Ideal Gas Equation

Q.

State Henrys law and mention some important applications?

Q.

An ideal gas expands isothermally from ${10}^{-3}{m}^3$ to ${10}^{-2}{m}^3$ at $300K$ against a constant pressure of ${10}^{5}N{m}^{-2}$. The work done on the gas is

Q.

The number of water molecules present in a drop of water (volume= 0.0018 ml) at room temperature is

Q.

How do gas laws apply to everyday life?

Q. The $K_{sp}$ of $A{g}_{2}Cr{O}_4,AgCl,AgBr\text{AgI}$ are respectively, $1.1\times {10}^{-12},1.8\times {10}^{-10},5.0\times {10}^{-13},8.3\times {10}^{-17}$. Which one of the following salts will precipitate last if $AgN{O}_3$ solution is added to the solution containing equal moles of $NaCl,NaBr,NaI\text{and}N{a}_{2}Cr{O}_4$?

1. $AgCl$
2. $AgBr$
3. $A{g}_{2}Cr{O}_4$
4. $AgI$

Q. A hydrogen gas electrode is made by dipping platinum wire in a solution of HCl of $pH=10$ and by passing hydrogen gas around the platinum wire at $1$ atm pressure and ${25}^{\text{0}}C$ Temperature. The oxidation potential of electrode would be:

1. 1018 V
2. 0.059 V
3. 0.59 V
4. 0.118 V

Q.

Calculate the number of moles in 44.8 liters of carbon dioxide at S.T.P.

Q.

$20\mathrm{ml}$ of $0.1\mathrm{M}{\mathrm{H}}_2{\mathrm{SO}}_4$ is added to $30\mathrm{ml}$ of $0.2\mathrm{M}{\mathrm{NH}}_4\mathrm{OH}$ then calculate $\mathrm{pH}$ of resultant solution. (Given that ${\mathrm{pK}}_{\mathrm{b}}\mathrm{of}{\mathrm{NH}}_4\mathrm{OH}\mathrm{is}4.7$)

1. $9$

2. $9.4$

3. $5.2$

4. $5$

Q. How many stereoisomers does this molecule have?
$C{H}_{3}CH=CHC{H}_{2}CHBRC{H}_3$

1. 8
2. 2
3. 4
4. 6

Q.

The vapour density of a mixture containing NO2 and N2O4 is 38.3 at 27'C. Calculate moles of NO2 in 100 g of mixture.

Q.

Find out the total number of optical isomer in the given compound?

1. 10
2. 2
3. 8
4. 6

Q.

Calculate the volume of oxygen at STP that can be produced by 12.25g of KClO3?

Q. $6.02\times {10}^{22}$ Oxygen Molecules are present at – ${13}^{\circ }C$ in 1500 ml vessel what would be the pressure of the gas?

1. 14.2 atm
2. 1.42 atm
3. 2.8 atm
4. 4 atm

Q. 100 ml , 0.5(M) H2SO4 solution is completely neutralised by 50ml 0.1(M) NaOH solution and Xml 0.1(M) Ca(OH)2 solution . Find value of x.

Q. What would be the electrode potential for the half cell reaction at pH = 5?
$2H_{2}O\to O_2+4H^{\oplus }+4e^{-};E_{red}^0=1.23V$
($R=8.314J{\text{mol}}^{-1}{K}^{-1};$ Temperature=298 K; oxygen under std. atm. pressure of 1 bar)

Q. What will be the work done by $3\text{moles}$ of an ideal gas when it expands spontaneously in a vacuum?

1. Zero
2. Infinite
3. 3 joules
4. 9 joules

Q.

Calculate the volume occupied by 8.8 g of $C{O}_2$ at ${31.1}^{\circ }C$ and 1 bar pressure.
$R=0.083barL{K}^{-1}mo{l}^{-1}$
.

Q.

Density of a gas is found to be $5.46g/d{m}^3$ at ${27}^{\circ }C$ at 2 bar pressure. What will be its density at STP?

Q.

What is the empirical formula of a compound containing $60\%$ Sulphur and $40\%$ Oxygen?

Q.

Why is the heat engine not 100% efficient?

Q.

34.05 mL of phosphorus vapour weighs 0.0625 g at ${546}^{\circ }C$ and 1 bar pressure. What is the molar mass of phosphorus?

Q. Solubility of $AgCl$ in 0.1 M calcium chloride solution is:
$(K_{sp}\text{of}AgCl=1.8\times {10}^{–10})$

Q.

State and explain Avogadros law.

Q.

What will be the pressure exerted by a mixture of 3.2 g of methane and 4.4 g of carbon dioxide contained in a $9d{m}^3$ flask at ${27}^{\circ }C$ ?

Q.

Pay load is defined as the difference between the mass of displaced air and the mass of the balloon. Calculate the pay load when a balloon of radius 10 m, mass 100 kg is filled with helium at 1.66 bar at ${27}^{\circ }C$. (Density of air = $1.2kg{m}^{-3}andR=0.083bard{m}^3{K}^{-1}mo{l}^{-1}$).

Q.

What would be the SI unit for the quantity $\frac{P{V}^2{T}^2}{n}$ ?

Q.

Carbon monoxide gas is dissolved in water at 25⁰c and 0.01 atm. Henry’s law constant is 5.8 × 10⁴ atm.

The mole fraction of CO is…………..?

Q.

What volume of 21% oxygen by volume is required of air at NTP to completely burn 1000 gram of sulphur containing 4% incombustible matter ?

Q.

At $0^{\circ }C$, the density of a certain oxide of a gas at 2 bar is same as that of dinitrogen at 5 bar. What is the molecular mass of the oxide?

Q.

The mass of a litre of oxygen at STP was 1.43g and that of a litre of sodium hydroxide is 2.857g.

I) How many molecules of each gas are there in this volume?

II) What is the mass in grams for a single molecule of each gas?