Question

СРОЧНО!!!! два моля идеального одноатомного газу ізохорно нагрівають в циліндрі об'ємом 4 л. Як при цьому змінилися внутрішня енергія і температура газу, якщо тиск збільшився від 40 кПа до 80 кПа

Answer 1

Ответ:

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Объяснение:

Answer 2

When an ideal monoatomic gas is heated isochorically (at constant volume), its internal energy and temperature change. In this case, the pressure of the gas increased from 40 kPa to 80 kPa while the volume remained constant at 4 L. Let's discuss how the internal energy and temperature of the gas changed.

Internal Energy Change:

The internal energy of an ideal gas is directly proportional to its temperature. When the gas is heated isochorically, the change in internal energy can be calculated using the equation:

ΔU = nCvΔT

Where: - ΔU is the change in internal energy - n is the number of moles of gas - Cv is the molar heat capacity at constant volume - ΔT is the change in temperature

For an ideal monoatomic gas, the molar heat capacity at constant volume (Cv) is given by:

Cv = (3/2)R

Where R is the ideal gas constant.

Since the volume is constant, the change in internal energy can be calculated as:

ΔU = (3/2)nRΔT

Temperature Change:

To find the change in temperature, we can rearrange the equation for internal energy change:

ΔT = ΔU / [(3/2)nR]

Now let's calculate the change in internal energy and temperature using the given values.

Given: - Initial pressure (P1) = 40 kPa - Final pressure (P2) = 80 kPa - Volume (V) = 4 L

To calculate the number of moles (n), we can use the ideal gas equation:

PV = nRT

Rearranging the equation, we have:

n = PV / RT

Substituting the given values, we can calculate the number of moles.

Now we can calculate the change in internal energy (ΔU) and the change in temperature (ΔT) using the formulas mentioned above.

Please wait a moment while I perform the calculations.