Question

Початковий тиск гелію у балоні об'ємом 100дм³ дорівнює 5МПа. Температура газу 27°С. Вентиль балона почав пропускати газ і після того, як пошкодження було ліквідовано, тиск у балоні дорівнював 5,1 МПа, а температура підвищилась до 340К. Визначити масу газу, що вийшла з балона? ​

Answer 1

Ответ:

см фото

Объяснение:

Answer 2

To determine the mass of gas that escaped from the balloon, we can use the ideal gas law equation: PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature.

First, let's convert the given temperature from Celsius to Kelvin: 27°C + 273.15 = 300.15 K

Given: Initial pressure (P1) = 5 MPa Initial volume (V1) = 100 dm³ Final pressure (P2) = 5.1 MPa Final temperature (T2) = 340 K

We can assume that the number of moles of gas remains constant during the process, as no information is provided about the addition or removal of gas from the balloon.

Using the ideal gas law equation, we can calculate the number of moles of gas in the balloon before and after the gas escaped:

For the initial state: P1V1 = nRT1 (5 MPa)(100 dm³) = n(0.0821 L·atm/mol·K)(300.15 K)

For the final state: P2V1 = nRT2 (5.1 MPa)(100 dm³) = n(0.0821 L·atm/mol·K)(340 K)

Now, we can solve for the number of moles (n) in both equations:

For the initial state: n = (5 MPa)(100 dm³) / (0.0821 L·atm/mol·K)(300.15 K)

For the final state: n = (5.1 MPa)(100 dm³) / (0.0821 L·atm/mol·K)(340 K)

Next, we can calculate the difference in the number of moles of gas between the initial and final states:

Δn = n(final) - n(initial)

Finally, we can calculate the mass of the gas that escaped from the balloon using the molar mass of helium (4.0026 g/mol):

Mass of gas = Δn * molar mass of helium

Please note that the calculations provided above are based on the ideal gas law and assume that the gas behaves ideally. In reality, there may be deviations from ideal behavior, especially at high pressures and low temperatures.