11th Std - Chemistry | Unit 6 - Book Back Exercise

[00:00:00]Greetings everyone. Welcome to our channel. The video 11 standard chemistry unit 6 gous state book question. So maximum questions because state boils page number 1660 at a given temperature the volume occupied by a fixed mass of a Gas is inversely proportional to its pressure proportionally constant.

[00:00:47]26th answer second name 27. Name two items that can serve as a model for Guzak's law and explain. So max 27th pressure in well inflated tire is almost constant but when temperature increases in summer summer days it increases the pressure and sometimes tires may bust.

[00:01:27]Okay. So, guns and other firing equipments are thrilling examples of Gail Luzak's law.

[00:01:37]When gun pin strikes, it ignites the gunpowder and this increases the temperature which in turn increases the pressure and bullet is fired from the gun.

[00:01:50]WhatsApp.

[00:01:52]So, WhatsApp unit 27th question answer then 28. Give the mathematical expression that relates gas volume and moles. Page number 165 hypothesis.

[00:02:15]Start the mathematical form. Sorry, the mathematical form may be expressed as right 28 answer.

[00:02:29]Then 29. What are ideal gases? In what way real gases differ from ideal gas?

[00:02:35]Page number 176. What are gases? Answer.

[00:02:42]Gases that obey the equation PV equal to NRT under all conditions are called ideal gases.

[00:02:52]Ideal gas, real gas. Ideal gases obey all gas laws under all conditions of temperature and pressure. Real gas obey gas law only at low pressure and high temperature. In what way?

[00:03:09]The volume occupied by the molecules is negligible as compared to the total volume occupied by the gas. The volume occupied by the molecules is not negligible as compared to the total volume of the gas. Either 2.6 ideal gas 29th answer. Okay. 30.

[00:03:29]No. Vanderwal's gas equation with a equal to0 cannot be liqufied.

[00:03:36]Page number 169 and then 271 169 30 question 30. The fact the fact that gases can be liqufied shows that the attractive force exist among molecules.

[00:04:00]Next point 271.

[00:04:09]Higher the value of A, greater the intermolecular force of attraction, easier the liquefaction.

[00:04:18]Third, if a equals zero, the Vanderval's force of attraction is very less and the gas cannot be liquified. Okay. So, three points on the page 271 169 + 271 and then third points.

[00:04:44]Suppose there is a tiny sticky area on the wall of container of gas molecules hitting this area stick there permanently. Is the pressure is greater or less than on the ordinary area of walls? So then 30 second answers explain the following observation answer. Then 33 gives suitable explanation.

[00:05:08]31st questionina. The pre the pressure on the sticky area is greater than the ordinary area of walls because molecules collide. The tiny sticky area on the wall of the container of gas moves faster as they get closer to sticky surface. But this effect is not permanent. Okay. So the pressure is greater than on the area of walls. Question. Second point 302. Explain the following observations.

[00:05:42]Aated water bottles are kept under water during summer.

[00:05:47]The airated water bottles are kept under the airated water bottle means the excess amount of oxygen and minerals present in the water which dissolved under certain pressure. Second point in summer the solubility of the gas and water is decreases because the rise in temperature and decreases the solubility. Hence more of gas will be present above the liquid surface and pressure of the gas becomes too high.

[00:06:12]The bottle may explode. So to avoid this the bottles are kept under water.

[00:06:18]At the second liquid ammonia bottle is cooled before opening the sealia. The vapor pressure of ammonia at room temperature is very high. Second point, cooling decreases the vapor pressure so that the liquid remains in the same state otherwise the bottle may explode.

[00:06:33]Hence the bottle is cooled before opening.

[00:06:37]See the tire of an automoil is inflated and the question according to Gay Luzak's law pressure is proportional to temperature. The point as the temperature increases the pressure also increases in summer. Hence pressure on the walls of the tube increases. If pressure inside is not kept low at the time inflation at high temperature the pressure may become so high the tire may bust.

[00:07:02]Uh further in winters due to lowering of temperature the pressure inside the tire may reduce the size of a weather balloon becomes larger and larger as it ascends up into the larger altitude according to boil as usual. Three points P inversely proportional to 1 by V. As we go to higher altitudes, the atmospheric pressure decreases. Thus, the pressure outside the balloon decreases. To regain equilibrium with the external pressure, the gas inside expands to decrease its pressure. Hence, the size of the balloon increase. So, WhatsApp 33 explanation. Gases don't settle at the bottom of a container. Solids and liquids would stay at the bottom as they are dense. But molecules and gases stay as far away from each other as possible.

[00:07:56]So gases don't settle at the bottom of a container.

[00:08:00]Gases diffuse through all the space available to them. Gases fill the entire space available to them because of low intermolecular space and weak intermolecular forces of attraction between the gas molecules. The weak forces allow them to flow freely in all the direction.

[00:08:18]34th patina suggest why there is no hydrogen H2 in our atmosphere. Hydrogen is the lightest element yet found. Thus when produced in free free form it rises above all the other gases to the top of the atmosphere. Hydrogen easily gains velocity required to escape earth's magnetic field. Then 35th.

[00:08:40]Explain whether explain whether a gas approaches ideal behavior or deviates from ideal behavior if it is comp if it is compressed to a smaller volume at constant temperature.

[00:08:55]Generally we learned that the behavior of a real gas approaches the behavior of an ideal gas under the conditions of low pressure and high temperature.

[00:09:03]At high pressure the gas molecules are close to each other. The volume occupied by the gas molecules is significant compared to the volume of its container.

[00:09:12]The interaction between gas molecules is significant. The gas deviate from ideal behavior.

[00:09:18]Question. The temperature is raised while keeping the volume constant. At high temperature, if a gas temperature is raised keeping the volume the constant, the pressure of the gas will increase. At high pressure the gas deviates from ideal behavior.

[00:09:32]Next Cana more gas is introduced into the same volume and at the same temperature. The more gases is introduced in the same into the same volume the gas approaches deviates from ideal behavior because the attractive forces between the molecules increases.

[00:09:48]So it becomes non ideal behavior.

[00:09:53]Then 36th. Which of the following gases would you expect to deviate from ideal behavior under conditions of low temperature? F_sub_2, CL2 or Br2.

[00:10:05]Explain. The larger the size of the molecules for the greater the deviation from an ideal gas. Clearly bromine has the biggest size than others. The amount of attraction between molecules is directly proportional to the boiling point of the liquid made from those molecules and bromine has the highest boiling point. So it has the greatest deviation from ideal gas behavior than F_sub_2 and CL2. F_sub_2 under the florine and CL2 chlorine.

[00:10:34]37 distinguish between diffusion and eusion. Page number 168 and 179. So diffusion 168 first point diffusion property of gas which involves the movement of the gas molecules molecules through another gases is called diffusion. First point, eusion.

[00:10:54]First point, eusion is another process in which a gas escapes from a container through a small hole. Very small hole.

[00:11:02]First point. Second point 170 179.

[00:11:13]Example in a closed room a perfume bottle is opened up. Diffusion. Example. Eusion.

[00:11:22]air escaping slowly through the pinhole in your tire. Okay, this is second point. Example on the second point.

[00:11:30]Next cans carry clear warning of heating the can. Why there are volatile liquids inside often LPG propellant. If these are heated, they will produce more vapor inside the can and which will make the pressure rise very quickly. At the room temperature, the lot of pressure created inside the can. Even though the cans are tested, they will burst if the pressure goes up too far.

[00:11:57]Answer 39. Would it be easier to drink water with the straw on the top of Mount Everest? It is difficult to drink water with your straw on the top of Mount Everest. This is because the reduced atmospheric pressure is less effective in pushing water into the straw at the top of the mountain because gravity falls off gradually with height. The air pressure falls off. There isn't enough atmospheric pressure to push the water up in the straw the way to the mouth.

[00:12:28]40. Write the Vanderwal's equation for a real gas. Explain the correction term for pressure and volume. 171 and 172.

[00:12:37]170.

[00:12:42]Vander found out the forces.

[00:12:47]Next 172 till this next volume correction calculate the correction term V= extended excluded volume right side Vanderwal's equation of state for Vanderwal's equation of state for real gases 40th question answer then 41 derive the values of critical constants in terms of Vanderwal constant 174 and 175 174 Best equation number one 6.2 numbers third equation equation 3 then 6.26 5 and 6.287 6.298 298 6.309 divide equation 9 by equation 8. Next equation uh 10 is substituted in equation 9 sorry 8 10 divided by substituted when equation 10 is substituted in equation 8 175 6.32 6.28 28 then 6.33.

[00:14:14]So equation 1 2 3 4 answer 41 42 43424 problems.

[00:14:37]So sorry. So best pages WhatsApp Next 42. Why do astronauts have to wear protective suits when they are on the surface of the moon? Astronauts must wear space suits whenever they leave a spacecraft and are exposed to the environment of space. In a space, there is no air to breathe and no air pressure. Space is extremely cold and filled with dangerous radiation without protection and astronauts would quickly die in space. Space suits are specially designed to protect astronauts from the cold radiation and low pressure. They also provide air to breathe.

[00:15:42]Finally, 43rd questionina. When ammonia combines with HCl, NH4 CL is formed as white dense fumes. Why do more fumes appear near HCl? NH3 plus HCl gives NH4 CLA. It can be explained by diffuse in property of gas. Ammonia and HCl solution are placed in a separate test tube. After some uh after some time the gases diffuses to meet and solid NH4 CL is formed near the HCl.

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