4. The gaseous state

Question 1

Boyle’s Law formula?
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Hint: Volume proportional to?

Answer 1

V = k/p
Volume = Constant x Pressure
When temperature is constant

Question 2

For a given amount of gas under two different sets of conditions at constant temperature, what is the formula?

Answer 2

p1 x V1 = p2 x V2

Question 3

Charles’s Law (Gay-Lussac’s Law) formula?
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Hint: Volume proportional to?

Answer 3

V/T = k
Volume / Temperature = Constant
When pressure is constant

Question 4

For a given amount of gas under two different sets of conditions at constant pressure, what is the formula?

Answer 4

V1 / T1 = V2 / T2

Question 5

How to convert Celsius into Kelvin?

Answer 5

Temperature (Kelvin) = Temperature (In celcius) + 273

Question 6

Avogradro’s Law formula?
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Hint: Volume proportional to?

Answer 6

V = N
Volume = Number of particles
Under the same conditions of temperature, pressure, volumes of all gases.

Question 7

What is the Ideal gas equation formula?
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Hint: Made up of Boyle, Charles, Avogadro Laws.

Answer 7

V = ( n x T ) / p
pV = nRT
Where R is the molar gas constant

Question 8

Define Dalton’s Law of Partial Pressures?

Answer 8

In a mixture of gases that do not react with one another, each gas behaves as if it were the only gas present.
At constant volume and temperature.

Question 8

For an ideal gas at constant V and T, p (partial pressure) of gas A is directly proportional to n (amount of molecules). Hence, what is the formula for an ideal gas?

Answer 8

pA / Ptotal = nA / ntotal
partial pressure A / pressure total = amount of molecules A / total amount of molecules

Question 9

The kinetic molecular theory of gases assumes that…
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Hint: 4 points

Answer 9

1) Gas molecules behave as rigid spheres
2) There are no intermolecular forces between the gas molecules
3) Collisions between the gas molecules are perfectly elastic hence, no loss of kinetic energy during collisions
4) Gas molecules have no volume

Question 10

Explain gas pressure within a container occurs.

Answer 10

Gas molecules are in constant random motion within the container the gas is in and collide with the walls of the container. They exert a force which results in pressure.

Question 11

Explain boyle’s law in relation to behaviour of gases within a container.

Answer 11

When volume of the gas decreases, distance between gas molecules and the wall of the container decrease. Hence, the molecules collide more often with the walls, leading to greater pressure being exerted by the gas.

Question 12

Explain Charles’ Law in relation to behaviour of gases within a container.

Answer 12

When temperature of the gas increase, the gas molecules have higher kinetic energy and move faster. They hit the walls of the container more frequently and at a greater force, leading to a greater pressure being exerted by the gas.

Question 13

Explain Dalton’s law of partial pressure in relation to behaviour of gases within a container.

Answer 13

The pressure exerted by the gas depends on the number of collisions per second, which is proportional to the number of gas molecules present.