Airforce Group X Quiz || Physics || Heat & Thermodynamics

The internal energy of an ideal gas decreases by the same amount as the work done by the system

Five moles of helium are mixed with two moles of hydrogen to form a mixture. Take molar mass of helium M₁ = 4g and that of hydrogen M₂ = 2g .The equivalent molar mass of the mixture is

Five moles of helium are mixed with two moles of hydrogen to form a mixture. Take molar mass of helium M₁ = 4g and that of hydrogen M₂ = 2g .The equivalent degree of freedom f of the mixture is

Five moles of helium are mixed with two moles of hydrogen to form a mixture. Take molar mass of helium M₁ = 4g and that of hydrogen M₂ = 2g. If the internal energy of He sample of 100J and that of the hydrogen sample is 200 J, then the internal energy of the mixture is

An ideal gas undergoes the process 1 → 2 as shown in the figure, the heat supplied and work done in the process is ΔQ and ΔW respectively. The ratio ΔQ : ΔW is

A reversible adiabatic path on a P-V diagram for an ideal gas passes through state A where P = 0.7 × 10⁵ N/m^-2 and V = 0.0049 m³. The ratio of specific heat of the gas is 1.4. The slope of path at A is :

An ideal gas expands from volume V₁ to V₂. This may be achieved by either of the three processes : isobaric, isothermal and adiabatic, Let ΔU be the change in internal energy of the gas, Q be the quantity of heat added to the system and W be the work done by the system on the gas. Identify which of the following statements is false for ΔU?

In an isobaric expansion of an ideal gas, which of the following is zero ?