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Dalton?s law of partial ..



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Q1. The fact that internal energy of a mixture is equal to the sum of the partial internal energies of the gases can also be applied to properties like H,Cv,Cp,S,F, and G.

(a) true
(b) false
(c) -
(d) -

Q2. When gases which are at equal pressure and temperature are mixed adiabatically without work, then

(a) internal energy of the gaseous system remains constant
(b) heat transfer of the gaseous system remains constant
(c) entropy of the gaseous system remains constant
(d) all of the mentioned

Q3. The total entropy of a mixture of gases is the ____ of the partial entropies.

(a) average
(b) weighted mean
(c) sum
(d) difference of the highest and the lowest

Q4. Which of the following statement is true?

(a) V=V1+V2+?.+Vc , where V is the partial volume of the component
(b) 1/v = 1/(v1) + 1/(v2) + ??.. + 1/(vc) , where v is the specific volume of the component
(c) total density is equal to the sum of the densities of the components
(d) all of the mentioned

Q5. A quantity called partial volume of a component of mixture is used.

(a) true
(b) false
(c) Same
(d) Zero

Q6. The gas constant of the mixture is the ____ of the gas constants of the components.

(a) average
(b) weighted mean
(c) sum
(d) difference of the highest and the lowest

Q7. Which of the following relation is correct?

(a) mole fraction of the Kth gas = moles of the Kth gas / total number of moles of gas
(b) partial pressure of Kth gas = (mole fraction of the Kth gas)*(sum of the partial pressures)
(c) sum of mole fractions of all the gases is unity
(d) all of the mentioned

Q8. According to the Dalton?s law of partial pressures, the total pressure of a mixture of ideal gases is equal to the

(a) difference of the highest and lowest pressure
(b) product of the partial pressures
(c) sum of the partial pressures
(d) none of the mentioned

Q9. The expression nRT/V is called the partial pressure of a gas.

(a) true
(b) false
(c) entropy of the gaseous system remains constant
(d)

Q10. The expression which represents the pressure exerted by a gas is

(a) nVRT
(b) nRT/V
(c) V/nRT
(d) 1/nVRT


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1 Answer
458 views

In A Closed Flask Of 5 Litres, 1.0 G Of H2 Is Headed From 300 To 600 K. Which Statement Is Not Correct

Modified 238 Year Ago

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238 Year Ago

In A Closed Flask Of 5 Litres, 1.0 G Of H2 Is Headed From 300 To 600 K. Which Statement Is Not Correct

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1 Answer
440 views

Equal Amounts Of Two Gases Of Molecular Weight 4 And 40 Are Mixed. The Pressure Of The Mixture Is 1.1 Atm. The Partial Pressure Of The Light Gas In This Mixture Is

Modified 238 Year Ago

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238 Year Ago

Equal Amounts Of Two Gases Of Molecular Weight 4 And 40 Are Mixed. The Pressure Of The Mixture Is 1.1 Atm. The Partial Pressure Of The Light Gas In This Mixture Is

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1 Answer
412 views

Assertion : Effusion Rate Of Oxygen Is Smaller Than Nitrogen. Reason : Molecular Size Of Nitrogen Is Smaller Than Oxygen.

Modified 238 Year Ago

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238 Year Ago

Assertion : Effusion Rate Of Oxygen Is Smaller Than Nitrogen. Reason : Molecular Size Of Nitrogen Is Smaller Than Oxygen.

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1 Answer
405 views

Molecules/ions And Their Magnetic Properties Are Given Below

Modified 238 Year Ago

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238 Year Ago

Molecules/ions And Their Magnetic Properties Are Given Below

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1 Answer
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Assertion : We Air Is Heavier Than Dry Air. Reason : The Density Of A Dry Air Is More Than Density Of Water.

Modified 238 Year Ago

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238 Year Ago

Assertion : We Air Is Heavier Than Dry Air. Reason : The Density Of A Dry Air Is More Than Density Of Water.

0 votes
1 Answer
400 views

Assertion : 4.58mm And 0.0098°C Is Known To Be Triple Point Of Water. Reason : At This Pressure And Temperature All The Three States I.e., Water, Ice And Vapour Exist Simultaneously.

Modified 238 Year Ago

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238 Year Ago

Assertion : 4.58mm And 0.0098°C Is Known To Be Triple Point Of Water. Reason : At This Pressure And Temperature All The Three States I.e., Water, Ice And Vapour Exist Simultaneously.

0 votes
1 Answer
395 views

In Van Der Waals Equation Of State Of The Gas Law, The

Modified 299 Year Ago

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299 Year Ago

In Van Der Waals Equation Of State Of The Gas Law, The

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