The graph of compressibility factor (Z) vs. P for one mole of a real gas is shown in following diagram. The graph is plotted at constant temperature 273K. If the slope of graph at very high pressure `((dZ)/(dP))` is `((1)/(2.8))atm^(-1)` , then calculate volume of one mole of real gas molecules (in L/mol) Given : `N_(A)=6xx10^(23)` and `R=(22.4)/(273)L atmK^(-1)mol^(-1)`

The graph of compressibility factor (Z) vs. P for one mole of a real g

1.	The graph of compressibility factor (Z) vs. P for one mole of a real gas is shown in following diagram. The graph is plotted at constant temperature 273K. If the slope of graph at very high pressure `((dZ)/(dP))` is `((1)/(2.8))atm^(-1)` , then calculate volume of one mole of real gas molecules (in L/mol) Given : `N_(A)=6xx10^(23)` and `R=(22.4)/(273)L atmK^(-1)mol^(-1)`
Answer» Correct Answer - 2 `Z=1+(Pb)/(RT)" high pressure"` `(dZ)/(dP)=(b)/(RT)=(1)/(2.8)` `b=(RT)/(2.8)=(22.4)/(2.8)=4xx(N_(A)xx(4)/(3)piR^(3))` `(N_(A)xx(4)/(3)piR^(3))="Volume of 1 mole gas"` `=(5.6)/(2.8)=2`

Discussion

No Comment Found

Related InterviewSolutions

When is deviation more in the behaviour of a gas from the ideal gas equation `PV=nRT`?A. At high temperature and low pressureB. At low temperature and high pressureC. At high temperature and high pressureD. At low temperature and low pressure
The density of a gas filled in electric lamp is `0.75kg//m^(3)` . After the lamp has been switched on, the pressure in it increases from `4xx10^(4)` Pa to `9xx10^(4)` Pa. What is increases in `u_("rms")` ?A. 100B. 200C. 300D. None of these
In a glass tube columns of water and mercury appear as shown. This is best attributed to the differences in their:A. densitiesB. molar massesC. surface tensionsD. viscosities
The volume of real gases often exceed those calculated by the ideal gas equation. These deviations are best attributed to the:A. attractive forces between the molecuels in real gases.B. dissociation of the molecuels in real gases.C. kinatic energy of the molecules in real gases.D. volumes of the molecules in rel gases.
A container holds 3 liter of `N_(2(g))` and `H_(2)O_((l))` at `29^(@)C` The prssure is found to be 1 atm The water in container is instantaneously electrolysed to give `H_(2)` and `O_(2)` following the reaction `H_(2)O_(l) rarrH_(2(g)) +(1)/(2)O_(2_(g))` At the end of electrolysis the pressure was found to be `1.86atm` calculate the amount of water present in the container If the aqueous tension of water at `29^(@)C` is `0.04 atm ` .
Match of following (where `U_(rms)`=root mean square speed `U_(av)` =average speed `U_(mp)` = most probable speed) `{:(,"List-I",,"List-II"),("(a)",U_(rms)//U_(av),,(p)1.22),("(b)",U_(av)//U_(mp),,"(q)1.13"),((c),U_(rms)//U_(mp),,"(r)1.08):}`
The `u_(rms)` of a gas at `300K` is `3R^(1//2)` The molar mass of the gas in `kg mo1^(-1)` is .A. `1.0 xx 10^(-1)`B. `1.0 xx 10^(-2)`C. `1.0 xx 10^(-3)`D. `1.0`
The cirtical constant for water are `374^(@)C` 218 atm and 0.0566 liter `mo1^(-1)` Calculate a,b and `R` .
The density of a gas `A` is twice that of a gas `B` at the same temperature. The molecular mass of gas `B` is thrice that of `A`. The ratio of the pressure acting on `A` and `B` will beA. `6:1`B. `7:6`C. `2:5`D. `1:4`
`n_(1)` and `n_(2)` moles of two ideal gases (mo1 wt `m_(1)` and `m_(2))` respectively at temperature `T_(1)K` and `T_(2)K` are mixed Assuming that no loss of energy the temperature of mixture becomes .A. `n_(1)T_(1)+n_(2)T_(2)`B. `(n_(1)T_(1)+n_(2)T_(2))/(T_(1)+T_(2))`C. `(n_(2)T_(1)+n_(1)T_(2))/(n_(1)+n_(2))`D. `(T_(1)xxT_(2))/(n_(1)xxn_(2))`

Discussion

No Comment Found

Related InterviewSolutions

Reply to Comment