction shown, how many moles of NH
_{3}are formed when 2 moles of N_{2}react with 8 moles of H_{2}?

N_{2}+ 3H_{2}⇌ 2NH_{3}- 4 moles
- 1 mole
- 3 moles
- 2 moles

- How many atoms are there in 2.5 moles of Gold (Au)?
- 1.5 x 10
^{24} - 1.5 x 10
^{23} - 3.0 x 10
^{23} - 3.0 x 10
^{24}

- 1.5 x 10
- There are 3 x 10
^{23}molecules in a sample of hydrogen (H_{2}) gas.

How many moles of H_{2}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 (SO
_{2})?- 2.7 x 10
^{24} - 9.0 x 10
^{23} - 9.0 x 10
^{24} - 2.7 x 10
^{23}

- 2.7 x 10
- 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 (H
_{2}SO_{4})?- 98
- 49
- 66
- 96

- There are 22,400 cm
^{3}in a mole of any gas at STP. How many cm^{3}are there in 0.05 mole of a gas at STP?- 1,120 cm
^{3} - 112 cm
^{3} - 44,800 cm
^{3} - 448 cm
^{3}

- 1,120 cm
- 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 10
^{23}, then how many__atoms__are there in 2.5 moles of hydrogen gas (H_{2})?- 3.0 x 10
^{24} - 3.0 x 10
^{23} - 1.5 x 10
^{23} - 1.5 x 10
^{24}

- 3.0 x 10
- If the molar volume of methane (CH
_{4}) is 22,400 cm^{3}and its molar mass is 16 grams, then how many grams of methane are there in 112 cm^{3}of methane gas?- 0.08 gram
- 0.8 gram
- 1400 grams
- 20 grams

- What will the mass of 5,600 cm
^{3}of nitrogen gas (N_{2}) be at STP?

{M_{r}(N_{2}) = 28 and molar volume at stp = 22,400 cm^{3}}- 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 dm
^{3}of a gas is increased from 2^{o}C to 64^{o}C at constant pressure.

What is the new volume in dm^{3}?C- 1.2
- 1.3
- 1.6
- 2.0

- gas sample occupies a volume V
_{1}at a pressure P_{1}and a Kelvin temperature T_{1}.

What would be the temperature of the gas, T_{2}, if both its**pressure**and**volume**are doubled?- T
_{2}= 4T_{1} - T
_{2}= ½T_{1} - T
_{2}= T_{1} - T
_{2}= 2T_{1}

- T
- 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 dm
^{3}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 dm
^{3} - 2.0 dm
^{3} - 3.0 dm
^{3} - 4.0 dm
^{3}

- 1.0 dm
- 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.
- exerts only a fraction of its normal pressure.
- exerts the same pressure as each other gas.