How many moles of pbcl2 will be formed

This theoretical yield calculator will answer all the burning questions you have regarding how to calculate the theoretical yield, such as how to find theoretical yield as well as the theoretical yield definition and the theoretical yield formula. Before carrying out any kind of lab work, you need to work out what is the theoretical yield so you know how much of your product, be it a molecule or lattice, you can expect from a given amount of starting material. This allows you to work out how efficiently you carried out your reaction (the quantity you can find at the IMPORTANT NOTE: Yields can only be found using the limiting reagent. If you are uncertain which of your reagents are limiting, plug in your reagents one at a time, and whichever one gives you the lowest number of moles is the limiting reagent. Remember to hit refresh at the bottom of the calculator to reset it. What is the theoretical yield? It is the amount of a product that would be formed if your reaction was 100% efficient. How to achieve 100% efficiency? Well, it would mean that every molecule reacted correctly (i.e., no side products are formed) at every step and that no molecule was lost on the sides of the glassware. As a normal reaction deals with quintillions of molecules or atoms, it should be obvious that some of these molecules will be lost. Therefore the percent yield will never be 100%, but it is still useful to know as a metric to base your efficiency of the reaction. For more on this, check out...

This problem has been solved! You'll get a detailed solution from a subject matter expert that helps you learn core concepts. See Answer See Answer See Answer done loading Question:QUESTION 1 33.7 ml of aqueous 0.255 M Pb(NO3)2 is mixed with 26.2 mt. of 0.415 M NaCl. The equation for the precipitate reaction is Pb(NO3)2 (aq) + 2 NaCl(aq) - PbCl2 (s) + 2 NaNO3(aq) How many moles of PbCl2 are formed? QUESTION 2 Silver sulfate is precipitated from solution according to the following reaction 2 AgNO3(aq) + Na2SO4 (aq) -> A2SO4() 2 QUESTION 1 33.7 ml of aqueous 0.255 M Pb(NO3)2 is mixed with 26.2 mt. of 0.415 M NaCl. The equation for the precipitate reaction is Pb(NO3)2 (aq) + 2 NaCl(aq) - PbCl2 (s) + 2 NaNO3(aq) How many moles of PbCl2 are formed? QUESTION 2 Silver sulfate is precipitated from solution according to the following reaction 2 AgNO3(aq) + Na2SO4 (aq) -> A2SO4() 2 NaNO3(aq) 3.80 moles of AgNO3 and 3.04 moles of Na2SO4 are present initially, how many moles of excess reactant will remain after precipitation is complete? Write your answer to 2 decimal places, QUESTION 3 If ammonia can be produced from calcium oxide and ammonium chloride according to the following reaction. If 17.6 g of calcium oxide is used in the reaction and 7.43 g of ammonia is recovered, what is the % yleld of the reaction? Cao(s) + 2NH4CKS) -- 2 NH3(g) +CaCl26) + H2O(g) Previous question Next question

A balanced equation for the above reaction is : PbO + 2HCl ---------------> PbCl 2 + H 2O Now,we see that PbO and HCl react in 1:2 mol ratio. Atomic mass of PbO = Atomic mass of Pb + Atomic mass of O = (206.9 + 16) g = 222.9 Atomic mass of HCl = Atomic mass of H + Atomic mass of Cl = ( 1.008 + 35.45 ) g = 36.45g moles of PbO = 6.5g / 222.9g = 0.029 = 0.03 moles of HCl = 3.2g / 36.45g = 0.08 Since we need only 0.06 mol HCl to react with 0.03 mol PbO As we can see,we have too much HCl so PbO is the limiting reagent. This just means that the amount of product will be determined by the amount of PbO. Now, from each mol of PbO we get 1 mol of PbCl2. Since we started with 0.03 mol PbO, we only form 0.03 moles of PbCl2.

• Chapter 1 - Measurements • Chapter 2 - Energy and Matter • Chapter 3 - Solids and Liquids • Chapter 4 - Atoms, Molecules, and Ions • Chapter 5 - Chemical Reactions and Equations • Chapter 6 - Stoichiometry and the Mole • Chapter 7 - Nuclear Chemistry • Chapter 8 - Chemical Bonds • Chapter 9 - Gases • Chapter 10 - Solutions • • • • • • • • • Chapter 11 - Acids and Bases • Chapter 12 - Chemical Equilibrium • Chapter 13 - Organic Chemistry • Lab Documents To print this page: Click on the printer icon at the bottom of the screen Is your printout incomplete? Make sure that your printout includes all content from the page. If it doesn't, try opening this guide in a different browser and printing from there (sometimes Internet Explorer works better, sometimes Chrome, sometimes Firefox, etc.). Alternative printing method: If the above process produces printouts with errors or overlapping text or images, try this method: • Using the cursor, capture the contents of the entire page • Paste this content into a Word document or other word processing program • Print that document Solutions Opening Essay More than 70% of the earth’s surface is covered by a very important solution—seawater. It is likely that without seawater, no life would exist on Earth. At its simplest, seawater is mostly H 2O. But about 3.5% of seawater is dissolved solids, mostly NaCl but other ions as well. Table 10.1 "Percentage by Mass of Ions in Seawater and Blood" lists the percentage by mass of the various ion...

More • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • Step 1: Given data • Given the mass of PbO = 6 . 5 gm • Given the mass of HCl = 3 . 2 gm Step 2: Calculating moles of lead(II) Chloride: When Lead oxide reacts with Hydrochloric acid there is the formation of Lead ( II) chloride PbO ( s ) Lead oxide + 2 HCl ( aq ) Hydrochloric acid → PbCl 2 ( s ) Lead ( II ) chloride + H 2 O ( aq ) Water Molecular mass of PbO = Atomic mass of Pb + Atomic mass of O = 207 + 16 ⇒ 223 gm Molecular mass of HCl = Atomic mass of H + Atomic mass of Cl = 1 + 35 . 5 ⇒ 36 . 5 gm The number of moles is calculated as Number of moles = Given mass Molecular mass Number of moles of PbO = 6 . 5 223 = 0 . 029 Number ...

More • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • • A balanced equation for the above reaction is : PbO + 2HCl ---------------> PbCl 2 + H 2O Now,we see that PbO and HCl react in 1:2 mol ratio. Atomic mass of PbO = Atomic mass of Pb + Atomic mass of O = (206.9 + 16) g = 222.9 Atomic mass of HCl = Atomic mass of H + Atomic mass of Cl = ( 1.008 + 35.45 ) g = 36.45g moles of PbO = 6.5g / 222.9g = 0.029 = 0.03 moles of HCl = 3.2g / 36.45g = 0.08 Since we need only 0.06 mol HCl to react with 0.03 mol PbO As we can see,we have too much HCl so PbO is the limiting reagent. This just means that the amount of product will be determined by the amount of PbO. Now, from each mol of PbO we get 1 mol of ...

Step 1: Given data • Given the mass of PbO = 6 . 5 gm • Given the mass of HCl = 3 . 2 gm Step 2: Calculating moles of lead(II) Chloride: When Lead oxide reacts with Hydrochloric acid there is the formation of Lead ( II) chloride PbO ( s ) Lead oxide + 2 HCl ( aq ) Hydrochloric acid → PbCl 2 ( s ) Lead ( II ) chloride + H 2 O ( aq ) Water Molecular mass of PbO = Atomic mass of Pb + Atomic mass of O = 207 + 16 ⇒ 223 gm Molecular mass of HCl = Atomic mass of H + Atomic mass of Cl = 1 + 35 . 5 ⇒ 36 . 5 gm The number of moles is calculated as Number of moles = Given mass Molecular mass Number of moles of PbO = 6 . 5 223 = 0 . 029 Number of moles of HCl = 3 . 2 36 . 5 = 0 . 0877 From the number of moles calculations, PbO is the limiting agent as its moles are less than HCl. When one mole of PbO is totally consumed there is the formation of one mole of PbCl 2. Hence, 0.029 moles of Lead(II) chloride are formed.

This problem has been solved! You'll get a detailed solution from a subject matter expert that helps you learn core concepts. See Answer See Answer See Answer done loading Question:QUESTION 1 33.7 ml of aqueous 0.255 M Pb(NO3)2 is mixed with 26.2 mt. of 0.415 M NaCl. The equation for the precipitate reaction is Pb(NO3)2 (aq) + 2 NaCl(aq) - PbCl2 (s) + 2 NaNO3(aq) How many moles of PbCl2 are formed? QUESTION 2 Silver sulfate is precipitated from solution according to the following reaction 2 AgNO3(aq) + Na2SO4 (aq) -> A2SO4() 2 QUESTION 1 33.7 ml of aqueous 0.255 M Pb(NO3)2 is mixed with 26.2 mt. of 0.415 M NaCl. The equation for the precipitate reaction is Pb(NO3)2 (aq) + 2 NaCl(aq) - PbCl2 (s) + 2 NaNO3(aq) How many moles of PbCl2 are formed? QUESTION 2 Silver sulfate is precipitated from solution according to the following reaction 2 AgNO3(aq) + Na2SO4 (aq) -> A2SO4() 2 NaNO3(aq) 3.80 moles of AgNO3 and 3.04 moles of Na2SO4 are present initially, how many moles of excess reactant will remain after precipitation is complete? Write your answer to 2 decimal places, QUESTION 3 If ammonia can be produced from calcium oxide and ammonium chloride according to the following reaction. If 17.6 g of calcium oxide is used in the reaction and 7.43 g of ammonia is recovered, what is the % yleld of the reaction? Cao(s) + 2NH4CKS) -- 2 NH3(g) +CaCl26) + H2O(g) Previous question Next question

• Chapter 1 - Measurements • Chapter 2 - Energy and Matter • Chapter 3 - Solids and Liquids • Chapter 4 - Atoms, Molecules, and Ions • Chapter 5 - Chemical Reactions and Equations • Chapter 6 - Stoichiometry and the Mole • Chapter 7 - Nuclear Chemistry • Chapter 8 - Chemical Bonds • Chapter 9 - Gases • Chapter 10 - Solutions • • • • • • • • • Chapter 11 - Acids and Bases • Chapter 12 - Chemical Equilibrium • Chapter 13 - Organic Chemistry • Lab Documents To print this page: Click on the printer icon at the bottom of the screen Is your printout incomplete? Make sure that your printout includes all content from the page. If it doesn't, try opening this guide in a different browser and printing from there (sometimes Internet Explorer works better, sometimes Chrome, sometimes Firefox, etc.). Alternative printing method: If the above process produces printouts with errors or overlapping text or images, try this method: • Using the cursor, capture the contents of the entire page • Paste this content into a Word document or other word processing program • Print that document Solutions Opening Essay More than 70% of the earth’s surface is covered by a very important solution—seawater. It is likely that without seawater, no life would exist on Earth. At its simplest, seawater is mostly H 2O. But about 3.5% of seawater is dissolved solids, mostly NaCl but other ions as well. Table 10.1 "Percentage by Mass of Ions in Seawater and Blood" lists the percentage by mass of the various ion...

This theoretical yield calculator will answer all the burning questions you have regarding how to calculate the theoretical yield, such as how to find theoretical yield as well as the theoretical yield definition and the theoretical yield formula. Before carrying out any kind of lab work, you need to work out what is the theoretical yield so you know how much of your product, be it a molecule or lattice, you can expect from a given amount of starting material. This allows you to work out how efficiently you carried out your reaction (the quantity you can find at the IMPORTANT NOTE: Yields can only be found using the limiting reagent. If you are uncertain which of your reagents are limiting, plug in your reagents one at a time, and whichever one gives you the lowest number of moles is the limiting reagent. Remember to hit refresh at the bottom of the calculator to reset it. What is the theoretical yield? It is the amount of a product that would be formed if your reaction was 100% efficient. How to achieve 100% efficiency? Well, it would mean that every molecule reacted correctly (i.e., no side products are formed) at every step and that no molecule was lost on the sides of the glassware. As a normal reaction deals with quintillions of molecules or atoms, it should be obvious that some of these molecules will be lost. Therefore the percent yield will never be 100%, but it is still useful to know as a metric to base your efficiency of the reaction. For more on this, check out...