Jack359 said:Homework Statement
Hello, I have really hard time to express the gas law PV=nRT to PQ=ṁRT where Q is volumetric flow rate and ṁ- mass flow rate.
Is it possible ?
Teacher told me, it is ...
The main difference between the two equations is the variable being solved for. In PV=nRT, the equation represents the ideal gas law and solves for pressure (P), volume (V), number of moles (n), gas constant (R), and temperature (T). On the other hand, PQ=ṁRT represents the mass flow rate (ṁ) and volumetric flow rate (Q) of a fluid, where P is pressure, R is the gas constant, and T is temperature.
The volumetric flow rate (Q) is calculated by dividing the mass flow rate (ṁ) by the density (ρ) of the fluid. This relationship can be represented as Q=ṁ/ρ. In some cases, ρ can be substituted with the specific volume (v) of the fluid, where ρ=1/v. Therefore, Q=ṁv.
The gas constant (R) is a proportionality constant that relates the pressure, volume, number of moles, and temperature of an ideal gas. It is a universal constant and is the same for all gases. In PQ=ṁRT, R is also used to relate the mass flow rate and volumetric flow rate of a fluid.
No, PQ=ṁRT is applicable only to ideal gases and incompressible fluids. Incompressible fluids are those that do not change in volume when subjected to pressure. Real gases and compressible fluids require more complex equations to determine the relationship between pressure, volume, temperature, and flow rate.
According to the equation PQ=ṁRT, the flow rate (Q) is directly proportional to the temperature (T). This means that as the temperature increases, the flow rate also increases and vice versa. This relationship is only valid for ideal gases and incompressible fluids, as real gases and compressible fluids may exhibit different behavior at different temperatures.