Home
Class 12
CHEMISTRY
Calculate % of 'free volume' available i...

Calculate % of 'free volume' available in 1 mol gaseous water at 1.0 atm and `100^(@)C` .Density of liquid water at `100^(@)C` is 0.958 `g//mol`.

Text Solution

AI Generated Solution

To calculate the percentage of 'free volume' available in 1 mole of gaseous water at 1.0 atm and 100°C, we can follow these steps: ### Step 1: Calculate the Volume of 1 Mole of Gaseous Water We will use the Ideal Gas Law, which is given by the equation: \[ PV = nRT \] Where: ...
Promotional Banner

Similar Questions

Explore conceptually related problems

Calculate the percentage of free volume available in 1 mole gaseous water at 1 atm pressure and 373 K.

On heating water from 0^(@)C to 100^(@)C its volume

A balloon of diameter 21 meter weight 100 kg. Calculate its pay-load, if it is filled with He at 1.0 atm and 27^(@)C . Density of air is 1.2 kg m^(-3) . (Given : R=0.082 L atm K^(-1)mol^(-1) )

Calculate the entropy change for vaporization of 1mol of liquid water to steam at 100^(@)C , if Delta_(V)H = 40.8 kJ mol^(-1) .

Calculate the entropy change (DeltaS) when 1 mol of ice at 0^(@)C is converted into water at 0^(@)C . Heat of fusion of ice at 0^(@)C is 1436 cal per mol.

One moles of strem is compressed reversibly of water at boiling point 100^(@)C . The heat of vapourisation of water at 100^(@)C and 1atm is 540cal g^(-1) . Calculate DeltaU and DeltaH .

What is Delta U when 2.0 mole of liquid water vaporises at 100^(@)C ? The heat of vaporisation (Delta H_("vap".)) of water at 100^(@)C is 40.66 KJmol^(-1) .

What is the free energy change, 'DeltaG' When 1.0 mole of water at 100^(@)C and 1 atm pressure is converted into steam at 100^(@)C and 1 atm pressure

If water vapour is assumed to be a perfect gas, molar enthalpy change for vapourisation of 1 mol of water at 1bar and 100^(@)C is 41kJ "mol"^(-1) . Calculate the internal energy change, when 1 mol of water is vapourised at 1 bar pressure and 100^(@)C.

Calculate the molar mass of a substance 1 g of which when dissolved in 100 g of water gave a solution boiling at 100.1^(@)C at a pressure of 1 atm (K_(b) for water = 0.52 K kg mol^(-1))