Determine the pressure of 4 gm of hydrogen occupying 16 litres of volume at `10^@C` (`R = 8.315 J//mol K`, molecular weight of hydrogen = 2)

If the R.M.S. velocity of oxygen molecules at N.T.P. is 460 m//s , determine the R.M.S. velocity of hydrogen molecules at N.T.P. (molecular weight of oxygen = 32, molecular weight of hydrogen = 2).

If the R.M.S. velocity of oxygen molecules at N.T.P. is 460 m//s , determine the R.M.S. velocity of hydrogen molecule at N.T.P. (molecular weight of O_2 = 32, molecular weight of hydrogen = 2).

Calculate kinetic energy of 10 gm of Argon molecule at 127^@C . (R = 8320 J//K mole K, Atomic weight of Argon = 40)

Compare the R.M.S. velocity of hydrogen molecules at 400 K with R.M.S. velocity of oxygen molecules at 900 K. (Molecular weight of hydrogen = 2, molecular weight of oxygen = 32)

Find the KE:- per molecule of nitrogen at N.T.P.(molecular weight of N_2 = 28, Normal pressure = 76 cm of mercury, density of mercury 1.36 gm//cm^2 , g = 980 cm//s^2 , Avogadro's number 6.023 xx 10^23 , R = 8.314 xx 10^7 erg//mol^k , molecular weight of nitrogen = 31).

Find the KE per kg of nitrogen molecule at 127^@C (molecular weight of nitrogen = 28, R = 8320 J//K mole K ).

IF 10 g of solute was dissolved in 250 mL. of water and osmotic pressure of the solution was found to be 600 mm of Hg at 300 K, then molecular weight of the solute is _______. g mol ^(-1)

Calculate the average molecular kinetic energy : per kg molecule of oxygen at 127 ∘ C, given that the molecular weight of oxygen is 32, R = 8.31 J m o l ^ -1 K − 1 , and Avogadros number N A ​ is 6.02×10 23 molecules mol −1 .

Determine the osmotic pressure of a solution prepared by dissolving 25 mg of K_2SO_4 in 2 litres of water at 25^@C , assuming that it is completely dissociated.