Oxygen weighing 16 g is compressed adiabatically, as a result

Oxygen weighing 16 g is compressed adiabatically

This product is a description of a physical problem describing the process of compressing oxygen weighing 16 g. The problem is to determine the change in the internal energy of the gas and the work expended on compressing the gas.

The description is written in an academic style and contains formulas that determine the change in the internal energy of the gas and the work expended on compressing the gas. It is intended for students and professionals in the field of physics.

The design is written using HTML code using heading and list tags to make the text easier to read and understand.

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Product description:

Oxygen is sold in 16 g weights, which can be compressed adiabatically. When a gas is compressed, its temperature increases from 300 K to 800 K. For this process, it is necessary to determine the change in the internal energy of the gas and the work expended on gas compression.

To solve this problem, you can use the following formulas and laws:

• The first law of thermodynamics: ΔU = Q - W, where ΔU is the change in internal energy of the gas, Q is the amount of heat transferred to the gas, and W is the work done on the gas.
• An adiabatic process is a process in which there is no heat exchange between the gas and the environment, that is, Q = 0.
• The ideal gas law is: PV = nRT, where P is the pressure of the gas, V is its volume, n is the amount of substance in the gas, R is the universal gas constant, and T is the absolute temperature of the gas.

Using these formulas and laws, you can get the following results:

• Change in internal energy of the gas: ΔU = 0, since the process is adiabatic and is not accompanied by heat exchange.
• Work expended on gas compression: W = -ΔE = -(E2 - E1), where E1 and E2 are the initial and final energies of the gas, respectively. Using the ideal gas law, we can express the initial volume V1 and final volume V2 of the gas, as well as the initial pressure P1 and final pressure P2 of the gas. Thus, the work can be expressed as W = -nR(T2 - T1)/(1-γ), where γ is the adiabatic exponent equal to the ratio of the molecular heat capacities of the gas at constant pressure and constant volume.

So, for this problem, the change in the internal energy of the gas is zero, and the work expended on gas compression can be calculated using the formula W = -nR(T2 - T1)/(1-γ), where T1 = 300 K, T2 = 800 K, n = mass of gas/molar mass of oxygen, R = universal gas constant, and γ for a monatomic gas (such as oxygen) is 5/3.

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