D. low pressure, high temperature. What does the R stand for in the ideal gas law (PV = nRT)? What is the effect on the volume of an ideal gas when the temperature is decreased from 700 K to 350 K at constant p
Planning tip: Asinara is ideally explored on a bike (or e-bike), which can be rented in Porto Torres or Cala Reale. The island is a popular spot between June and September, but in the low season, it is often empty. If you do visit during the low season, stock up on water and ...
Gases behave most ideally under conditions of... (a) low pressure and high temperature (b) high pressure and low temperature (c) high density and low temperature (d) high pressure and high temper Which of the following gases has a density of 0.716 g/L at STP? a) He b) CO_2 c) ...
Which of the following gases is expected to behave most ideally at a given temperature and pressure? a. H2O b. NH3 c. Xe d. He Which of the following gases is likely to behave the the least like an ideal gas at ...
In cold areas, keep the plant inside to protect it from low temperatures. Basil also does exceptionally well when grown hydroponically.Learn how to do it here. Is Basil a Perennial? Sweet basil, the edible herb that most people grow at home, is not perennial. It has to be replanted eve...
It is also worth noting that Fuji stands at just under 4000 metres in height. As you ascend, the air is notably thinner. It will affect most people and can have serious health implications for some visitors. Even in summer, temperatures can be cold – potentially below 0°C – near the...
Excluded volume effect vanishes and chains behave ideally. Where does the ideal chain model satisfy? On dealing with solutions, the osmotic pressure (渗透压) rather than pressure p becomes the quantity of interest: ... 3 3 2 2 1 m m m c A c A c A kT Concentration and temperature...
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Do all gases that behave ideally have the same molar volume? If any two gases are taken in different containers that are the same size at the same pressure and same temperature, what is true about the moles of each gas? Why is this true? Explain the following...