Real Gases

Q.

The normality of 4.9% (w/w) H2SO4 Solution having density 1.02 g / ml is ?

Q.

A real gas most closely approaches the behaviour of an ideal gas at

1. 15 atm and 200 K

2. 1 atm and 273 K

3. 0.5 atm and 500 K

4. 15 atm and 500 K

Q. Q. The max solubility of Ag2CO3 in 0.02M Na2CO3?{ksp=8x10^-12}

Q. Some amount of air is kept in an open container at 27 C. At what temperature the container be heated to eliminate 37.5% of air from the container?

Q. Vander Waal's constants 'a' and 'b' are related with..... respectively

1. Attractive force and bond energy of molecules
2. Volume and repulsive force of molecules
3. Shape and repulsive forces of molecules
4. Attractive force and volume of the molecules

Q. A gas such as carbon monoxide would be most likely to obey the ideal gas law at :

1. high temperature and high pressure
2. low temperature and low pressure
3. high temperature and low pressure
4. low temperature and high pressure

Q. Solubility of AgCl in 0.1M CaCl2 is

Q.

At extremely low pressure van der Waal’s equation can be expressed as

1. $(P+\frac{a{n}^2}{V^2})V=nRT$

2. $p(V-nb)=nRT$

3. $PV=nRT$

4. $Noneoftheabove$

Q. Calculate solubility product of Hg2Cl2 if its solubility at room temperature is 2.0*10^-3

Q. One mole of a real gas at its critical temperature has a relation between its pressure (in atm) and volume (in litres) as follows:
$P=\frac{2R{T}_c}{V}-\frac{3X}{V^2}+\frac{Y}{V^3}$
Where $T_c$ is the critical temperature (in K) and R is the gas constant while X and Y are some constants. Find the correct option(s) about the gas and its given relation.

1. The unit of the constant X is $atmL$
2. The unit of the constant Y is atm $atm{L}^3$
3. $T_c=\frac{3X^2}{2RY}$
4. At critical volume $\frac{dP}{dV}=0$

Q. 30. A solution of urea in water is labelled as 20% by weight. The molality of the solution is

Q.

Calculate the pressure of one mole of nitrogen gas in a 10 L cylinder at ${50}^{\circ }C$ using the Van der Waals equation.Also find the value of ideal gas pressure.(Van der Waals constants a and b for nitrogen are $1.4L^{2}atmmo{l}^{-2}and0.04L^{2}mo{l}^{-1}$ respectively) .

1. 2.18 atm

2. 2.965 atm

3. 2.652 atm

4. None of these

Q.

Calculate the pressure of one mole of nitrogen gas in a 10 L cylinder at ${50}^{\circ }C$ using the Van der Waal's equation.Also find the value of ideal gas pressure.(Van der Waal's constants a and b for nitrogen are $1.4L^{2}atmmo{l}^{-2}and0.04L^{2}mo{l}^{-1}$ respectively) .

1. 2.18 atm

2. 2.965 atm

3. 2.652 atm

4. None of these

Q. $50\text{ml}$ of a mixture of $N{H}_3$ and $H_2$ was completely decomposed by sparking into nitrogen and hydrogen. $40\text{ml}$ of oxygen was added and the mixture was sparked again. After cooling to the room temperature, the mixture was shaken with alkaline pyrogallol solution and a contraction of $6\text{ml}$ was observed. Calculate the % by volume of $N{H}_3$ in the original mixture.

1. 36%
2. 54%
3. 27%
4. 72%

Q. Two Gases X and Y have densities $d_x=3d_y$ and Molecular Masses , $M_x=0.5M_y$. Then, the ratio of their pressures, i.e. $P_x:P_y$ would be

1. 1/4

2. 1/6

3. 4

4. 6

Q. For an equilibrium rxn involving gases, the forward rxn is 1st order while reverse is second order rxn. the units of K_pare atm atm^2 atm^{-1} atm^-

Q.

Which of the following graphs correctly represents the variation of $\beta$ = - $(\frac{\frac{dV}{dP}}{V}{)}_{\gamma }$ with P for an ideal gas at constant temperature.

1. 

2. 

3. 

4. 

Q. $\begin{array}{cc}\text{Column -I}& \text{Column -II}\\ \left(A\right)P{V}^{(}\gamma )\text{Constant}& \text{(p)Expansion of ideal gas in vacuum}\\ \left(B\right)\Delta T=0& \text{(q)}Z=1-\frac{a}{V_{m}RT}\\ \text{(C) For}{H}_2\text{and He at}{0}^{\circ }C& \text{(r) Adiabatic reversible process}\\ \text{(C) At low density of gas}& \left(s\right)Z=1+\frac{pb}{RT}\end{array}$

1. $A\to R$, $B\to P$, $C\to S$, $D\to Q$
2. $A\to Q$, $B\to R$, $C\to S$, $D\to P$
3. $A\to P$, $B\to R$, $C\to S$, $D\to Q$
4. $A\to Q$, $B\to P$, $C\to S$, $D\to R$

Q. 27.If 200g of solution is removed from 500g of 20%(w/w) aqueous sugar solution and 20g more sugar is mixed in the remaining solution, find the concentration of the new solution?

Q.

Van der Waals’ equation explains the behavior of:

1. Ideal gases

2. Real gases

3. Only monoatomic gases

4. Only diatomic gases

Q.

In Van der Waals equation of state of the gas law, the constant b is a measure of__.

1. Intermolecular repulsions

2. Intermolecular collisions per unit volume

3. Volume occupied by the molecules

4. Intermolecular attractions

Q.

Van der waals constant "b" of helium is $24mLmo{l}^{-1}$. Find molecular diameter of helium.

1. 

2. 

3. 

4. 

Q. the solubility product of a sparingly soluble salt AX2 is 3.2*10^-11 its solubility

Q. The Vander wall's equation for $\left(\frac{1}{2}\right)$ mole of a gas?

1. $(P+\frac{a}{V^2})(V-b)=RT$
2. $(P+\frac{a}{4V^2})\left(\frac{V-b}{2}\right)=RT$
3. $(P+\frac{a}{4V^2})(V-\frac{b}{2})=\frac{RT}{2}$
4. $(P+\frac{a}{4V^2})\left(\frac{V-b}{2}\right)=2RT$

Q.

In Van der Waals equation of state of the gas law, the constant b is a measure of__.

1. Intermolecular repulstions

2. Intermolecular collisions per unit volume

3. Volume occupied by the molecules

4. Intermolecular attractions

Q. Which of the following is not true regarding Henry's law constant?

1. It has same unit as that of pressure
2. Different gas-liquid system have different $K_H$​
3. It decreases with increase in solubility
4. It decreases with increase in temperature

Q. The weight of silver $\text{(atomic wt.}=108)$ displaced by a quantity of electricity which displaces $5600mLof{O}_2$ at STP will be : -
(AIPMT-2014

1. $54.0g$
2. $10.8g$
3. $108g$
4. $5.4g$

Q. For a gas, the deviation from ideal behavior is maximum at:

1. $0^{\circ }\text{C and}1.0\text{atm}$
2. ${100}^{\circ }\text{C and}2.0\text{atm}$
3. $-{13}^{\circ }\text{C and}1.0\text{atm}$
4. $-{13}^{\circ }\text{C and}2.0\text{atm}$

Q. Which of the following is not true regarding Henry's law constant?

1. Different gas-liquid system have different $K_H$​
2. It decreases with increase in solubility
3. It decreases with increase in temperature
4. It has same unit as that of pressure

Q.

For the chemical equilibrium, $CaC{O}_3\left(s\right)\rightleftharpoons CaO\left(s\right)+C{O}_2\left(g\right),\Delta H^{.}$, can be determined from which one of the following plots

1. 

2. 

3. 

4.