Study of Gas Laws

Questions

Question 1(1988)

"When stating the volume of a gas the pressure and temperature should also be given". Why ?

Answer

The change in any one of the parameters [pressure, volume, temperature] affects the other two parameters. Therefore, when stating the volume of a gas the pressure and temperature should also be given.

Question 1(1989)

Define or state : Boyle's Law

Answer

Temperature remaining constant, the volume of a given mass of dry gas is inversely proportional to it's pressure.

V ∝ $\dfrac{1}{\text{P}}$ [T = constant]

Question 1(1990)

State : Boyle's Law

Answer

Temperature remaining constant, the volume of a given mass of dry gas is inversely proportional to it's pressure.

V ∝ $\dfrac{1}{\text{P}}$ [T = constant]

Question 2(1990)

Express Kelvin Zero in °C

Answer

Kelvin zero or absolute zero = -273°C.

Question 1(1992)

A fixed volume of a gas occupies 760 cm³ at 27°C and 70 cm of Hg. What will be it's vol. at s.t.p.

Answer

Using gas laws:

$\dfrac{\text{P}_1{\text{V}_1}}{\text{T}_1}$ = $\dfrac{\text{P}_2{\text{V}_2}}{\text{T}_2}$

Substituting the values:

$\dfrac{70 \times 760}{300}$ = $\dfrac{76 \times {\text{V}_2}}{273}$

Therefore:

$\text{V}_2 =\dfrac{70 \times 760 \times 273}{300 \times 76} = 637 \text{cm}^3$

Therefore, the volume occupied by the gas is 637 cm³.

Question 1(1993)

State : Boyle's Law

Answer

Temperature remaining constant the volume of a given mass of dry gas is inversely proportional to it's pressure.

V ∝ $\dfrac{1}{\text{P}}$ [T = constant]

Question 1(1995)

At 0°C and 760 mm Hg pressure, a gas occupies a volume of 100 cm³. The Kelvin temperature (Absolute temperature) of the gas is increased by one-fifth while the pressure is increased one and a half times. Calculate the final volume of the gas.

Answer

Initial conditions [S.T.P.] :

P₁ = Initial pressure of the gas = 760 mm Hg
V₁ = Initial volume of the gas = 100 cm³
T₁ = Initial temperature of the gas = 0°C = 273 K

Final conditions:

P₂ (Final pressure) = increased one and a half times of P₁
= (1 + $\dfrac{1}{2}$) of 760
= $\dfrac{3}{2}$ x 760
= 3 x 380
= 1140
V₂ (Final volume) = ?
T₂ (Final temperature) = increased by one-fifth of 273 K = 1 + $\dfrac{1}{5}$ of 273
= $\dfrac{6}{5}$ x 273 = $\dfrac{1638}{5}$

By Gas Law:

$\dfrac{\text{P}_1\times\text{V}_1}{\text{T}_1} = \dfrac{\text{P}_2\times\text{V}_2}{\text{T}_2}$

Substituting the values :

$\dfrac{760 \times 100 }{273} = \dfrac{1140 \times \text{V}_2}{\dfrac{1638}{5}} \\[1em] \dfrac{760 \times 100 }{273} = \dfrac{5 \times 1140 \times \text{V}_2}{1638} \\[1em] \text{V}_2 = \dfrac{760 \times 100 \times 1638}{273 \times 5 \times 1140} \\[1em] \text{V}_2 = 80 \text{cc}$

Therefore, final volume of the gas = 80 cc

Question 1(1996)

The pressure on one mole of gas at s.t.p. is doubled and the temperature is raised to 546 K. What is the final volume of the gas ? [one mole of a gas occupies a volume of 22.4 litres at stp.]

Answer

Initial conditions [S.T.P.] :

P₁ = Initial pressure of the gas = 1 atm
V₁ = Initial volume of the gas = 22.4 litres
T₁ = Initial temperature of the gas = 273 K

Final conditions:

P₂ (Final pressure) = 2 atm
V₂ (Final volume) = ?
T₂ (Final temperature) = 546 K

By Gas Law:

$\dfrac{\text{P}_1\times\text{V}_1}{\text{T}_1} = \dfrac{\text{P}_2\times\text{V}_2}{\text{T}_2}$

Substituting the values :

$\dfrac{1 \times 22.4}{273} = \dfrac{2\times \text{V}_2}{546}\\[0.5em] \text{V}_2 = \dfrac{1 \times 22.4\times 546}{273\times 2} \\[0.5em] \text{V}_2 = 22.4 \text{ lit}$

Therefore, final volume of the gas = 22.4 lit.

Question 1(1997)

Is it possible to change the temperature and pressure of a fixed mass of gas without changing it's volume. Explain your answer.

Answer

No, it is not possible. Change in any one of the parameters [pressure, volume, temperature] affects the other two parameters.

Additional Questions

Question 1

What volume will a gas occupy at 740 mm pressure which at 1480 mm occupies 500 cc ? [Temperature being constant]

Answer

V₁ = Initial volume of the gas = 500 cc
P₁ = Initial pressure of the gas = 1480 mm

P₂ = Final pressure of the gas = 740 mm
V₂ = Final volume of the gas = ?

By Boyle's Law:

$\text{P}_1 \text{V}_1 = \text{P}_2 \text{V}_2$

Substituting the values :

$1480 \times 500 = \text{V}_2 \times 740 \\[0.5em] \text{V}_2 = \dfrac{1480 \times 500}{740} \\[0.5em] \text{V}_2 = 1000 \text{ cc}$

Therefore, final volume of the gas = 1000 cc

Question 2

The volume of a given mass of a gas at 27°C is 100 cc. To what temperature should it be heated at the same pressure so that it will occupy a volume of 150 cc ?

Answer

V₁ = Initial volume of the gas = 100 cc
T₁ = Initial temperature of the gas = 27°C = 27 + 273 = 300 K

V₂ = Final volume of the gas = 150 cc
T₂ = Final temperature of the gas = ?

By Charles's Law:

$\dfrac{\text{V}_1}{\text{T}_1} = \dfrac{\text{V}_2}{\text{T}_2}$

Substituting the values :

$\dfrac{100}{300} = \dfrac{150}{\text{T}_2} \\[0.5em] \text{T}_2 = 150 \times 3 = 450 \text{K}$

T₂ in °C = 450 - 273 = 177°C

Therefore, final temperature of the gas = 177°C

Question 3

A fixed mass of a gas has a volume of 750 cc at -23°C and 800 mm pressure. Calculate the pressure for which it's volume will be 720 cc. The temperature being -3°C.

Answer

By Gas Law:

$\dfrac{\text{P}_1\times\text{V}_1}{\text{T}_1} = \dfrac{\text{P}_2\times\text{V}_2}{\text{T}_2}$

Substituting the values :

$\dfrac{800 \times 750}{250} = \dfrac{\text{P}_2 \times 720}{270} \\[1em] \text{P}_2 = \dfrac{800 \times 750 \times 270}{250 \times 720} \\[1em] \text{P}_2 = 900 \text{ mm}$

Therefore, final pressure of the gas = 900 mm

Question 4

What temperature would be necessary to double the volume of a gas initially at s.t.p. if the pressure is decreased by 50% ?

Answer

By Gas Law:

$\dfrac{\text{P}_1\times\text{V}_1}{\text{T}_1} = \dfrac{\text{P}_2\times\text{V}_2}{\text{T}_2}$

Substituting the values :

$\dfrac{1\times \text{V}}{273} = \dfrac{0.5\times\text{2\text{V}}}{\text{T}_2} \\[0.5em] \text{T}_2 = 0.5\times 2 \times 273\\[0.5em] \text{T}_2 = 273\text{K}$

Therefore, final temperature of the gas = 273 K = 0 °C

Question 5

A gas cylinder having a capacity of 20 litres contains a gas at 100 atmos. How many flasks of 200 cm³ capacity can be filled from it at 1 atmos. pressure if the temperature remains constant ?

Answer

V₁ = 20 lits.

1 lit. = 1000 cc Therefore, 20 lit = 20,000 cc

P₁ (Initial pressure) = 100 atmos.

P₂ (Final pressure) = 1 atmos.

V₂ = ?

By Boyle's Law:

$\text{P}_1 \text{V}_1 = \text{P}_2 \text{V}_2$

Substituting the values :

$100 \times 20,000 = 1 \times \text{V}_2 \\[0.5em] \text{V}_2 = 20,00,000 \text{ cc}$

200 cc = capacity of 1 flask
Therefore, number of flasks required for 20,00,000 cc of gas

$= \dfrac{20,00,000 }{200} = 10,000$

Therefore, number of flask that can be filled = 10,000

Question 6

A certain mass of gas occupied 850 ml at a pressure of 760 mm of Hg. On increasing the pressure it was found that the volume of the gas was 75% of it's initial value. Assuming constant temperature, find the final pressure of the gas?

Answer

V₁ = Initial volume of the gas = 850 ml
P₁ = Initial pressure of the gas = 760 mm of Hg

V₂ (Final volume) = 75% of initial 850 ml = $\dfrac{75}{100}$ of 850 atm. = $\dfrac{3 \times 850}{4}$
P₂ = Final pressure of the gas = ?

By Boyle's Law:

$\text{P}_1 \text{V}_1 = \text{P}_2 \text{V}_2$

Substituting the values :

$760 \times 850 = \dfrac{\text{P}_2 \times 3 \times 850}{4} \\[1em] \text{P}_2 = \dfrac{760 \times 4}{3} \\[1em] \text{P}_2 = 1013.33 \text{ mm of Hg}$

Therefore, final pressure of the gas = 1013.33 mm of Hg.

Question 7

It is required to reduce the volume of a gas by 20% by compressing it at a constant pressure. To do so, the gas has to be cooled. If the gas attains a final temperature of 157°C, find the initial temperature of the gas ?

Answer

Initial conditions:

V₁ = Initial volume of the gas = V
T₁ = Initial temperature of the gas = ?

Final conditions

V₂ (Final volume) = reduce by 20%

= V - $\dfrac{20}{100}$ of V

= $\dfrac{80\text{V}}{100}$

= $\dfrac{4\text{V}}{5}$

T₂ = Final temperature of the gas = 157°C = 157 + 273 = 430 K

By Charles Law:

$\dfrac{\text{V}_1}{\text{T}_1} = \dfrac{\text{V}_2}{\text{T}_2}$

Substituting the values :

$\dfrac{\text{V}}{\text{T}_1} = \dfrac{\dfrac{4\text{V}}{5}}{430} \\[1em] \dfrac{\text{1}}{\text{T}_1} = \dfrac{4}{5 \times 430} \\[1em] \text{T}_1= \dfrac{430 \times 5}{4} \\[1em] \text{T}_1 = 537.5 \text{K}$

Therefore, final temperature of the gas = 537.5 K - 273 K = 264.5°C

Question 8

At a given temperature the pressure of a gas reduces to 75% of it's initial value and the volume increases by 40% of it's initial value. Find this temperature if the initial temperature was -10°C.

Answer

Initial conditions :

P₁ = Initial pressure of the gas = P
V₁ = Initial volume of the gas = V
T₁ = Initial temperature of the gas = -10°C = 273-10 = 263 K

Final conditions:

P₂ = Final pressure of the gas = reduces to 75% of P = $\dfrac{75}{100}$ of P = $\dfrac{3}{4}\text{P}$

V₂ = Final volume of the gas = increases by 40% of it's initial value

$= \dfrac{40}{100} \text{ of V + V} \\[1em] = \dfrac{4\text{V}}{10} + \text{V} \\[1em] = \dfrac{4\text{V + 10\text{V}}}{10} \\[1em] = \dfrac{14\text{V}}{10}$

T₂ = Final temperature of the gas = ?

By Gas Law:

$\dfrac{\text{P}_1\times\text{V}_1}{\text{T}_1} = \dfrac{\text{P}_2\times\text{V}_2}{\text{T}_2}$

Substituting the values :

$\dfrac{\text{P} \times \text{V}}{263} = \dfrac{\dfrac{3}{4}\text{P} \times\dfrac{14\text{V}}{10}}{\text{T}_2} \\[0.5em] \text{T}_2 = \dfrac{3}{4} \times\dfrac{14}{10} \times 263 \\[0.5em] \text{T}_2 = 276.15 \text{K}$

Therefore, final temperature of the gas = 276.15 K - 273 K = 3.15 °C

Unit Test Paper 7 — Study of Gas Laws

Question 1

Name or state the following :

1. The law which states that pressure remaining constant the volume of a given mass of dry gas is directly proportional to it's absolute [Kelvin] temperature.
2. The law which studies the relationship between pressure of a gas and the volume occupied by it at constant temperature.
3. An equation used in chemical calculations which gives a simultaneous effect of changes of temperature and pressure on the volume of a given mass of dry gas.
4. The standard pressure of a gas in cm. of mercury corresponding to one atmospheric pressure.
5. The absolute temperature value corresponding to 35°C.

Answer

1. Charle's Law.
2. Boyle's Law.
3. Gas equation.
4. 76 cm.
5. 35 + 273 = 308K

Question 2.1

Give reasons for the following :

Gases unlike solids and liquids exert pressure in all directions.

Answer

The force of attraction between the molecules is negligible in case of gases. The molecules of a gas move in straight lines, undergo random collision with other molecules and occupy the complete space available unlike solids and liquids. The impact of gas molecules with high velocity causes pressure to be exerted in all directions.

Question 2.2

Give reasons for the following :

Gases have lower densities compared to solids or liquids.

Answer

The inter-molecular distance between the molecules of gases is very large. Hence, the number of molecules per unit volume of a gas is much lower compared to solids and liquids. Gases therefore, have low densities.

Question 2.3

Give reasons for the following :

Temperature remaining constant the product of the volume & the pressure, of a given mass of dry gas is a constant.

Answer

Let a particular mass of a gas occupy

Volume = V; Pressure = P; At constant temperature = T

According to Boyle's Law:

$\text{V} ∝ \dfrac{1}{\text{P}} \text{ [T = constant]} \\[1em] \therefore \text{V} = \text{K} \dfrac{1}{\text{P}} \text{ [K is a constant]} \\[1em] \therefore \text{P}\text{V} = \text{K} = \text{constant}$

Hence, temperature remaining constant, the product of the volume & the pressure, of a given mass of dry gas is a constant.

Question 2.4

Give reasons for the following :

All temperatures on the Kelvin scale are in positive figures.

Answer

The lowest temperature on Kelvin scale is 0 K = -273°C. Practically, it is impossible for any gas to go below this temperature, as they solidify or liquify before reaching this temperature. Hence, all temperatures on the Kelvin scale are in positive figures.

Question 2.5

Give reasons for the following :

Volumes of gases are converted into s.t.p. conditions and then compared.

Answer

Volumes of gases change with temperature and pressure – hence a standard value of temperature and pressure is chosen to which gas volumes are referred. Hence, volumes of gases are converted into s.t.p. conditions and then compared.

Question 3.1

Calculate the temperature to which a gas must be heated, so that the volume triples without any change in pressure. The gas is originally at 57°C and having a volume 150 cc.

Answer

V₁ = Initial volume of the gas = 150 cc
T₁ = Initial temperature of the gas = 57°C = 57 + 273 = 330 K

V₂ = Final volume of the gas = 3 x 150 = 450 cc
T₂ = Final temperature of the gas = ?

By Charles's Law:

$\dfrac{\text{V}_1}{\text{T}_1} = \dfrac{\text{V}_2}{\text{T}_2}$

Substituting the values :

$\dfrac{150}{330} = \dfrac{450}{\text{T}_2} \\[1em] \text{T}_2 = \dfrac{450 \times 11}{5} = 990 \text{K}$

T₂ °C = 990 - 273 = 717°C

Therefore, final temperature of the gas = 717°C

Question 3.2

A gas 'X' at -33°C is heated to 127°C at constant pressure. Calculate the percentage increase in the volume of the gas.

Answer

V₁ = Initial volume of the gas = V cc
T₁ = Initial temperature of the gas = -33°C = -33 + 273 = 240 K

T₂ = Final temperature of the gas = 127°C = 127 + 273 = 400 K
V₂ = Final volume of the gas = ?

By Charles's Law:

$\dfrac{\text{V}_1}{\text{T}_1} = \dfrac{\text{V}_2}{\text{T}_2}$

Substituting the values :

$\dfrac{\text{V}}{240} = \dfrac{\text{V}_2}{400} \\[1em] \text{V}_2 = \dfrac{400 \times \text{V}}{240} \\[1em] \text{V}_2 = \dfrac{5\times \text{V}}{3}$

Increase in vol. = $\dfrac{5\text{V}}{3}$ - V = $\dfrac{2\text{V}}{3}$

Percentage increase in vol. = $\dfrac{\text{Increase}}{\text{Original}}$ x 100 = $\dfrac{2\text{V}}{3\text{V}}$ x 100 = 66.67%

Therefore, percentage increase in the volume of the gas = 66.67 %

Question 3.3

Calculate the volume of a gas A at s.t.p., if at 37°C and 775 mm of mercury pressure, it occupies a volume of $9\dfrac{1}{2}$ litres.

Answer

By Gas Law:

$\dfrac{\text{P}_1\times\text{V}_1}{\text{T}_1} = \dfrac{\text{P}_2\times\text{V}_2}{\text{T}_2}$

Substituting the values :

$\dfrac{775\times 9.5}{310} = \dfrac{760\times\text{\text{V}}_2}{273} \\[0.5em] \text{V}_2 =\dfrac{775\times 9.5\times 273}{310\times 760} \\[0.5em] \text{V}_2 = \dfrac{20,09,962.5}{2,35,600} \\[0.5em] \text{T}_2 = 8.53125 \text{ lit.}$

Therefore, final volume of the gas = 8.5312 lit

Question 3.4

Calculate the temperature at which a gas A at 20°C having a volume of 500 cc. will occupy a volume of 250 cc.

Answer

V₁ = Initial volume of the gas = 500 cc
T₁ = Initial temperature of the gas = 20°C = 20 + 273 = 293 K

T₂ = Final temperature of the gas = ?
V₂ = Final volume of the gas = 250 cc

By Charles's Law:

$\dfrac{\text{V}_1}{\text{T}_1} = \dfrac{\text{V}_2}{\text{T}_2}$

Substituting the values :

$\dfrac{500}{293} = \dfrac{250}{\text{T}_2} \\[0.5em] \text{T}_2 = \dfrac{293}{2} \\[0.5em] \text{V}_2 = 146.5\text{ K}$

Final temperature in °C = 146.5 - 273 = -126.5°C

Question 3.5

A gas X is collected over water at 17°C and 750 mm. pressure. If the volume of the gas collected is 50 cc., calculate the volume of the dry gas at s.t.p. [at 17°C the vapour pressure is 14 mm.]

Answer

By Gas Law:

$\dfrac{\text{P}_1\times\text{V}_1}{\text{T}_1} = \dfrac{\text{P}_2\times\text{V}_2}{\text{T}_2}$

Substituting the values :

$\dfrac{736\times 50}{290} = \dfrac{760\times\text{\text{V}}_2}{273} \\[1em] \text{V}_2 =\dfrac{736\times 50 \times 273}{290\times 760} \\[1em] \text{V}_2 =\dfrac{1,00,46,400}{2,20,400} \\[1em] \text{V}_2 = 45.58 \text{ cc.}$

Therefore, final volume of the gas = 45.58 cc

Question 4.1

Assuming temperature remaining constant calculate the pressure of the gas :

The pressure of a gas having volume 1000 cc. originally occupying 1500 cc. at 720 mm. pressure.

Answer

V₁ = Initial volume of the gas = 1500 cc
P₁ = Initial pressure of the gas = 720 mm

V₂ (Final volume) = 1000 cc
P₂ = Final pressure of the gas = ?

By Boyle's Law:

$\text{P}_1 \text{V}_1 = \text{P}_2 \text{V}_2$

Substituting the values :

$720 \times 1500 = 1000 \times \text{P}_2 \\[1em] \text{P}_2 = \dfrac{720 \times 1500 }{1000} \\[1em] \text{P}_2 = 1080 \text{ mm }$

Therefore, final pressure of the gas = 1080 mm.

Question 4.2

Assuming temperature remaining constant calculate the pressure of the gas :

The pressure of a gas having volume 100 lits. originally occupying 75 dm³ at 700 mm. pressure.

Answer

V₁ = Initial volume of the gas = 75 dm³
As 1 dm³ = 1 lit, hence, 75 dm³ = 75 lit
P₁ = Initial pressure of the gas = 700 mm

V₂ (Final volume) = 100 lit.
P₂ = Final pressure of the gas = ?

By Boyle's Law:

$\text{P}_1 \text{V}_1 = \text{P}_2 \text{V}_2$

Substituting the values :

$700 \times 75 = 100 \times \text{P}_2 \\[0.5em] \text{P}_2 = \dfrac{700 \times 75 }{100} \\[0.5em] \text{P}_2 = 525 \text{ mm }$

Therefore, final pressure of the gas = 525 mm.

Question 4.3

Assuming temperature remaining constant calculate the pressure of the gas :

The pressure of a gas having volume 380 lits. originally occupying 800 cm³ at 76 cm. pressure.

Answer

V₁ = Initial volume of the gas = 800 cm³
P₁ = Initial pressure of the gas = 76 cm

V₂ (Final volume) = 380 lit.
As 1 lit. = 1000 cm³, hence, 380 lit. = 3,80,000 cm³
P₂ = Final pressure of the gas = ?

By Boyle's Law:

$\text{P}_1 \text{V}_1 = \text{P}_2 \text{V}_2$

Substituting the values :

$800 \times 76 = 3,80,000 \times \text{P}_2 \\[0.5em] \text{P}_2 = \dfrac{800 \times 76 }{3,80,000 } \\[0.5em] \text{P}_2 = 0.16 \text{ cm}$

Therefore, final pressure of the gas = 0.16 cm.

Question 4.4

Assuming temperature remaining constant calculate the pressure of the gas :

The pressure of a gas having volume 1800 ml. originally occupying 300 ml. at 6 atms. pressure.

Answer

V₁ = Initial volume of the gas = 300 ml
P₁ = Initial pressure of the gas = 6 atmos.

V₂ (Final volume) = 1800 ml
P₂ = Final pressure of the gas = ?

By Boyle's Law:

$\text{P}_1 \text{V}_1 = \text{P}_2 \text{V}_2$

Substituting the values :

$6 \times 300 = \text{P}_2 \times 1800 \\[0.5em] \text{P}_2 = \dfrac{1800 }{1800} \\[0.5em] \text{P}_2 = 1\text{ atm. }$

Therefore, final pressure of the gas = 1 atm.

Question 4.5

Assuming temperature remaining constant calculate the pressure of the gas :

The pressure of a gas having volume 1500 cm³ originally occupying 750 cc. at 5 atms. pressure.

Answer

V₁ = Initial volume of the gas = 750 cc
P₁ = Initial pressure of the gas = 5 atms.

V₂ (Final volume) = 1500 cc
P₂ = Final pressure of the gas = ?

By Boyle's Law:

$\text{P}_1 \text{V}_1 = \text{P}_2 \text{V}_2$

Substituting the values :

$5 \times 750 = \text{P}_2 \times 1500 \\[0.5em] \text{P}_2 = \dfrac{5 \times 750}{1500} \\[0.5em] \text{P}_2 = 2.5 \text{ atms }$

Therefore, final pressure of the gas = 2.5 atms.

Question 5.1

Calculate the following :

The temp, at which 500 cc. of a gas 'X' at temp. 293K occupies half it's original volume [pressure constant].

Answer

V₁ = Initial volume of the gas = 500 cc
T₁ = Initial temperature of the gas = 293 K

T₂ = Final temperature of the gas = ?
V₂ = Final volume of the gas = 250 cc

By Charles's Law:

$\dfrac{\text{V}_1}{\text{T}_1} = \dfrac{\text{V}_2}{\text{T}_2}$

Substituting the values :

$\dfrac{500}{293} = \dfrac{250}{\text{T}_2} \\[0.5em] \text{T}_2 = \dfrac{293}{2} \\[0.5em] \text{V}_2 = 146.5\text{ K}$

Final temperature in °C = 146.5 - 273 = -126.5°C

Question 5.2

Calculate the following :

The volume at s.t.p. occupied by a gas 'Y' originally occupying 760 cc. at 300 K and 70 cm. press, of Hg.

Answer

By Gas Law:

$\dfrac{\text{P}_1\times\text{V}_1}{\text{T}_1} = \dfrac{\text{P}_2\times\text{V}_2}{\text{T}_2}$

Substituting the values :

$\dfrac{70 \times 760}{300} = \dfrac{76\times\text{\text{V}}_2}{273} \\[1em] \text{V}_2 =\dfrac{760\times 70 \times 273}{300\times 76} \\[1em] \text{V}_2 = 637 \text{ cc.}$

Therefore, final volume of the gas = 637 cc.

Question 5.3

Calculate the following :

The volume at s.t.p. occupied by a gas 'Z' originally occupying 1.57 dm³ at 310.5 K and 75 cm. press. of Hg.

Answer

By Gas Law:

$\dfrac{\text{P}_1\times\text{V}_1}{\text{T}_1} = \dfrac{\text{P}_2\times\text{V}_2}{\text{T}_2}$

Substituting the values :

$\dfrac{75\times 1.57}{310.5} = \dfrac{76\times\text{\text{V}}_2}{273} \\[1em] \text{V}_2 =\dfrac{75\times 1.57 \times 273}{310.5\times 76} \\[1em] \text{V}_2 = 1.36 \text{ dm}^3$

Therefore, final volume of the gas = 1.36 dm³

Question 5.4

Calculate the following :

The volume at s.t.p. occupied by a gas 'Q' originally occupying 153.7 cm³ at 287 K and 750 mm. pressure [vapour pressure of gas 'Q' at 287 K is 12 mm of Hg.]

Answer

By Gas Law:

$\dfrac{\text{P}_1\times\text{V}_1}{\text{T}_1} = \dfrac{\text{P}_2\times\text{V}_2}{\text{T}_2}$

Substituting the values :

$\dfrac{738\times 153.7}{287} = \dfrac{760\times\text{\text{V}}_2}{273} \\[1em] \text{V}_2 =\dfrac{738\times 153.7 \times 273}{287\times 760} \\[1em] \text{V}_2 = 141.970 \text{ cm}^3$

Therefore, Final volume of the gas = 141.970 cm³

Question 5.5

Calculate the following :

The temperature to which a gas 'P' has to be heated to triple it's volume, if the gas originally occupied 150 cm³ at 330 K [pressure remaining constant].

Answer

V₁ = Initial volume of the gas = 150 cm³
T₁ = Initial temperature of the gas = 330 K

T₂ = Final temperature of the gas = ?
V₂ = Final volume of the gas = 3 x 150 cm³ = 450 cm³

By Charles's Law:

$\dfrac{\text{V}_1}{\text{T}_1} = \dfrac{\text{V}_2}{\text{T}_2}$

Substituting the values :

$\dfrac{150}{330} = \dfrac{450}{\text{T}_2} \\[0.5em] \text{T}_2 = \dfrac{450 \times 330}{150} \\[0.5em] \text{T}_2 = 990 \text{ K}$

Final temperature in °C = 990 - 273 = 717°C

Question 6

Fill in the blanks with the correct word, from the words in bracket :

1. If the temperature of a fixed mass of a gas is kept constant and the pressure is increased, the volume correspondingly .............. [increases/decreases]
2. If the pressure of a fixed mass of a gas is kept constant and the temperature is increased, the volume correspondingly .............. [increases/decreases]
3. 1 dm³ of a gas is equal to .............. [1 litre / 100 ml. / 100 cc.]
4. All the temperatures on the kelvin scale are in .............. figures [negative/positive]
5. At -273°C the volume of a gas is theoretically .............. [272 cc. / 0 cc. /274 cc.]

Answer

1. If the temperature of a fixed mass of a gas is kept constant and the pressure is increased, the volume correspondingly decreases.
2. If the pressure of a fixed mass of a gas is kept constant and the temperature is increased, the volume correspondingly increases.
3. 1 dm³ of a gas is equal to 1 litre.
4. All the temperatures on the kelvin scale are in positive figures.
5. At -273°C the volume of a gas is theoretically 0 cc.