Boyle's Law

Q.

Air at sea level is dense. This is a practical application of

1. Boyle's law

2. Dalton's law

3. Charle's law

4. Avogadro's law

Q. $I,II,III$ are three isotherms respectively at $T_1,T_2$ and $T_3$. The temperatures will be in the order:

1. $T_1=T_2=T_3$
2. $T_1<T_2<T_3$
3. $T_1>T_2>T_3$
4. $T_1>T_2=T_3$

Q. 46. 16g of O2 and 3g of H2 are mixed and kept at 760mm pressure and 273 K . The total volume occupied by mixture will nearly a. 22.4l b. 33.6l c. 448l d. 44800l

Q. The temperature at which intermolecular attractionforce balance the intermolecular repulsion force isknown as(1) Boyle temperature(2) Critical temperature3) Boiling temperature4) Equilibrium temperature

Q.

A gas occupies a volume of 300 cc at ${27}^{\circ }$C and 620 mm pressure. The volume of the gas at ${47}^{\circ }$C and 640 mm pressure is

1. 260cc

2. 310cc

3. 390cc

4. 450cc

Q. If there is no force of attraction between gas particles according to kinetic molecular theory postulates then how molecules of gases can collide without any force of attraction?

Q. Which of the following plots does not represent Boyle’s law?

1. 
2. 
3. 
4. 

Q. What is the equation for work done in isothermal and adiabatic process

Q. 20.An equilibrium mixture at 300K contains N2O4 and NO2 at 0.28 and 1.1 atm pressure respectively. If the volume of the container is doubled, calculate the new equilibrium pressure of two gases a)0.095, 0.64 b)0.95, 0.064 c)0.95, 0.64 d)0.95, 0.028

Q. a gas at 350 k and 15 bar has molar volume 20percent smaller than that for an ideal gas under the same condion, the z is?? which force is dominant?

Q.

According to the kinetic theory of gases, the effect of an increase in temperature on the distribution of molecular speeds is that

1. The most probable speed increases

2. The distribution becomes broader

3. The fraction of molecules, with most probable speed increases

4. Area under distribution curve remains the same as that of under lower temperature

Q. For a fixed amount of ideal gas, match the two Lists.

1. A - Q; B - P; C - R; D - S
2. A - S; B - R; C - S; D - R
3. A - Q; B - P; C - S; D - R
4. A - Q; B - S; C - R; D - Q

Q. 30 ton) of61 The intercept on y-axis and slope of curve plotted between P/T vs. TFor an ideal gas having 10 moles in a closed rigid container of volume 8.21 L (P Pressure inatm and T- Temp. in K, log 10 2-0.30)) are respectively:(a) 001, 0(b) 0.1, 0(c) 0.1, 1(d) 10. 1

Q. A cylinder contains 100 g of an ideal gas ( mol weight is 40g/ mol) at 27^° C and 2 atm pressure. In tranference process, the cylinder fell and a dent was created i.e. there was a decrease in the volume of cylinder. But valve attached to the cylinder cannot keep the presssure greater than 2 atm so 10 g of gas is leaked out.Calculate volume of the cylinder before dent in dm3

Q. 63.An ideal gas expands along the path AB as shown in the p-V diagram.The work done is

Q. If N${}_2$ gas is hubbled through water at 293 K, how many millimoles of N${}_2$ gas would dissolve in 1 litre of water? Assume that N${}_2$ exerts a partial pressure of 0.987 bar. Given that Henry's law constant for N${}_2$ at 293 K is 76.48 kbar.

1. $0.561$ mmol
2. $0.716$ mmol
3. $0.222$ mmol
4. $0.828$ mmol

Q. Why q is not equal to zero in an isothermal process?

Q. At what pressure will a quantity of gas which occupies 100 ml at a pressure of 720 mm ocupy a volume of 84 ml

Q. Calculate the concentration of $C{O}_2$ in a soft drint that is bottled at partial pressure of $C{O}_2$ of 4 atm over the liquid at ${25}^{o}C$. The Henry's law constant for $C{O}_2$ in water at ${25}^{o}C$ is $3.1\times {10}^{-2}$ mol/litr4e-atm.

Q. The diameter of a bubble at the surface of a lake is $4\text{mm}$ and at the bottom of the lake is $1\text{mm}$. If the atmospheric pressure is $1\text{atm}$ and the temperature of the lake and the atmosphere are equal, what is the depth of the lake?
(The density of the lake and mercury are $1\text{g/ml}$ and $13.6\text{g/ml}$ respectively. Ignore the surface tension)

1. $453\text{m}$
2. $651\text{m}$
3. $784\text{m}$
4. $102\text{m}$

Q. a mixture of N2and Ar gases in a cylinder contains 7g of N2 and 8gof Ar if the total pressure of the mixture of gases in the cylinder is 27 bar the partial pressure of N2 is

Q. Air contains 23 % oxygen and 77 nitrogen by weight . The percentage of O_2 by volume is

Q. What percent of a sample of nitrogen must be allowed to escape if its temperature, pressure and volume are to be changed from 220^{†extdegree⊂}, 3 atm and 1.65 litre to 110^{}, 0.7 atm and 1.00 litre respectively?

Q. If the solubility of any gas in the liquid at $1$ bar pressure is $0.05$ mol/L. What will be its solubility at $3$ bar pressure, keeping the temperature constant?

1. $\frac{0.05}{3}$ mol/L
2. $0.15$ mol/L
3. $0.05$ mol/L
4. $1.0$ mol/L

Q. Graph of pressure (P) vs volume (V) of a gas at different temperatures

The correct order of temperature will be

1. $T_1<T_2<T_3$
2. $T_1=T_2=T_3$
3. $T_1>T_2=T_3$
4. $T_1>T_2>T_3$

Q. volume at NTP of oxygen req. to completely burn 1kg of coa

Q. A $10.0\text{cm}$ column of air is trapped by a column of 4 cm long $Hg$ in a capillary tube of uniform bore when the tube is held horizontally at $1\text{atm}$. The length of the air column when the tube is held vertically with the open end up is:
Given: $P_{atm}=76$ cm of Hg

1. $3.53\text{cm}$
2. $10.52\text{cm}$
3. $9.50\text{cm}$
4. $4.61\text{cm}$

Q.

If pressure becomes double at the same absolute temperature on 2 L $C{O}_2$ , then the volume of $C{O}_2$

1. 2 L

2. 4 L

3. 25 L

4. 1 L

Q.

The following graph correctly reflects log P vs log $\left(\frac{1}{V}\right)$ for a finite amount of gas at a constant temperature - True or False?

1. True

2. False

Q. Equal volume of two gases which do not react together are enclosed in separate vessels. Their pressures are $10\text{mmHg}$ and $400\text{mmHg}$ respectively. If the two vessels are joined together, then what will be the pressure of the resulting mixture (temperature remaining constant)?

1. $125\text{mm}Hg$
2. $150\text{mm}Hg$
3. $410\text{mm}Hg$
4. $205\text{mm}Hg$