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Which of the following indicates Kinetic...

Which of the following indicates Kinetic gas equation ?
a) `PV = (3M)/(C^2) "   "` b) `PV = 1/3 mnC^2 "    "` c) `P = 1/3 dC^3 "     "` d) `KE = 3/2 RT`

A

a,c

B

b,d

C

a,b

D

b,c

Text Solution

Verified by Experts

The correct Answer is:
D
`PV = 1/3 mnc^2 implies PV = 1/3 dc^2`
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Knowledge Check

  • If A, B, C are mutually exclusive and exhaustive events such that P(B) = (3)/(2)P(A) , P(C) = (1)/(3)P(B) then P(A) =

    A
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    B
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    C
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    D
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  • On the basis of the postulates of kinetic theory of gases, it is possible to derive the mathematical expression, commonly known as kinetic gas equation. PV = 1/3 m n u^3? where, P= Pressure of the gas, V a volume of the gas, m=Mass of a molecule, n = Number of molecules present in the given amount of a gas and u = root mean square speed For one mole of gas, PV = RT and n=N_A 1/3 m N_a u^2 = RT or 2/3 .1/2m N_A u^2 = N_A [1/2mN_Au^2 = KE "per mole"] ,2/3K.E. = RT implies K.E. 3/2RT Average kinetic energy per mol does not depend on the nature of the gas but depends only on temperature. This, when two gases are mixed at the same temperature, there will be no rise or decrease in temperature unless both react chemically. Average kinetic energy per molecule = ("Average K.E. per mole")/N = 3/2(RT)/(N) implies 3/2kT where k is the Boltzmann constant The average kinetic energy (in joule) of the molecules in 8g methane at 27&@C is.

    A
    `62.14 xx 10^(-22)J`
    B
    `72.68 xx 10^(-21) J`
    C
    `68.2 xx 10^(-21) J`
    D
    `62.14 xx 10^(-20)J`

  • On the basis of the postulates of kinetic theory of gases, it is possible to derive the mathematical expression, commonly known as kinetic gas equation. PV = 1/3 m n u^3? where, P= Pressure of the gas, V a volume of the gas, m=Mass of a molecule, n = Number of molecules present in the given amount of a gas and u = root mean square speed For one mole of gas, PV = RT and n=N_A 1/3 m N_a u^2 = RT or 2/3 .1/2m N_A u^2 = N_A [1/2mN_Au^2 = KE "per mole"] ,2/3K.E. = RT implies K.E. 3/2RT Average kinetic energy per mol does not depend on the nature of the gas but depends only on temperature. This, when two gases are mixed at the same temperature, there will be no rise or decrease in temperature unless both react chemically. Average kinetic energy per molecule = ("Average K.E. per mole")/N = 3/2(RT)/(N) implies 3/2kT where k is the Boltzmann constant Which of the following expressions correctly represents the relationship between the average molar kinetic energies of CO and N_2 molecules at the same temperature ?

    A
    `K.E.(CO) = KE.(N_2)`
    B
    `K.E.(CO) gt KE.(N_2)`
    C
    `K.E.(CO) lt KE.(N_2)`
    D
    cannot be predicated

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