Related InterviewSolutions

• Under standard conditions the density of a helium (atomic weight `=m_(1)`) and nitrogen (atomic weight `m_(2)`) mixture is `rho`. Find the concentration of the helium atoms in the mixture.
• One mole of oxygen is mixed withone mole of helium. What is `gamma` of the mixture?
• If the kinetic energy of the molecules in 5 litre of helium at 2 atm is `(E )`. What is the kinetic energy of molecules in 15 litre of oxygen at 3 atm in terms of `(E )` ?
• How many atoms do the molecules of a gas consist of if its `gamma` increases 1.2 times when the vibrational degrees of freedom are frozen? Assume the atoms to hbe linearly arranged.
• One cubic metre of air at `27^(@)C` and `10^(5)Nm^(-2)` pressure weighs `1.18kg`. Calculate the value of the gas constant for `1kg` of the gas and calculate `c_(p)` of air if `168 cal kg^(-1)K^(-1)` and `J=4.2Jcal^(-1)`
• The gran -molecular sp heat capacity of hydrogen at constant pressure `=6.865` cal and volume `=0.0224` cubic metre and coefficient of expansioin of hydrogen at constant pressure `alpha=1/273.3` per kelvink. Calculate the value of `J`. ( 1 atmospheric pressure `=1.013xx10^(5)` newtons per square metre.)
• The density of gas at NTP `=2.468kgm^(-3)` and `c_(p)=156cal kg^(-)K^(-1)`. Find the ratio of specific heat capacities of the gas. Is it diatomic or tiratomic?
• One cubic metre of hydrogen at `0^(@)C` and `76cm` and of `Hg` weighs `0.0896kg`. The specific heat capacities of hydrogen at constant pressure volume are 3409 and 2411 cal per kg per kelvin, respectively. Calculate the value of `J`. (`g=9.81,ms^(-2)` density of mercury `=13.6xx10^(3)` kg per cubic metre)
• The difference in the two molar specific heat capacities of a gas is 2 calories. Calculate the mechaical equivalent of heat assuming that the molar volume of a gas a NTP is `0.0244m^(3)`. `(g=9.81ms^(-2)` and density of mercury `=13.6xx10^(3)kgm^(-3)`)
• Find the specific heat capacities `c_v` and `c_p` for a gaseous mixture consisting of `7.0 g` of nitrogen and `20 g` of argon. The gases are assumed to be ideal.