Calculate the value of `c_(v)` for air, given that `c_(p) = 0.23` calorie `g^(-1)K^(-1)`. Density of the air at S.T.P. is 1.293 `g litre ^(-1)` and `J = 4.2 xx 10^(7)` erg ` calorie ^(-1)`.

Calculate the two specific heats of nitrogen from the following data : gamma = c_(p)//c_(v) = 1.51 density of nitrogen at N.T.P = 1.234 g litre ^(-1) and J = 4.2 xx 10^(7) erg cal^(-1) .

Calculate difference in specific heats for 1 gram of air at N.T.P . Given density of air at N.T.P. is 1.293 g litre^(-1), j=4.2xx10^(7)" erg "cal^(-1) .

The mass of 1 L of air at STP is 1.293 g. If c_(v) = 0.169 cal cdot g^(-1) cdot^(@)C^(-1) for air, what is the value of c_(p) ? Given density of mercury at 0^(@)C = 13.6 g cdot cm^(-3) and J = 4.2 xx 10^(7) erg cdot cal^(-1) .

Calculate the r.m.s velocity of air molecules at S.T.P. Density of air at S.T.P. is 1.29 kg m^(-3)

Specific heat of argon at constant pressure is 0.125 cal.g^(-1) K^(-1) , and at constant volume 0.075 cal.g^(-1)K^(-1) . Calculate the density of argon at N.T.P. Given J = 4.18 xx 10^(7)" erg "cal^(-1) and normal pressure = 1.01 xx 10^(6)" dyne "cm^(-2) .

Calculate the ratio of specific heats for nitrogen. Given that the specific heat of nitrogen at cinstant pressure =0.236 cal g^(-1) K^(-1) and density at S.T.P. is 0.001234 g//c c . Atmospheric pressure =1.01xx10^(6) dyn e//cm^(2) .

Find the molecular kinetic energy of 1 g of helium at S.T.P. Given R = 8.3 xx 10^(7) erg .

The volume of 1.0 g of hydrogen in litres at N.T.P. is