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Which gas of the following will have the greatest deviation from ideal behavior H2 F2 Br2 and Cl2?
The two factor Van de Waals gave as correction for real molecules instead of the ideal gas, are the size of the molecule, and the amount of attraction between the molecules. The larger the size of the molecule for the greater the deviation from an ideal gas, clearly bromine wins here since it has the biggest size of its atom. The amount of attraction between molecules is directly proportional to the boiling point of the liquid made from those molecules, and again bromine wins here since its has the highest boiling point. So bromine has the greatest deviation from ideal gas behaviour.
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How can you use ideal in a sentence?
This is an ideal example!
What are the essential characteristics of an ideal text book of general science?
an ideal text book of science must have the following for the following reasons: 1.diagrams: For a better pictorial representation. 2.definitions:for better understanding in shorter limes. 3.examples:for proving the context in practical life, and better understanding. 4.bright colours: for increasing interest in reading the book. 5.colourful pages reader's interest. sorry if it doesn't meets your requirements.......
A 75.0L steel tank at 20.00 degree C contains acetylene gas C2H2 at a pressure of 1.39atm Assuming ideal behavior how many grams of acetylene are in the tank?
=26 x (pressure in kpa times 75.0)/(8.31 x 293)
Is water an ideal fluid?
Ideal Fluid:An incompressible fluid that has no internal viscosity.
What is the ideal temp in a freezer in Fahrenheit?
Zero
How does temperature impact the deviation of a gas from ideal behavior?
Temperature impacts the deviation of a gas from ideal behavior by affecting the speed and energy of gas particles. Higher temperatures can cause gas particles to move faster and collide more frequently, leading to greater deviations from ideal gas behavior.
Which molecule among the following would exhibit the most ideal behavior?
The molecule that would exhibit the most ideal behavior among the options provided.
Why helium and hydrogen show less deviation from ideal behavior than other gases?
Helium and hydrogen show less deviation from ideal behavior because they are both light gases with weak intermolecular forces. These weak forces result in minimal interactions between gas particles, which closely resembles the assumptions of an ideal gas behavior. Additionally, the small size and simplicity of helium and hydrogen molecules make them less likely to experience significant deviations under normal conditions.
What are two types of non ideal solutions?
They are two types of Non-Ideal solutions. They are (i) Non-Ideal solutions showing positive deviation (ii) Non-ideal solutions showing negative deviation
Why is butane gas not an ideal gas?
Butane gas is not an ideal gas because it exhibits some deviation from the ideal gas law at high pressures and low temperatures. This is due to the intermolecular forces present in butane molecules that influence their behavior. Additionally, butane gas can liquefy at relatively low temperatures, further deviating from ideal gas behavior.
What should be the ideal standard deviation for a process?
For a process, the ideal SD is 0.
What are two types of non-ideal solutions?
Two types of non-ideal solutions are ideal mixtures and non-ideal mixtures. Ideal mixtures follow Raoult's Law, where the vapor pressure of each component is directly proportional to its mole fraction in the solution. Non-ideal mixtures do not obey Raoult's Law due to interactions between the components, such as deviations from ideal behavior or the formation of new chemical species.
How do you calculate the compressibility factor for a given gas mixture?
The compressibility factor for a gas mixture can be calculated by dividing the observed pressure of the gas mixture by the ideal gas pressure at the same temperature and volume. This ratio helps to account for the deviation of real gases from ideal gas behavior.
When do gases deviate from ideal behavior?
Gases deviate from ideal behavior at high pressures and low temperatures.
Why real gases deaviat from ideal behaviou?
It is assumed that Ideal Gases have negligible intermolecular forces and that the molecules' actualphysical volume is negligible. Real Gases have the molecules closer together so that intermolecular forces and molecules' physical volumes are no longer negligible. High pressures and low temperatures tend to produce deviation from Ideal Gas Law and Ideal Gas behavior.
Which of the following properties minimizes the differences between an ideal gas and a real gas?
- Weak intermolecular forces -Low density
Why do gases deviate from ideal behavior at high pressure?
Gases deviate from ideal behavior at high pressure because the molecules are closer together, leading to stronger intermolecular forces that affect their behavior.
