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 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 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) .

Calculate the specific heat of a gas at constant volume from the following data. Desity of the gas at N.T.P=19xx10^(-2)kg//m^(3) , (C_(p)//C_(v))=1.4,J =4.2xx10^(3) J//kcal : atmospheric pressure =1.013xx10^(5)N//m^(2) . ("in" kcal//kg k)

Calculate the difference between two specific heats of 1 g of nitrogen. Given molecular weight of nitrogen = 28 and J = 4.2 times 10^7 erg cal^-1 .

Calculate the gas constant for 1 g of gas from the following data : C_p=0.245 "cal g"^(-1).^@C^(-1), C_v=0.165" cal g"^(-1).^@C^(-1)and J=4.2 xx10^7 erg cal^(-1)

Calculate the gas constant for 1 g of gas from the following data : C_p=0.245 "cal g"^(-1).^@C^(-1), C_v=0.165" cal g"^(-1).^@C^(-1)and J=4.2 xx10^7 erg cal^(-1)

Calculate the molar specific heat at constant volume . Given : specific heat of hydrogen at constant pressure is 6.85 "cal" mol^(-1) K^(-1) and density of hydrogen = 0.0899 "g" cm^(-3) . One mole of gas = 2.016g, J=4.2xx10^(7) "erg" cal^(-1) and 1 atmosphere = 10^(6) "dyne" cm^(-2) .

Calculate the molar specific heat at constant volume . Given : specific heat of hydrogen at constant pressure is 6.85 "cal" mol^(-1) K^(-1) and density of hydrogen = 0.0899 "g" cm^(-3) . One mole of gas = 2.016g, J=4.2xx10^(7) "erg" cal^(-1) and 1 atmosphere = 10^(6) "dyne" cm^(-2) .