Home
Class 11
CHEMISTRY
A vessel of 25 L capacity contains 10 mo...

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)`.

Text Solution

AI Generated Solution

To solve the problem using the van der Waals equation, we will follow these steps: ### Step 1: Write down the van der Waals equation The van der Waals equation is given by: \[ \left(P + \frac{a n^2}{V^2}\right)(V - nb) = nRT \] Where: ...
Promotional Banner

Topper's Solved these Questions

  • STATES OF MATTER : GASES AND LIQUIDS

    MODERN PUBLICATION|Exercise Practice Problems|54 Videos

  • STATES OF MATTER : GASES AND LIQUIDS

    MODERN PUBLICATION|Exercise Advanced Level (PROBLEMS)|14 Videos

  • SOME BASIC CONCEPTS OF CHEMISTRY

    MODERN PUBLICATION|Exercise COMPETITION FILE (INTEGER TYPE AND NUMERICAL VALUE TYPE QUESTIONS)|10 Videos

  • STRUCTURE OF ATOM

    MODERN PUBLICATION|Exercise Unit Practice Test|13 Videos

Similar Questions

Explore conceptually related problems

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) .

A quantity of 2 mol of NH_(3) occupies 5L at 27^(@)C . Calculate the pressure of the gas using the van der Waals equation if a = 4.17 "atm "L^(2)" mol"^(-2) and b = 0.3711 L "mol"^(-1) .

Two moles of ammonia were found to occupy a volume of 5 L at 27^(@)C . Calculate the pressure using van der Waals equation (a="4.17 bar L"^(2)"mol"^(-2), b="0.0371 L mol"^(-1)).

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) .

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)

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) .

Pressure exerted by 1 mole of methane in a 0.25 litre container at 300K using Vander Waal’s equation : (Given : a = 2.253 "atm" l^(2) "mol"^(-2) and b = 0.0428 l "mol"^(-1) ) is

Calculate the critical temperature of a Van der Waals gas for which p_(c ) is 100 atm and b is "0.050 dm"^(3)" mol"^(-1) .

Compare the temperature of 3 molof SO_(2) at 15 bar occupying a volume of 10 L obtained by the ideal gas equation and van der Waals equation (a="6.7 bar L"^(2)"mol"^(-2), b="0.0564 L mol"^(-1))

Pressure exerted by 1 mole of methane, in a 0.25 litre container at 300K using van der Waals' equation (given a= 2.253 atm L^(2) mol^(-2), b= 0.0428L mol^(-)) is