11th Std - Chemistry | Unit 7 - Question Answer Marked In Book

[00:00:00]Greetings everyone. Welcome to our channel. The video 11th standard chemistry unit number two, write brief answer to the following questions. First one, state the first law of thermodynamics. Page number 195, 195.

[00:00:24]The first law of thermodynamics the first law of thermodynamics known as the Okay. Now, the mathematical statement of the first law I've been to system ready to go 26th answer.

[00:00:40]Then 27, define Hess's law of constant heat summation. Page number 207, 207.

[00:00:50]See the enthalpy change of a reaction off the year.

[00:00:59]Then 28, explain intensive properties with two examples. Page number 189.

[00:01:06]189.

[00:01:08]Intensive properties in heading off the year. The property that is independent in the examples etc. 28 question answer intensive properties.

[00:01:18]Then 29, what is the usual definition of entropy? What is the unit of entropy?

[00:01:25]Page number 210.

[00:01:30]210.

[00:01:32]Entropy order definition but they cannot right side first left side entropy is a measure of the other end of the start button you cannot right side left system or you cannot other you cannot other DS equal to other other second point unit of the year. Second point the entropy is is equal to heat energy exchanged divided by the temperature at which the exchange takes place. Therefore, the SI unit of entropy is JK - 1.

[00:02:14]Predict the feasibility of a reaction when both delta H and delta S positive and delta H delta S negative and delta H decreases but delta S increases. Page number 216 in the tabular column 216 la Well, at low temperature and a high temperature non-spontaneous spontaneous second question but delta H delta S both negative in the 31st in the learning 31st delta H decreases delta S delta S increases in the first second third 31st corner answer.

[00:02:54]Then 32nd define Gibbs free energy. Page number 214 Gibbs energy.

[00:03:03]Gibbs energy 214 available energy other than Gibbs energy again Gibbs free energy is the energy available to do useful work at constant temperature and pressure. G equal to H minus TS. So H is enthalpy, T temperature, S entropy. G equal to H minus 2S so the definition Gibbs free energy is the energy available to do useful work at constant temperature and pressure. Okay, 33.

[00:03:40]33 define enthalpy of enthalpy of combustion page number 200 200 enthalpy of heat of combustion so the heat of combustion the start burning >> So the heat of combustion on the start money del H C 2.

[00:04:01]Then Question number 34. Define molar heat capacity give its unit page number 201.

[00:04:08]Molar heat capacity right side second paragraph molar heat capacity It is strike out by the molar heat capacity.

[00:04:20]35 Define the calorific value of food.

[00:04:24]What is the unit of calorific value page number 206?

[00:04:28]206 but you know calorific value So calculation of calorific value of food and fuel earlier. The calorific value is defined as the amount of heat produced other than that of the six lines. It is usually expressed in C L G minus one.

[00:04:45]Okay.

[00:04:47]So calorific 35 answer 36 Define enthalpy of neutralization page number 206. Heat of neutralization heading The heat of neutralization learn the dilute solution like them. So on the five lines edited I look at the H plus aqueous either you going to 36.

[00:05:11]Okay. Next What is lattice energy page number 208?

[00:05:16]What is lattice energy lattice energy lattice energy lattice enthalpy in the six lines up there. Lattice energy is defined as the amount of energy required to completely remove the constant ions crystal lattice to an indefinite distance from one mole of crystal. It is also referred to as lattice enthalpy. 37 kind of answer.

[00:05:39]Then 38 What are the state and path functions give two example page number 190 and 191.

[00:05:48]State functions and uh path functions So, state function heading here at the bottom of the second line. A state function is a thermodynamic property other than the state is reached. It will become 38. It is going to example. Right side example again any two examples will be written so any three will be taken.

[00:06:06]After path functions, path functions left in the four lines up there ready to example work heat. Okay, now 38 going to answer. State function and path functions.

[00:06:16]Next.

[00:06:19]39, give Kelvin statement of second law of thermodynamics. Page number 210.

[00:06:25]Kelvin Kelvin statement of second law of thermodynamics 210 page number.

[00:06:34]So, Kelvin-Planck state Kelvin-Planck statement.

[00:06:40]The Kelvin-Planck statement here. It is impossible other than the start burning.

[00:06:45]Fifth line left cold sink and other than the 39 question going to answer other than the uh Kelvin statement of second law of thermodynamics. Then 40, the equilibrium constant of a reaction is 10. What will be the sign of del G? Will this reaction be spontaneous? Uh on the page here at the end of the book left.

[00:07:05]Okay, now free army or paper left and I'll copy going to copy going to copy.

[00:07:09]So, the equilibrium constant 10 and put it again here. So, del G equal to minus 2.393 RT 10 g uh K at the equilibrium K equilibrium put it at 10 and put it again. Next del G but you know negative value so the reaction will be spontaneous. So, you can copy going to copy going to 40 40 going to answer. 41 Enthalpy of neutralization is always constant when a strong acid is neutralized by a strong base account for the statement. Page number 206. Six. is in the page 206.

[00:07:45]In the the right side paragraph strong acids and strong bases completely ionized in aqueous solution clear.

[00:07:55]Second point when they del H is always constant for strong acid strong base reactions. Because only H+ and OH- ions combine to form water.

[00:08:09]41 going to answer. Then 42, state the third law of thermodynamics page number 218.

[00:08:17]218 page number third law of thermodynamics 218 there the third law of thermodynamics clear other than this start burning crystalline state where you can 42nd going to answer third law of thermodynamics.

[00:08:33]Then 43, write down the Born-Haber cycle for the formation of CaCl2. The same page.

[00:08:41]Born-Haber CaCl2 Born-Haber in the going to there in the going to there Born-Haber there uh in the going to there in the going to there NaCl in the money CaCl2 So in the CaCl2 Born-Haber cycle for the formation of CaCl2. Born-Haber cycle is used to calculate the lattice enthalpy of CaCl2.

[00:09:11]In the going to there CaS So in the going to there in the going to there del H1 enthalpy change for the sublimation of CaS to CaG. Then del H2 but in the enthalpy change for dissociation of Cl2 to 2Cl in the going to there H3 in the ionization energy for Ca to Ca2+ Then del H4 in the electron in affinity for the conversion of 2 Cl 2 2 Cl minus.

[00:09:43]Then, delta H 5 lattice enthalpy for the formation of solid CaCl2.

[00:09:48]So, delta Hf equal to delta H1 plus delta H2 plus delta H3 delta H4 and then delta H5. Okay, now. So, it up here copy bunny corner number CaCl2 good get to the corner.

[00:09:59]44 corner question but you know, identify the state and path functions out of the following. Enthalpy of being the function of fun and a function of being a state function. Entropy it will state function heat on the path function. Temperature state function work one day path function free energy state function. Okay, now. See, state function the enthalpy entropy temperature free energy. Then, path function the heat work.

[00:10:28]Then, 45th.

[00:10:31]State the various statements of second law of thermodynamics. Page number 210 and 211.

[00:10:42]210.

[00:10:46]Number get to get the various statements of second law of thermodynamics. So, various statements and the first Kelvin Planck statement already number but show me that second law of thermodynamics and then cold sink where you go first and you go in the Kelvin Planck statement and in heading put it there. And the various statement get to get the Clausius statement put it is impossible and the some work in second statement Clausius statement. Next entropy statement put it there. The entropy of an isolated system increases during a spontaneous process. 45th question corner answer. So, you know, so Kelvin statement one and Clausius statement one and entropy statement 45th corner answer. 46 what are spontaneous reactions? What are the conditions for the spontaneity of a process? 213 page number 213.

[00:11:33]In the First is spontaneous. Right side Gibbs free energy fourth line reaction that occurs spontaneous reaction four lines 46. Next page number 215 215 criteria for spontaneity of a process 216 the 46 kind of answer I want to criteria conditions for the spontaneity of a process kind of answer List the characteristics of internal energy page number 191 characteristics of 191 characteristics of internal energy kind of answer So first point the internal energy extensive property kind of answer Second point the internal energy state function second point Third point Fourth point as fifth sixth Okay now 47 kind of answers six points characteristics of internal energy then 48 explain how heat absorbed at constant volume is measured using bomb calorimeter with a neat diagram page number 202 and 203 204 202 kind of answer See.

[00:13:03]And that measurement first start heat evolved at constant volume is measured in a bomb calorimeter 48 first kind of answer And the apparatus set up put it in the paragraph kind of answer four lines apparatus set up in the diagram with parts order And then experiment a weight amount weight amount of the substance start burning electrical heating kind of answer Then calculation a known amount of then calculation a known amount of combustible so the length of 203 and then 204 RT so 48 going to answer then 49 calculate the work involved in expansion and compression process page number 193 and 194 193 193 work involved in second paragraph start for understanding pressure volume work start money to so I pray it a derivation of a pudding here in and a work involved in at the next page number 194 la the full of positive article 49 going to answer then question number 50 derive the relation between H and U for an ideal gas explain each term involved in the equation page number 197 and 198 important questions first midterm upload money to so I don't link one WhatsApp channel book back questions important questions PDF model question paper it all of me 11 standard biomax group so other than you go eat in the subject refer money club page number 197 relation between enthalpy and internal energy area 50th question right side left the full of page number 198 RT in the vertical 50th going to answer so my channel is a subscriber because of coming days a lot of lesson of a book a lot of me upload money for then 50 question over 51 suggest and explain indirect method calculate lattice enthalpy of sodium chloride crystal page number 209 209 the cycle for determining the lattice enthalpy of NaCl as follows. Strike out money doing that.

[00:15:40]52, list the characteristics of Gibbs free energy 214 and 215.

[00:15:48]characteristics of Gibbs free energy 214 left Gibbs free energy is defined At the second point, the Gibbs free energy is an extensive property. Third point, it is a single-valued state function.

[00:16:05]For any system at constant temperature and pressure pressure and temperature external pressure by the call 52nd kind of answer Then 53 281 left page number the kind of answers So the reference money going important questions book in this question Can you buy the reference money going?

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