A gas mixture composed of 0.200 mol C2H4 and 4.81 g CH4 occupies a constant-volume container at a pressure of 2.00 atm. (There is no chemical reaction in the container.) Which of the following is/are false for this mixture? If the temperature in the container is raised, density of the mixture decreases. O If 0.200 mol C,H, is added to the container at constant temperature, the partial pressure of CH, does not change. O Mole fraction of CH, in the mixture is 0.600. O Partial pressure of C,H, in the mixture is 0.800 atm. O Molar mass of the mixture is 44.09 g/mol.
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.
Step by step
Solved in 4 steps with 1 images
