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Published on: 04/09/2019
State of Matter
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1.
Rohan takes an open pan to cook vegetables and pulses at a hill station while Sohan cooks pulses and vegetables in a pressure cooker at the same place.The gas cylinder of Rohan lasts for only 15 days whereas Sohan uses one gas cylinder per month.
Why does Sohan need only one gas cylinder per month and not two like Rohan?
2.
An iron cylinder contains helium at a pressure of 250 KPa at 300 K. The cylinder can withstand a pressure of \(1\times { 10 }^{ 6 }Pa\) . The room in which cylinder is placed catches fire. Predict whether the cylinder will blow up before it melts or not (mp of the cylinder = 1800 K).
3.
Explain
The boiling point of water (373 K) is abnormally high when compared to that H2S (211.2 K).
4.
Compressibility factor, Z of a gas is given as \(Z=\frac { pV }{ nRT } \) For real gas what will be the effect on the value of Z above Boyle's temperature?
5.
35mL of oxygen were collected at 6\(^{o}\)C and 758 mm pressure. Calculate its volume at NTP.
6.
What would have happened to the gas if the molecular collision were not elastic?
7.
Explain the physical significance of van derWaals' parameters.
8.
Explain why temperature of a boiling liquid remains constant?
9.
A gas that follows Boyle's law, Charle's law and Avogadro's law is called an ideal gas.Under what condition a real gas would behave ideally?
10.
One of the assumptions of kinetic theory of gases states that "there is no force of attraction between the molecules of a gas "How far is this statement correct?Is it possible to liquefy an ideal gas? Explain.
11.
The compression factor(compressibility factor) for one mole of a van der Waals gas at 0oC and 100 atm pressure is found to be 0.5. Assuming that the volume of a gas molecule is negligible, calculate the van der Walas' constant a.
12.
A student forgot to add the reaction mixture to the round bottom flask at 27\(^{o}\) C but instead, he/she placed the flask on the flame. After a lapse of time, he realized his mistake and using a pyrometer he found the temperature of the flask was 477 C. What fraction of air would have been expelled out?
1.
Sohan needs less fuel as pressure cooker helps in cooking at faster rate.
2.
According to Gay-Lussac's law, \(\frac { { p }_{ 1 } }{ { T }_{ 1 } } =\frac { { p }_{ 2 } }{ { T }_{ 2 } } \)
\(\frac { 250 }{ 300 } =\frac { { p }_{ 2 } }{ 1800 } or{ \ p }_{ 2 }=1500kPa\)
As the cylinder can withstand a pressure of \({ 10 }^{ 6 }\)
\(Pa=10^{ 3 }kPa\) = 1000kPa, hence, it will blow up.
3.
The extensive hydrogen bonding in water gives a polymeric structure. This makes the escape of molecules from the liquid more difficult.
4.
Above Boyle's temperature, real gases show positive deviation
So, Z > 1
5.
Given Condition
V1 = 35mL
p1 = 758 mm
T1 = 6 + 273 =279K
T2 = 0 +273 = 273K
Final Conditions
V2 = ? mL
p2 = 760 mm
By applying gas equation, we have
\(\cfrac { 760\times { { V }_{ 2 } } }{ 273 } =\cfrac { 758\times 35 }{ 279 } \)
V2 = \(\cfrac { 758\times 35 }{ 279 } \times \cfrac { 273 }{ 760 } =34.16\)
Volume of chloride gas = 34.16 mL.
6.
( )
On every collision, there would have been loss of energy.As a result, the molecules would have slowed down and ultimately settle down in the vessel.Moreover, the pressure would have gradually reduced to zero.
7.
( )
a is measure of magnitude of intermolecular forces of attraction while b is a measure of the effective volume of the gas molecules.Value of a and b depends upon the characteristics of a gas.
8.
( )
This is because at the boiling point, the heat supplied is used up in breaking off the intermolecular forces of attraction of the liquid to change it into vapour and not for raising the temperature of the liquid.
9.
( )
A low pressure and high temperature, a real gas behaves as an ideal gas.
10.
( )
This statement is correct only for ideal gases.It is not possible to liquefy an ideal gas because there is no intermolecular forces of attraction between the molecules of an ideal gas.
11.
\(Z=\frac { pV }{ nRT } \ i.e \ 0.5=\frac { 100\times V }{ 1\times 0.082\times 273 } \)
or
\(V=0.1119L\)
\( \left( P+\frac { a }{ { V }^{ 2 } } \right) (v-b)=RT \ for \ 1 \ mol\)
Neglecting b, \(\left( P+\frac { a }{ { V }^{ 2 } } \right) V=RT\)
or \(pV+\frac { a }{ V } =RT\)
or \(\frac { pV }{ RT } +\frac { a }{ VRT } =1\)
or
\(a=\left( 1-\frac { pV }{ RT } \right) VRT=(1-0.5)0.1119\times 0.082\times 273\)
\( =1.252 \ atm \ L^{ 2 }mol^{ -2 }\)
12.
Suppose volume of the air in flask = V cm3 at 27\(^{o}\) C (300K).
V1 = Vcm3 , V2 = ?, T1= 300 K, T2 = 750 K
\(\cfrac { { V }_{ 1 } }{ { T }_{ 1 } } =\cfrac { { V }_{ 2 } }{ { T }_{ 2 } } \)
or \(\cfrac { { V } }{ 300 } =\cfrac { { V }_{ 2 } }{ { 750 } } \)
or \(300{ V }_{ 2 }=750V\)
or \({ V }_{ 2 }=2.5V\) (final volume)
Volume expelled = 2.5 V - V = 1.5 V
Fraction of air expelled = \(\cfrac{1.5 V}{2.5 V}=0.6\)
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