What are 3 characteristics of a gas?
Gases have three characteristic properties: (1) they are easy to compress, (2) they expand to fill their containers, and (3) they occupy far more space than the liquids or solids from which they form. An internal combustion engine provides a good example of the ease with which gases can be compressed.
What is the difference between a real gas and an ideal gas quizlet?
Terms in this set (10) Real gases do not exhibit attractive or repulsive forces between the particles. False, Ideal gases do not exhibit attractive or repulsive forces between the particles. Real gases behave like ideal gases when they are under high pressure and are at low temperatures.
Which of the following statement is true for ideal gas?
According to the ideal gas law, it is true that pV=nRT p V = n R T , where R is the ideal gas law constant.
Why do real gases deviate from the ideal gas laws at low temperatures quizlet?
gases deviate from ideal behavior because the molecules are moving slower. This allows for intermolecular forces between neighboring molecules or atoms to take effect.
Why do gases deviate from the ideal gas law at high pressures quizlet?
At high pressures, the two factors that cause deviations during ideal law calculations are volume and intermolecular attractions. With volume, real gases tend to liquify rather than go to zero volume. With intermolecular attractions, they become more significant.
Which of the following conditions will cause a gas to deviate from ideal?
The Effect of Intermolecular Forces. At high pressures and low temperatures, intermolecular forces between gas particles can cause significant deviation from ideal behavior.
Under what conditions of temperature and pressure do real gases differ most from ideal gas?
As the temperature of an enclosed gas increases, the pressure increases, if the volume is constant. What is the relationship between the temperature and pressure of a contained gas at constant volume? Real gases differ most from ideal gases at low temperature and high pressures.
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