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For the last Question, N204 = 2N02; 1)Temp = Since, its a decomposition reaction [DIMER - MONOMER] heat should be supplied to it, which means It is ENDOTHERMIC, there temp should be high 2)Pressure = should be lower as, high pressure means eq. shifts towards lower mole side 3)Inert material = should be Added as, eq shifts to the side having more moles of substance
Ans for the last question: Pressure = low Inert material should be added. Is it exo or endo, it,s not mentioned in the equation , so, temp isn't defined.
It is decomposition reaction...so heat should be supplied to break the compound...this information will most likely be not given in the question, so you have to know it...hope this helps
N2O4 is being converted to NO2.. Dimer to monomer ..i.e. heat has to be supplied which implies forward direction reaction is endothermic. Hence increasing the temperature will yield more NO2
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Answer for the last question... 1) Increase the concentration of N2O4 2) high temperature is required 3) Low pressure is required 4) addition of inert material at constant pressure is also required... Thank you sir, you are doing a great job...
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Temperature : High (since it is an endothermic reaction although not mentioned) Pressure: Low Inert material : we will use as it shifts the equilibrium forward towards more no of moles.
commando offical At 1:01:10 sir stated that if no delta H is given, the reaction is forward. So in order to increase the production of NO2 temperature has to be increased.
@@bijitdas208 Yes,here we don't know either it is exothermic or endothermic,so go by the basic thumb rule.....that is on high temp molecules will gain kinetic energy hence the molecules can easily collide with each other thus resulting NO2.... or do generally consider it to be endothermic [PLEASE DO CORRECT ME IF IAM WRONG]
There is one more point . . . 5. The addition of catalyst: it doesn't effect the concentration of equilibrium mixture, as it only increases or decrease the time to attain equilibrium.
As catalyst is inert to the reaction (because it increases the rate of reaction but doesn't itself react with any product /reactant) , it is hence included in 4th point
answer of homework question PRESSURE ----- PRESSURE SHOULD BE LOW TEMP----- TEMPERATURE SHOULD BE HIGH AS ENERGY IS REQUIRED TO BREAK BOND --- N204 IS DIMER OF NO2 AND ENERGY IS REQUIRED TO BREAK THE N---N BOND SO THE RXN IS ENDOTHERMIC AND TEMP SHOULD BE HIGH INERT MATERIAL---- SHOULD BE ADDED
Temp:- not defined cuz it's not that reaction is endo or exo. Pressure :- low Inert gas should be added. *Sir aap hum bachcho ke liye vardan ho.* 🙏🏻🙏🏻😁😁
Reaction endothermic hogi na....kyu ki bond break ho rhe h......! Or hume energy deni pdegi(endothermic) bond break krane k lie..... Hence to favour endothermic reaction we hv to Inc the temperature.. 🙋🏼♂️🙋🏼♂️
Hey but if we increase the temp pressure also rises n if pressure increases the equilibrium shifts backward so we can say that the conditions are: Low temp Low pressure Addition of inert gas
Guys have u noticed,at 26:00 jo sir ne example dia tha usme reaction ka direction phle forward bataya tha,but after some seconds sir ne usko edit krke backward krdia.?isse ye pta chlta hai sir bhi kbi kbi confuse hote hai.no problem sir hota hai : )
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I usually understand this principle by using the " Mad man method " where it is said that mad man will do the opposite you do.. You increase pressure, mad man tries to decrease it, he goes there.. You increase conc., mad man tries to decrease it, he goes to less moles... You increase temp. , mad man tries to decrease it, he goes to less temp. system... like that it can be easy..
@@RajendraKumar-br9gj decomposition reaction mein heat is required to break bonds so reaction will proceed in forward direction as N2O4 + ∆ ------> 2NO2 Reaction will proceed in the direction of heat absorption (NO2 production increases) 😊
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Temp not defined Pressure low means high vol therefore no of mole production high Inter gas c vol no effect And c pressure more no of moles therefore in the forward direction sir❤
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38:16 sir has committed mistake there, as in habers process the forward reaction is exothermic and not endothermic so low temp is favorable instead of high temp.
1. Temprature high (bcz : N2O4 do heat absorb than convert in NO2) 2. Pressure low 3. Inert material was like advantage for this reaction 🙏... ..........🙇 Tx so much sir 🙇.......... .....🙇for solve all type of doubts🙇.......
N2O4 is a stable than NO2 ( Dimer), hence Backward reaction Energy releases - Exothermic therfore low temp is favoured for backward reaction. But Question is about Forward reaction . Obviously forward reaction is endothermic Hence temp must be high @Aakash Nigam
Favorable conditions for the last reaction :- 1 : By increasing the concentration of [N2O4] or by removing [NO2] 2 :Pressure should be low 3 :Can't define temperature 4: at ∆P=0 then forward reaction (which will not help in increasing the production )
Actually physics lectures' questions are pretty hard which definitely is an issue with my IQ but concept wise i feel he has benefited me A LOT in Chemistry than physics. In a nutshell , he's definitely one of the best teachers on RU-vid platform.
@@ksuhanidas3226 Arrey sir ne temp., pressure aur inert material ke baare pucha he, to Maine bata diya to, ha bas bola he ki conc. to hum bata denge kyunki easy he to woh mana kiya he
Home work Temp- high, ( heat acts as rectant in the decomposition of dinitrogen tetroxide, the reaction is endothermic) Pressure_low Inert material -needed with constant pressure
@@naveensoni5771N2O4->2NO2 mai 100% n2o4 colorless at -11 degree celsius and 100% brown fumes of No2 at 140 degree Celsius so obviously this reaction is endothermic that's why high temperature is favorable.
Temp---decrese Pressure---decrese Ya I know heat is not given And even not that it is exo or Endo But pressure directly proportional ...to temp And even Inert material should be added 💖🔥 Thx sir for your love and support 👍