Question

Пожалуйста очень Срочно!!! повесят((( умоляю))) На укр| Визначте роботу і зміну внутрішньої енергії кисень (О2), якщо його об’єм збільшився від 10 до 20 л. Тиск є незмінним і дорівнює 4ꞏ105 Па. На рус| Определите работу и изменение внутренней энергии кислород (О2), если объем его увеличился от 10 до 20 л. Давление является неизменным и равно 4ꞏ105 Па.

Answer 1

Ответ: 4 кДж          10 кДж

Объяснение:

Answer 2

Calculation of Work and Change in Internal Energy of Oxygen

To determine the work and change in internal energy of oxygen (O2) when its volume increases from 10 to 20 liters, with a constant pressure of 4 x 10^5 Pa, we can use the ideal gas law and the first law of thermodynamics.

The ideal gas law states that for an ideal gas, the product of pressure (P) and volume (V) is proportional to the number of moles (n) and the absolute temperature (T). Mathematically, it can be expressed as:

PV = nRT

Where: P = pressure V = volume n = number of moles R = ideal gas constant T = absolute temperature

In this case, the pressure is constant, so we can rewrite the ideal gas law as:

V1 / T1 = V2 / T2

Where: V1 = initial volume T1 = initial temperature V2 = final volume T2 = final temperature

Since the pressure is constant, the temperature remains constant as well. Therefore, we can simplify the equation to:

V1 = V2

Now, let's calculate the work done and the change in internal energy.

Calculation of Work (W)

The work done on or by a gas can be calculated using the equation:

W = P * (V2 - V1)

Where: W = work done P = pressure V2 = final volume V1 = initial volume

In this case, the pressure is 4 x 10^5 Pa, and the initial volume is 10 liters while the final volume is 20 liters. Plugging these values into the equation, we get:

W = (4 x 10^5 Pa) * (20 L - 10 L)

Now, let's calculate the value of work.

Calculation of Change in Internal Energy (ΔU)

The first law of thermodynamics states that the change in internal energy (ΔU) of a system is equal to the heat added to the system (Q) minus the work done by the system (W). Mathematically, it can be expressed as:

ΔU = Q - W

In this case, the pressure is constant, so there is no heat transfer (Q). Therefore, the change in internal energy is equal to the negative of the work done. Mathematically, it can be expressed as:

ΔU = -W

Now, let's calculate the change in internal energy.

Calculation:

Given: Initial volume (V1) = 10 L Final volume (V2) = 20 L Pressure (P) = 4 x 10^5 Pa

Using the equation for work:

W = (4 x 10^5 Pa) * (20 L - 10 L)

Calculating the value of work:

W = 4 x 10^5 Pa * 10 L = 4 x 10^6 J

Since the change in internal energy (ΔU) is equal to the negative of the work done:

ΔU = -W = -4 x 10^6 J

Therefore, the work done on the oxygen gas is 4 x 10^6 J, and the change in internal energy is -4 x 10^6 J.

Please note that the calculations provided above are based on the given information and assumptions.