Question

При температуре 10 градусов и давлении 10 в 5 степени Па, плотность газа равна 2,5 кг/(м)^3, Какова молярная масса газа?

Answer 1

дана плотность p = m/V = M*P/(R*T), откуда M = p*R*T/P = 2.5*8.314*(273+10)/1e5 = 0.0588 кг/моль = 58.8 г/моль

Answer 2

Calculation of Molar Mass of Gas

To calculate the molar mass of a gas, we can use the ideal gas law equation:

PV = nRT

Where: - P is the pressure of the gas (in Pa) - V is the volume of the gas (in m^3) - n is the number of moles of the gas - R is the ideal gas constant (8.314 J/(mol·K)) - T is the temperature of the gas (in Kelvin)

In this case, we are given: - Temperature (T) = 10 degrees Celsius = 283.15 Kelvin - Pressure (P) = 10^5 Pa - Density (ρ) = 2.5 kg/m^3

To find the molar mass, we need to calculate the number of moles (n) first. We can use the ideal gas law equation to solve for n:

n = PV / RT

Let's substitute the given values into the equation:

n = (10^5 Pa) * (V) / ((8.314 J/(mol·K)) * (283.15 K))

Since we are given the density (ρ) of the gas, we can use the relationship between density, molar mass (M), and volume (V):

ρ = M / V

Rearranging the equation, we get:

V = M / ρ

Substituting this into the equation for n, we have:

n = (10^5 Pa) * (M / ρ) / ((8.314 J/(mol·K)) * (283.15 K))

Simplifying, we get:

n = (10^5 Pa) * M / (8.314 J/(mol·K) * (283.15 K) * ρ

Now, let's solve for M, the molar mass:

M = n * (8.314 J/(mol·K) * (283.15 K) * ρ / (10^5 Pa)

Substituting the given values: - T = 283.15 K - P = 10^5 Pa - ρ = 2.5 kg/m^3

M = n * (8.314 J/(mol·K) * (283.15 K) * (2.5 kg/m^3) / (10^5 Pa)

Now we can calculate the molar mass of the gas using the given values.

Please note that the given values in the question are not clear. The temperature is given as 10 degrees Celsius, but the unit for pressure is not specified. Therefore, we cannot provide an accurate calculation without the proper units for temperature and pressure.

If you provide the correct units for temperature and pressure, we can calculate the molar mass of the gas for you.