CH # 01 Stoichiometry in one shot for NMDCAT students only

[00:00:01]Manalamkum subject chemistry students the chemistry syllabus the chemistry course lecture number one Number one concepts.

[00:00:32]More concepts.

[00:00:35]More than chemical equation.

[00:00:38]And chemical equation.

[00:00:42]Students equation students limiting reactant limiting reactant limiting reactant and X is reactant.

[00:01:12]limiting reactant and excess reactant.

[00:01:19]Yield of reaction.

[00:01:24]Yield of reaction.

[00:01:48]The lectures students leadership books 2026 National Dental College admission testific Special books topics the same text students concept.

[00:02:59]Concepts Quantitative unit.

[00:03:20]Quantitative unit.

[00:03:35]Substance 1 6.02 power 23 particles one 6.02 023 particles one of each substance the substance one will contain same number of particles will contains same number of particles the hurry of substance One more.

[00:04:21]Number one.

[00:04:38]One more. Small number.

[00:04:49]number of particles.

[00:04:57]Students is also called home.

[00:05:20]mass. Atomic mass of the express.

[00:05:41]For example, 23 23 g sodium 23 g sodium g of sodium.

[00:06:02]Students, one mole of sodium atom students amb of carbon 1 g atom of carbon one carbon 1 g atom of carbon students is also called molecule Reason students molecule For example, 18 students relative mass. Relative mass.

[00:07:48]The one mole of water.

[00:07:50]One mole of water.

[00:07:55]One g molecule of water. 1 g molecule of water.

[00:08:09]G formula.

[00:08:13]Mole is also called gram formula.

[00:08:18]Common formula 58.5 mass relative express 58.5 g initial Student 58.5 g 1 g for n students.

[00:09:20]Got molecule molecule.

[00:09:38]For example, Z the number of atoms of the number of atoms in 5 g atoms of carbon 5 g atoms of carbon 5 option number A 6.02 02 into 10^ 23 carbon 8 * D. Option number B 3.01 into 10^ 23 carbon 8 * D. Option number C 3 0 into 10 ^ 24 carbon A. Yeah. Option number D 12 into 10 ^ 24 carbon atom and so on. Now students the number of atoms and five atoms of carbon simple the number of moles of carbon moles carbon number of number of atoms graphite.

[00:11:10]Diamonds short formulas moles numbers 5 multip number 6.02 02 power 23 options figure 5 power 23 24 34 Number of atoms.

[00:12:38]Number of atoms of molecule.

[00:12:47]Number of bonds.

[00:12:49]Number of coalent bonds.

[00:12:55]Yeah. Number of ions in a formula unit. Formula unit number of ions.

[00:13:07]Number of electrons.

[00:13:13]Number n a number of example Number of carbon atoms.

[00:13:46]Number of carbon atoms in 180 g of glucose. For example, electrons.

[00:14:18]formula C6 H126 atoms six carbon atoms of hydrogen atoms. Number of hydrogen atoms and 180 g of glucose. Now students question number of bonds.

[00:15:01]Number of coalent bonds in five moles of water. Five moles of water given the number of Number of coalent bonds, number of atoms, number of electrons 6.02 into 10^ 23. So students for example solution 180 glucose number of carbon students 180 mass value number six NA of carbon atoms Answer students number of hydrogen atom 180.

[00:16:30]So hydrogen atom 12* number 12 NA hydrogen atoms.

[00:16:42]Question number three, number of moles of 10 NA of coalent bonds.

[00:17:13]Which of the following Which of the following contains greater number of carbon atoms? Contains greater number of greater number of atoms. Number of atoms number 32 gy number 44.8 8 D MQ of carbon dioxide gas same number of same number of atoms all have same number of atoms That's students.

[00:18:17]CH4 16 time four time 16 0.5 32 oxygen 44.8 dm 22.41 Number eight of methane for option number 0.5 N.5 CH4 2.5 NA at option number A to number of C option 44.8 multiples number 2 3 are six nt option number students The first papers 20 23 or 2024 students 2023 24 questions.

[00:21:11]The number of moles of carbon dioxide which contains 16 g of oxygen.

[00:21:30]O2 students 16* 2 32 carbon dioxide oxygen 16 g 16 g 32.5 g half oxygen 0.5.

[00:22:39]What is the mass of one mole of calcium carbonate? The calcium carbonate number 12 oxygen oxygen mass 16 40 + 12 + 48 dioxide 1 44 g C6 H6 benzene 78 g C6 H1206 C12 H22 011 180 uh 34 42 g 342 g for example 64 g how many moles are there in 60 g of sodium hydroxide 200 23 MD question students 60 sodium hydroxide numberal.

[00:24:37]Okay. The one hour 40.5 Students chemical equation questions.

[00:25:33]Students question the balance chemical equation.

[00:26:09]For example, N2 + 3 H2 to give 2 NH3 equation.

[00:26:34]equation must be balance.

[00:26:40]to obey law of conservation of mass. To obey law of conservation of mass of conservation of mass follower of masservation of mass can neither be created nor destroyed during a chemical reaction.

[00:27:07]The react of product information.

[00:27:45]Yeah. The mass perform the volume students.

[00:28:14]ratio.

[00:28:17]The number of moles Students nitrogen hydrogen Three moles students volume.

[00:29:19]Volume one gas. Volume by one mole gas. One volume condition and pressure 0° centigrade and one atmosphere Mumbai. Yeah. 273 and pressure 76 cm of mercury of mercury 132 22.4 4 decime volumets room temperature and atmospheric pressure 29 atmosphere students 0° ° volume 24.

[00:31:25]condition 22.47.2.4 Four decor volume students.

[00:32:15]G. Now the nitrogen 14 28 1 nitrogen 28 g hydrogen. Now go to hydrogen 2 hydrogen students.

[00:32:39]information into plus 3 H2 2 to give 2 NH3.

[00:33:13]If if 10 moles of nitrogen is reacted 10 moles react to ammonia.

[00:33:27]How many moles of hydrogen will be needed?

[00:33:39]volume.

[00:33:41]The 10 nitrogen nitrogen amrogenit the hydrogen For example, large number of questions.

[00:35:07]For example, question the volume the volume of ammonia produced the volume of ammonia produced when 10 moles of nitrogen is reacted has reacted with excess of hydrogen with excess of hydrogen. Hydrogen large students react with three moles of hydrogen to yield 2 mo of ammonia. Answerance volume students 44.8 Nitrogen students nitrogen given 44.8 decipher 440.8 8 decimeter cube.

[00:37:35]Students topic limiting an excess reactant.

[00:37:45]Limiting a reactant and X is reactant.

[00:38:00]reacting.

[00:38:20]The maximum amount of product.

[00:38:24]Maximum amount of product.

[00:38:31]Remaining amount of excess reactant.

[00:38:35]Remaining amount of excess reactant.

[00:38:47]Single reactant.

[00:39:09]Single reactant.

[00:39:15]The limiting of the excess reactance concept.

[00:39:19]No concept of limiting an excess reactant.

[00:39:33]The limiting reactance reactant concept reactant Our consume. Consumed of first.

[00:40:05]Consumed of first.

[00:40:26]small quantity small amount small amount.

[00:40:42]So for example equation into plus 3 H2 to give 2 NH3 amount 20 student consume.

[00:41:41]One small amount studenting reaction.

[00:42:19]reaction stop. The reaction will stop the limiting reactor. Now control product of the reaction.

[00:42:52]Limiting reactant.

[00:43:19]Excess react remains unreacted in the vessel.

[00:43:28]remains unreacted in the vessel.

[00:43:41]large amount students can give large amount of product. Can give large amount of product.

[00:44:06]large amount of product.

[00:44:32]students react.

[00:44:44]For example, students.

[00:44:51]If if 10 moles of nitrogen is reacted with 20 moles of hydrogen 20 moles of hydrogen students reacting amount amount of producting amount of reacting amount of excess reactant. The X is reactant. Remaining amounts reacting students. The volume differently students.

[00:46:18]same masses react molar mass mass If if 50 g of nitrogen is reacted with 50 g of hydrogen, The nitrogen mass 28 will be reacting.

[00:47:41]mass will be limiting.

[00:47:55]For example, if if 56 g of nitrogen is reacted with 20 g of hydrogen limiting reactant student massive Answer will be limiting reactant 56.

[00:48:47]Same volume different students.

[00:49:18]For example, The number of moles are same question.

[00:49:24]Therefore, five moles of each of each nitrogen and hydrogen are allowed to re to form limiting reactive moles. Given the hydrogen limiting for example If 20 cm cube of each nitrogen and hydrogen are allowed to mix allowed to react reactant reactants.

[00:50:51]student answering reacting reacting react.

[00:51:07]import cm cube of nitrogen is reacted is reacted with with 50 cm cube of hydrogen.

[00:51:45]Now the volume of ammonia produced the volume of ammonia produced volume.

[00:51:59]Now balance equation N2 + 3 H2 to give 2 NH3 equation the videos 20 different student answer 20 answer 16.6 Small answer. Small answer will be limiting reactant.

[00:52:56]Three moles.

[00:52:59]Volume two volumes.

[00:53:19]volume 3 cm 2 cm x = 50 * 2 / 3 100 / is equal to 33.3 cm maximum amount of product.

[00:53:52]This question remaining amount of reactant.

[00:53:58]Remaining amount of reactant remaining.

[00:54:18]Now remaining amount of the X is reactant students.

[00:54:30]2015 in the given reaction given limiting reactance balance equation.

[00:54:58]No concept of limiting reactance equation ratio.

[00:55:11]Question students 2019 cm cube methane gas was burned in 10 cm cube of oxygen to produce carbon dioxide. The limiting reaction is combustion reaction.

[00:55:27]The combustion reaction CH4 plus 22 to give 2 CO2 plus 2 H2O plus energy sorry CO2 H2O 20 cm 20 cm divide one true answer will be limiting reactant. Now limiting reactant for 2023.

[00:56:28]The reaction that is consumed first during uh the reactant sorry the reactant that is consumed first during chemical reaction.

[00:56:52]2024.

[00:56:54]Consider the reaction. The reaction consider each hydrogen and oxygen are allowed to react.

[00:57:04]Same volume each Oxygen limiting reactant. Yeah. Hydrogen X reaction.

[00:57:45]Hydrogen is limiting reactant.

[00:57:48]Limiting reactant questions. No comments violation students yield of reaction example nitrogen gas reacts with hydrogen gas to yield ammonia hydrogen reactants the reactants ammonia come Ammonia the product reaction of the reaction.

[00:58:46]Yield of the reaction 2 mo 34 gip 22.4 cube at STP 44.8 of the reaction.

[00:59:11]The amount of product obtained the amount of product obtained chemical reaction of the reaction.

[00:59:40]Theoretical.

[00:59:42]Theoretical percent.

[00:59:58]First one.

[01:00:01]Theoretical student N2 + 3 H2 to give 2 NH3 experiment.

[01:00:22]Sorry question. Therefore 10 moles of nitrogen is allowed to react 10 mo nitrogen reenit.

[01:00:54]10 moles 10 moles ammonia 20 ammonia the yield of n the yield of 10.

[01:01:16]Theoretically, the yield of 10 theoretically by calculations.

[01:01:34]equation.

[01:01:39]Students also calculated expectation.

[01:02:01]It is also called expected yield.

[01:02:05]Expect perform experimentally amount.

[01:02:35]Experimental practical yield.

[01:02:43]Experimental yield.

[01:02:45]Practical amount of product. The amount of product which is obtained practically which is obtained practically by performing experiment in laboratory.

[01:03:04]By performing experiment in laboratory students experimental experimental practical theor reasons.

[01:03:43]Now students maybe maybe all reactants are not converted into products.

[01:03:54]React all reactants are not converted into product.

[01:04:03]100% not performed reactant unreacted unreacted reactance.

[01:04:23]Maybe the reaction is reversible.

[01:04:26]Reversibility reaction students. Reaction conditions.

[01:04:37]Reaction conditions like temperature conditions effects.

[01:04:55]Recovery from home possible.

[01:04:58]Recovery from vessels.

[01:05:17]100% error.

[01:05:32]Systematic error. Personal error.

[01:05:37]Systematic error.

[01:05:48]always% Now students ratio percent.

[01:06:40]The percentage yield is is is it is the ratio of actual yield to theoretical multip theor form the percent possible.

[01:07:36]is equal or greater than 90%. Answer 90% efficiency.

[01:07:55]Efficiency of a reaction. Efficiency of a reaction.

[01:08:01]The percentage.

[01:08:14]more efficient.

[01:08:37]Students question.

[01:08:43]No question is always 2020. The efficiency of a reaction can be expressed by the reaction efficienc The reaction efficienc Percent is equal to multip.

[01:09:52]Choose the correct relation about the percentage. The relation students relation correct relation theoretical divided by actual multip for 2022 question. The amount of product that is actually produced during chemical reaction by performing experiment.

[01:10:16]The actual 2024 the efficiency of reaction can be checked by calculating by calculating percentage yield of the reaction actual yield reaches the ideal value ideal value 100%.

[01:10:41]When the percent is 100 questions students chapter number One stochometry.