In lower temperatures, the molecules of real gases tend to slow down enough that the attractive forces between the individual molecules are no longer negligible. In high pressures, the molecules are forced closer together- as opposed to the further distances between molecules at lower pressures. This closer the distance between the gas molecules, the more likely that attractive forces will develop between the molecules. As such, the ideal gas behavior occurs best in high temperatures and low pressures. (Answer to your question: C) This is because the attraction between molecules are assumed to be negligible in ideal gases, no interactions and transfer of energy between the molecules occur, and as temperature decreases and pressure increases, the more the gas will act like an real gas.
Answer:
Q = 114349.5 J
Explanation:
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In this case, since this a problem in which we need to calculate the total heat of the described process, it turns out convenient to calculate it in three steps; the first one, associated to the heating of the liquid water from 40 °C to 100 °C, next the vaporization of liquid water to steam at constant 100 °C and finally the heating of steam from 100 °C to 115 °C. In such a way, we calculate each heat as shown below:
Thus, the total energy turns out to be:
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According to Kepler's second law of orbital motion, a plane's orbital speed changes , depending on how far it is from the sun. The closer a planet is to the sun, the stronger the sun's gravitational pull on it, and the faster the planet moves. The farther away from the sun, the weaker the sun's gravitational pull and the slower it moves in its orbit.
The orbit of a planet around the sun is not a perfect circle, but an ellipse - a flattened circle.
Qualitative observation. Which is data or information with your senses such as sight, taste, smell, and touch.
