Based on Charles's law, which of the following statements is true for an ideal gas at constant pressure and mole amount? The number of collisions is independent of volume. The number of collisions decreases with an increase in volume. Volume is directly proportional to absolute temperature. Volume is inversely proportional to absolute temperature. Based on the kinetic theory, which statement is true? The particles of matter are stationary. The matter is composed of very small particles. Matter is made up of only charged particles. The particles of matter have zero kinetic energy.
Ideal and Real Gases
Ideal gases obey conditions of the general gas laws under all states of pressure and temperature. Ideal gases are also named perfect gases. The attributes of ideal gases are as follows,
Gas Laws
Gas laws describe the ways in which volume, temperature, pressure, and other conditions correlate when matter is in a gaseous state. The very first observations about the physical properties of gases was made by Robert Boyle in 1662. Later discoveries were made by Charles, Gay-Lussac, Avogadro, and others. Eventually, these observations were combined to produce the ideal gas law.
Gaseous State
It is well known that matter exists in different forms in our surroundings. There are five known states of matter, such as solids, gases, liquids, plasma and Bose-Einstein condensate. The last two are known newly in the recent days. Thus, the detailed forms of matter studied are solids, gases and liquids. The best example of a substance that is present in different states is water. It is solid ice, gaseous vapor or steam and liquid water depending on the temperature and pressure conditions. This is due to the difference in the intermolecular forces and distances. The occurrence of three different phases is due to the difference in the two major forces, the force which tends to tightly hold molecules i.e., forces of attraction and the disruptive forces obtained from the thermal energy of molecules.
Based on Charles's law, which of the following statements is true for an ideal gas at constant pressure and mole amount?
The number of collisions is independent of volume.
The number of collisions decreases with an increase in volume.
Volume is directly proportional to absolute temperature.
Volume is inversely proportional to absolute temperature.
Based on the kinetic theory, which statement is true?
The particles of matter are stationary.
The matter is composed of very small particles.
Matter is made up of only charged particles.
The particles of matter have zero kinetic energy.
Bella observes that the gas-filled tire of her bicycle becomes a little deflated when she keeps the bicycle outside in cold weather. Which of the following laws is used to understand the behavior of the gas and why?
The low temperature outside lowers the volume of the gas according to Charles's law because this law describes how a gas will behave at constant pressure.
The low temperature outside increases the volume of the gas according to Charles's law because this law describes how gas will behave at constant pressure.
The low temperature outside lowers the volume of the gas according to Boyle's law because this law describes how gas will behave when the number of moles remains constant.
The low temperature outside increases the volume of the gas according to Boyle's law because this law describes how gas will behave when the number of moles remains constant.
A substance in a specific
It is highly compressible.
It also has a definite shape.
Its particles slide past one another.
Its intermolecular forces are of high strength.
Read the chemical equation.
N2 + 3H2 → 2NH3
Using the volume ratio, determine how many liters of NH3 is produced if 4.2 liters of H2 reacts with an excess of N2, if all measurements are taken at the same temperature and pressure?
2.8 liters
3.2 liters
5.4 liters
6.3 liters
Based on the kinetic molecular theory, which of the following statements is correct about a sample of gas at a constant temperature and volume?
The net kinetic energy of its particles decreases due to collisions.
The net kinetic energy of its particles increases due to collisions.
It has a constant average kinetic energy.
Its average kinetic energy is always zero.
Which statement is true about the particles of a gas when the gas changes into a liquid?
They stop vibrating.
They move farther apart.
Their kinetic energy increases.
The attractive force between them increases.
The pressure of a gas is 1.0 atm, the volume is 3.0 L, and the temperature is 200 K. A chemist changes one factor while keeping another constant so that the new pressure is 2.0 atm. Which of the following could be the new conditions?
The final volume is 6.0 L, while the temperature is kept constant.
The final temperature is 100 K, while volume is kept constant.
The final volume is 4.0 L, while the temperature is kept constant.
The final temperature is 400 K, while volume is kept constant.
Two glasses labeled A and B had equal amounts of water. Ted heated the water in one of the glasses. He then put two drops of food coloring into each of the two glasses. The table shows the time taken by the food coloring in the two glasses to spread out.
Food Coloring Experiment
| Glass | Time |
|---|---|
| A | 25 seconds |
| B | 6 seconds |
Which of the following statements is correct?
The water in Glass B was heated; therefore, the particles in Glass B have greater kinetic energy and move faster.
The water in Glass A was heated; therefore, the particles in Glass A have greater kinetic energy and move faster.
The water in Glass B was heated; therefore, the particles in Glass B move slower.
The water in Glass A was heated; therefore, the particles in Glass A move slower.
Which of the following most likely happens when the temperature of a gas increases?
The number of collisions of gas particles remains the same.
The number of collisions of gas particles increases.
The pressure of the gas remains the same.
The pressure of the gas decreases.
A 2.36-gram sample of NaHCO3 was completely decomposed in an experiment.
2NaHCO3 → Na2CO3 + H2CO3
In this experiment, carbon dioxide and water vapors combine to form H2CO3. After decomposition, the Na2CO3 had a mass of 1.57 grams.
- Determine the mass of the H2CO3 produced.
- Calculate the percentage yield of H2CO3 for the reaction. Show your work or describe the calculation process in detail.
What happens to the average kinetic energy of gas when the particles of the gas collide against each other at a constant temperature and volume? Explain your answer.
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