Statements on ideal gases

• Janiceleong26
In summary, an ideal gas is a theoretical gas that follows the ideal gas law, which relates pressure, volume, temperature, and moles of gas. It is used in various fields and in the design of gas-powered systems. The assumptions of ideal gases are no intermolecular forces, no volume, and constant particle motion. Real gases differ in that they do have intermolecular forces and volume, and require specific equations to account for these differences.

The Attempt at a Solution

I chose 1&2, but all three are correct. I thought for a constant pressure, if temperature is doubled, then the volume would doubled too? As P=V/T ?

3 is not a correct statement. Change from 25°C to 50°C is not doubling the temperature. Change from 100 K to 200 K is.

Borek said:
3 is not a correct statement. Change from 25°C to 50°C is not doubling the temperature. Change from 100 K to 200 K is.
Sorry I typed wrongly, I chose 1,2&3, but ans. is 1&2.
oh.. Right, they must be in Kelvins. Thanks again

1. What is an ideal gas?

An ideal gas is a theoretical gas that conforms to the ideal gas law, which describes the relationship between pressure, volume, temperature, and moles of gas. It is assumed to have no intermolecular forces and occupy no volume, making it easy to calculate and predict its behavior.

2. What is the ideal gas law?

The ideal gas law is a mathematical equation that describes the relationship between pressure (P), volume (V), temperature (T), and the number of moles (n) of an ideal gas. It is written as PV = nRT, where R is the universal gas constant.

3. How is the ideal gas law used in real life?

The ideal gas law is used in various fields, such as chemistry, physics, and engineering, to predict the behavior of gases in different conditions. It is also used in the design and operation of gas-powered systems, such as engines and refrigeration systems.

4. What are the assumptions of ideal gases?

The assumptions of ideal gases are that they have no intermolecular forces, occupy no volume, and their particles are in constant, random motion. These assumptions make it easier to calculate and predict the behavior of gases under different conditions.

5. How do real gases differ from ideal gases?

Real gases differ from ideal gases in that they do have intermolecular forces, occupy a small volume, and their particles can interact with each other. This can cause deviations from the ideal gas law at high pressures and low temperatures. Real gases also have specific properties, such as compressibility factor and van der Waals equation, that are used to account for these deviations.

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