Ideal Gas Law

Q.

Match the following graphs of ideal gas with their coordinates.

Q. When an ideal gas is compressed adiabatically and reversibly, the final temperature is:

1. higher than the initial temperature
2. lower than the initial temperature
3. the same as the initial temperature
4. dependent on the rate of compression

Q.

What is the difference between standard temperature and pressure and standard state?

Q.

100 ml of a gas occupies a pressure of 720 mm of Hg. At what pressure will the same gas occupy a volume of 84 ml?

1. 672 mm

2. 824 mm

3. 857 mm

4. 724 mm

Q. A stopcock connecting two bulbs of volume 10 litre and 5 litre containing an ideal gas at 6 atm and 9 atm respectively, is opened. What is the final pressure if the temperature remains the same?

1. 7 atm
2. 7.5 atm
3. 15 atm
4. 8 atm

Q. Pressure remaining constant, the volume of a fixed mass of a gas is directly proportional to its absolute temperature. This law is popularly known as :

1. Boyle's law
2. Charles' law
3. Gay Lusac's law
4. Avogadro law

Q. 1 mole of monoatomic ideal gas undergoes the following operation

Select the incorrect relation.

1. $T_E>T_D$
2. $T_D>T_C$
3. $T_B>T_D$
4. $T_B>T_C$

Q.

Two gas bulbs A and B are connected by a tube having a stop cock. Bulb A has a volume of 100 ml and contains $H_2$ . After stopcock is opened, $H_2$ from A travels to evacuated bulb B and the pressure falls to $40\%$. The volume of B in ml is –

1. 250 ml

2. 200 ml

3. 150 ml

4. 75 ml

Q. Two glass bulbs of equal volume are connected by a narrow tube and filled with a gas at $0^{\circ }C$ and pressure of $76cm$ of $Hg$. One of the bulb is then placed in a water bath maintained at ${62}^{\circ }C$. What is the new value of the pressure inside the bulbs? The volume of the connecting tube is negligible.

Q. The volume of a given mass of a gas is 300 ml, measured at 798 mm pressure. What will be the volume, if pressure is reduced to 760 mm at constant temperature?

1. 513 ml
2. 135 ml
3. 360 ml
4. 315 ml

Q. It is desired to increase the volume of $800c{m}^3$ of a gas by $20$% keeping the pressure constant. To what temperature should the gas be heated, if the initial temperature is ${22}^{\circ }C$?

Q. At constant temperature, the pressure of a fixed amount of gas is inversely proportional with its volume. This law is popularly known as :

1. Charle's law
2. Boyle's law
3. Gay Lussac's law
4. Avogadro's law

Q. The mass of $3.01\times {10}^{23}$ molecules of a gas iss $32.0g$. What volume does $8.00$ g of the gas occupy at STP?

1. $2.80L$
2. $8.00L$
3. $22.4L$
4. $11.2L$
5. $64.0L$

Q. A gas occupies a volume of $250$ ml at $745$ mm Hg and ${25}^{\circ }$C. What additional pressure is required to reduce the gas volume to $200$ ml at the same time?

1. $180.25$ mm
2. $200.9$ mm
3. $186.25$ mm
4. $189.4$ mm

Q. At what centigrade temperature will a given volume of a gas at $0^{\circ }$C becomes double if pressure remains constant?

1. ${546}^{\circ }$C
2. ${273}^{\circ }$C
3. ${200}^{\circ }$C
4. ${320}^{\circ }$C

Q. When an ideal gas is compressed adiabatically and reversibly, the final temperature is:

1. higher than the initial temperature
2. lower than the initial temperature
3. the same as the initial temperature
4. dependent on the rate of compression

Q. State whether the statement is true or false:

Q. The compressibility factor of gas is less than unity at STP, therefore:
(V${}_m$ is the molar volume)

1. V${}_m$ > 22.4 L
2. V${}_m$ < 22.4 L
3. V${}_m$ $=$ 44.8 L
4. V${}_m$ $=$ 22.4 L

Q. The density of ammonia at ${30}^{o}C$ and $5$ atm pressure is:

1. $3.42$ g/L
2. $2.42$ g/L
3. $1.171$g/L
4. $3.84$ g/L

Q. A balloon is filled with hydrogen at room temperature. It will burst if pressure exceeds $0.2$ bar.

1. $11.35$ L
2. $22.7$ L
3. $44.8$ L
4. $67.3$ L

Q. When 4.215 g of a metallic carbonate was heated in a hard glass tube, the $C{O}_2$ evolved was found to measure 1336 mL at ${27}^{\circ }C$ and 700 mm pressure. The equivalent weight of the metal(only integer part) is _______.

Q. $105$ mL of pure water at $4$${}^{o}C$ is saturated with $N{H}_3$ gas yielding a solution of density $0.9g{mL}^{-1}$ and containing $30\%$ $N{H}_3$ by mass. The volume (in litres) of $N{H}_3$ gas at $4$${}^{o}C$ and $775$ mm of Hg, which was used to saturate the water is (as the nearest integer) :

Q. The $pH$ of pure water at ${25}^{o}C$ and ${60}^{o}C$ are $7$ and $6.5$ respectively. $HCl$ gas is passed through water at ${25}^{o}C$ till the resulting $1$ litre solution aquires a $pH$ of $3$. Now $4\times {10}^{-3}$ mole of $NaCN$ are added into this solution. Also a fresh $0.1M$ $HCN$ solution has $pH$ $5.1936$. Now in the one part of solution obtained after addition of $NaCN$, one millimole of $NaOH$ are added and in the second part of this solution $0.5$ miili mole of $HCl$ are added.

1. $24.46mL$
2. $244.6mL$
3. $2.446mL$
4. $0.2446mL$

Q. When an ideal gas is compressed adiabatically and reversibly, the final temperature is:

1. higher than the initial temperature
2. lower than the initial temperature
3. the same as the initial temperature
4. dependent on the rate of compression

Q. A burette can accurately measure the volumes of a solution delivered.

1. True
2. False

Q. When $2$ g of gas A is introduced into an evacuated flask kept at ${25}^{o}C$, the pressure was found to be $1$ atm. If $3$ g of another gas B is then added to the same flask containing A, the pressure becomes $1.5$ atm. Assuming ideal behaviour, the ratio of molecular weights $(M_A:M_B)$ is :

1. 1:3
2. 2:3
3. 3:2
4. 3:1

Q.

One mole of a gas exhibiting ideal behavior is enclosed in vessel of 1 litre capacity and is placed in a reservoir at temperature T(K). The pressure recorded in a flask is 2 bar. If the pressure in the flask is to be changed to 1.5 bar, how many molecules of the gas must escape out from the vessel?

1. $12.5\%$
2. $6\%$
3. $25\%$
4. $30\%$

Q. A sample of neon gas is contained by a closed 5-liter vessel. The temperature of container is 25${}^o$C and pressure is 1.5 atmospheres (R is equal to 0.08 L atm/mol K).
Find the expressions which is equal to the molar quantity of gas in the sample?

1. $\frac{\left(1.5\right)\left(5.0\right)}{\left(0.08\right)\left(25\right)}$
2. $\frac{\left(0.08\right)\left(25\right)}{\left(1.5\right)\left(5.0\right)}$
3. $\frac{\left(1.5\right)\left(25\right)}{\left(0.08\right)\left(5.0\right)}$
4. $\frac{\left(0.08\right)\left(298\right)}{\left(1.5\right)\left(5.0\right)}$
5. $\frac{\left(1.5\right)\left(5.0\right)}{\left(0.08\right)\left(298\right)}$

Q. What volume of $N{O}_2$ gas at ${27}^{o}C$ and $1.0$ atm pressure would be produced?

1. $6.97$ L
2. $5.97$ L
3. $4.97$ L
4. $3.97$ L

Q. $0.303$ g of the organic compound in Duma's method on combustion gave $32.27$ ml of moist nitrogen at ${27}^{\circ }$C and at P mm of Hg pressure. The vapour pressure at ${27}^{\circ }$C is $21$ mm of Hg. Find the value of P.

1. $725$ mm of Hg
2. $746$ mm of Hg
3. $710$ mm of Hg
4. $760$ mm of Hg