The `r.m.s`. velocity of hydrogen at `27^(@)C, R= 8.314 J mol^(-1)K^(-1)` is:

Find the kinetic energy of 8 g of oxygen at 27^@C (R = 8.3 J mol^(-1) K ^(-1) ).

Calculate the temperature at which the rms velocity of hydrogen will be equal to 8 km//s. Take R = 8.31 J "mole"^(-1) K^(-1)

The kinetic energy in J of 1 mole of N_2 at 27^@ C is (R= 8.314 mol^(-1) k^(-1))

Calculate the total and average kinetic energy of 32 g of methane molecules at 27^(@)C. (R="8.314 J K"^(-1)"mol"^(-1)) .

Calculate the molar specific heat at constant volume of neon gas. (R = 8.314 J mol^(-1) K^(-1) )

A reaction has an activation energy of 209 KJ "mol"^(-1) . The rate increase 10-fold when the temperature is increased from 27^(@)C to X ""^(@)C . The temperature X is closed to [Gas constant, R = 8.314 J "mol"^(-1) K^(-1) ]

A first order reaction is 50% complete in 30 minutes at 27^(@) C and in 10 minutes at 47^(@) C. Calculate the reaction rate constants at these temperatures and the energy of activation of the reaction in kJ//mol (R=8.314 J mol^(-1)K^(-1))