হাইড্রোজেনের জন্য ভ্যান ডের ওয়ালস ধ্রুবক a এবং b হল `0.246` atm `লিটার^(2) mo1^(-2)`

van der Waals constants a and b for hydrogen are 0.246 atm liter^(2) mo1^(-2) and 0.0267 litre mo1^(-1) respectively Calculate inversion temperature and Boyle's temperature of H_(2) gas .

Calculate the temperature of gas if it obeys van der Waals equation from the following data A flask of 25 litre contains 10 moles of a gas under 50 atm Given a = 5.46 atm "litre"^(2) mo1^(-2) and b =0.031 litre mo1^(-1) .

How many moles of SO_(2) will occupy a volume of 10 litre at a pressure of 15 atm and temperature 624 K ? (a = 6.71 atm L^(2) mol^(-2) , b = 0.0564 litre mol^(-1) )

A ballon of diameter 20 metre weighs 100 kg Calculate its pay-load if its is filled with He at 1.0 atm and 27^(@)C Density of air is 1.2 kg,^(-3) [ R =0.082 dm^(3) atm K^(-1) mo1^(-1)] .

Find the temperature at which 3 moles of SO_(2) will occupy a volume of 10 litre at a pressure of 15 atm a = 6.71 atm "litre"^(2) mol^(-2), b = 0.0564 " litre " mol^(-1)

The volume of 2.8 g of carbon monoxide at 27^(@) C and 0.821 atm pressure (R = 0.821 "atm" K^(-1) "mol"^(-1))

The van der Waal's constants for a gas are a=1.92 atm L^(2) "mol"^(-2),b=0.06 L "mol"^(-1) . If R = 0.08 L atm K^(-1) "mol"^(-1) , what is the Boyle's temperature (in K) of this gas ?

What is the density of N_(2) gas at 227^(@)C and 5.00 atm pressure? (R= 0.0821 atm K^(-1)mol^(-1))

In a closed cylinder of capacity 24.6 L the following reaction occurs at 27^@C , A_2(s) hArr B_2(s) +2C(g) At equilibrium 1 g of B_2(s) (molar mass = 50 g mol^(-1) ) is present . The equilibrium constant K_p for the equilibrium in atm^2 unit is (R=0.082 L atm K^(-1) mol^(-1) )