Home
Class 11
CHEMISTRY
Calculate the temperature of 2 moles of ...

Calculate the temperature of 2 moles of sulphur dioxide gas contained in a 5 L vessel at 10 bar pressure. Given that for `SO_(2)` gas, van der Waals constants are : a=6.7 bar `L^(2) mol^(-2)` and b=0.0564 L `mol^(-1)`.

Text Solution

Verified by Experts

According to van der Waals equation, `(P+(an^(2)))/(V^(2))(V-nb)=nRT`
`T=((P+an^(2)//V^(2))(V-nb))/(n R)`
As pressure is in bar, taking R=0.083 L `K^(-1) mol^(1)` and substituting the given values, we get
`T=([10 "bar "+(6.7 " bar "L^(2)mol^(-2))(2 mol)^(2)//(5 L)^(2)](5L^(-2)molxx0.0564 L mol^(-1)))/(2 molxx0.083" L bar K"^(-1) mol^(-1))`
`=((10 " bar"+1.072" bar")(5 L-0.1128 L))/(2xx0.083" L bar K"^(-1))=326 K`
Promotional Banner

Topper's Solved these Questions

  • STATES OF MATTER : GASES AND LIQUIDES

    PRADEEP|Exercise PROBLEM|18 Videos

  • STATES OF MATTER : GASES AND LIQUIDES

    PRADEEP|Exercise PROBLEMS FOR PRACTICE|44 Videos

  • SOME p-BLOCK ELEMENTS

    PRADEEP|Exercise Competition Focus (JEE( Main and Advanced)/Medical Entrance) VIII. Assertion-Reason Type Questions (Type I)|23 Videos

  • STATES OF MATTER: SOLID MATTER

    PRADEEP|Exercise COMPETITION FOCUS (ASSERTION-REASON)|17 Videos

Similar Questions

Explore conceptually related problems

Calculate the critical constants of a gas whose van der Waals constants are : a=0.751" L"^(2)" atm "mol^(-2) and b=0.0226" L mol"^(-1) .

At what temperature will 128 g of SO_(2) confined in a vessel of 5 dm^(3) capacity exhibit a pressure of 10.0 bar? The van der waals constants for SO_(2) are a = 6.7 bar L^(2) mole^(-2) and b = 0.0564 L mol^(-1) .

Calculate the pressure exerted by 110 g of carbon dioxide in a vessel of 2 L capacity at 37^(@)C . Given that the van der Waal’s constants are a = 3.59 L^(2) " atm "mol^(-2) and b = 0.0427 L mol^(-1) . Compare the value with the calculated value if the gas were considered as ideal.

A vessel of 25 L capacity contains 10 mol of steam under 50 bar pressure. Calculate the temperature of steam using van der Waals equation if for water : a="5.46 bar L"^(2)"mol"^(-2) and b="0.031 L mol"^(-1) .

Calculate the pressure of 10^(23) molecules of sulphur dioxide (SO_(2)) when enclosed in a vessel of 2.5 L capacity at a temperature of 27^(2)C .

Assuming CO_(2) to be van der Waals gas, calculate its Boyle temperature. Given a=3.59" L"^(2)" atm " mol^(-2) and b=0.0427" L "mol^(-1) .

One mole of CO_(2) occpuies 1.5 L at 25^(@)C . Calculate the pressure exerted by the gas using (i) ideal gas equation van der Waals gas equation with a=3.6 L^(2)" bar mol"^(-2) and b="0.04 L mol"^(-1)

180 g of steam is contained in a vessel of 25 L capacity under a pressure of 50 atm. Calculate the temperature of the steam. Given that for water vapour, a=5.46" bar" L^(2)mol^(-2)" and "b=0.031 L mol^(-1) .

Calculate critical temperature and critical pressure of oxygen if the values of the van der Waal's constants a and b are 1.32 dm^(6) "bar" mol^(-2) and 0.0312 dm^(3) mol^(-1) respectively.