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April 20, 2014

Search: Chem problem- percent yield

Number of results: 56,668

chem
Follow the steps in this example stoichiometry problem. This will give you the theoretical yield. Then percent yield = (actual yield/theoretical yield)*100 = ?
Thursday, February 9, 2012 at 8:28pm by DrBob222

Chem problem- percent yield
Okay, the formula is Actual Yield/Theortical Yield * 100 = Percent Yield 9.84g Sb is your actual yield To find your theortical yield, you first have to find the grams of Fe. Then find out which is the limiting reaction. Use the limiting reaction (your theortical yield) and ...
Sunday, March 22, 2009 at 7:01pm by Chopsticks

Chem problem- percent yield
Is the percent yield 91.5%?
Sunday, March 22, 2009 at 7:01pm by Stephanie

chemistry
The only difference here is that the problem TELLS you that 119.3 g PCl5 were formed. That is the ACTUAL yield. So use the 61.3 g Cl2 as the starting material and go through the steps in the worked example. The answer you obtain will be the THEORETICAL YIELD (Look down through...
Wednesday, July 13, 2011 at 10:35pm by DrBob222

Chem problem- percent yield
thanks for helping. :)
Sunday, March 22, 2009 at 7:01pm by Stephanie

Chem problem- percent yield
Heating an ore of antimony (Sb2S3) in the presence of iron gives the element antimony and iron(II) sulfide. Sb2S3 (s) + 3Fe(s) 2Sb(s) + 3FeS(s) When 15.0 g Sb2S3 reacts with an excess of Fe, 9.84 g Sb is produced. What is the percent yield of this reaction?
Sunday, March 22, 2009 at 7:01pm by Stephanie

Chem- Percent Yield
When HgO is heated, it decomposes into elemental mercury and diatomic oxygen gas. If 42.9 g of Hg is obtained from 70.1 g of the mercuric oxide, what is the percent yield of the reaction?
Thursday, October 11, 2012 at 1:03am by Lara

Chem problem- percent yield
91.5% is correct.
Sunday, March 22, 2009 at 7:01pm by DrBob222

Chemistry :)
Cr2O3 + 3CCl4 ---> 2CrCl3 + 3CCl2O In one experiment, 6.37 grams of Cr2O3 was treated wiht excess CCl4 and yielded 8.75 grams of CrCl3. What was the percent yeild? I have no idea how to do this. I know that percent yield is actual/theorectical yield *100. And i know how to ...
Wednesday, February 6, 2008 at 3:52pm by Miley

chemistry
percent yield = [actual yield/theoretical yield]*100 Remember this equation. It will work all the percent yield problems you have.
Friday, February 29, 2008 at 7:23am by DrBob222

Chemistry
1. The reaction CO+2H2-CH3OH was carried and it is found that only 332g of CH3Oh is actually produced when 407g CH3Oh was the expected yield. What is the Percent yield? 2. If 112g of CaO is reactied with an excess of NH4Cl and 64.0g of NH3 are produced, what is the percent ...
Wednesday, March 20, 2013 at 6:22pm by Nancy

Chemistry
This is the same kind of stoichiometry problem as the percent yield except the last step of % yield is not done. That is to say you want to calculate the theoretical yield (100% that is). Post your work if you get stuck.
Monday, July 29, 2013 at 11:34am by DrBob222

chem
Here is a worked example of a stoichiometry problem to find the theoretical yield. % yield = (actual yield/theoretical yield)*100 = ?
Wednesday, February 1, 2012 at 7:55pm by DrBob222

Chem problem- percent yield
Woops! I worked it over and got about 91.5% You are right. Sorry.
Sunday, March 22, 2009 at 7:01pm by Chopsticks

Chemistry
I have this question and I am pretty sure on what to use to solve it but I am just stuck. The reaction of 8 g of hydrogen and 28 g of carbon monoxide gave 16 g of methanol. What was the theoretical yield if the percent yield was 50%? actual yield ________________ X 100% = ...
Friday, September 16, 2011 at 2:16pm by Justin

chem
SiO2+6HF-----> H2SiF6+2H2O actual yield is 52.8 what is percent yield
Wednesday, February 1, 2012 at 7:55pm by Anonymous

chem
Thanks! And can you calculate the percent yield if they don't give the actual yield?
Thursday, April 8, 2010 at 3:58pm by Marc

Chemistry Pretest
Fe can be prepared as 2 Al + Fe2O3 ----> 2 Fe + Al2O3. Suppose that 0.450 moles of Fe2O3 are reacted with an excess of Al. Suppose that 43.6 grams of Fe are obtained. What is the percent yield of Fe? a) 16.2% b) 60.7% c) 86.7% d) 43.4% Percent yield= actual yield of product...
Friday, September 28, 2012 at 7:15am by Sarah

Chemistry
The problem I have with this is, that if I change the initial 1 concentration to something else, like 2 for example, then x/2 solves to a different yield % (71%). This leads me to believe that there is no constant yield percent for the given problem.
Tuesday, July 22, 2008 at 1:16pm by chemstudent

chemistry
The example gives theoretical yield and that's all you can calculate from the data you posted. If you have the percent yield you can determine actual yield by actual yield = theor yield x (%yield/100) = ??; otherwise, it can be done only by performing the experiment and ...
Saturday, May 14, 2011 at 7:47pm by DrBob222

Chem 104
percent yield = (actual yield/theoretical yield)*100 = ? 2.00 g is given in the problem as the actual yield. You must calculate the theoretical yield. The easy way to do that is with a planned approach to stoichiometry problems. Here is a step by step procedure. http://www....
Thursday, July 21, 2011 at 11:15pm by DrBob222

chem
You knew exactly what to do in the limiting reagent problem. These are simpler since there is only one reagent to worry about. Convert 12.28 g phosphorus to moles. moles = grams/molar mass. This is the limiting reagent because you have only this reagent given and the other is...
Sunday, December 11, 2011 at 9:48pm by DrBob222

chem
Oh..so that's what it was for... I guess I didn't think of that. I suspect you did not oxidize anything with NaCl No I didn't use NaCl at all in this lab. You CAN calculate two percent yields if you wish but I suspect your prof wants the overall yield. The first would be the ...
Saturday, November 24, 2007 at 7:40pm by ~christina~

Chemistry
mols NaHCO3 - grams/molar mass Use the coefficients to convert moles NaHCO3 to mols CO2. mols CO2 = mols NaHCO3 x (3 mol CO2/3 mol NaHCO3) = mols NaHCO3 x (3/3) = ? Convert mols CO2 to grams. g = moles x molar mass. This is the theoretical yield of CO2. You can't do percent ...
Tuesday, February 28, 2012 at 3:38pm by DrBob222

chemistry
One thing the percent yield will tell you is something about the side reactions. If the percent yield is virtually 100% you know that the side reactions were minimal. If the percent yield is 25% or so, you know that at leat another side reaction is competing with what you ...
Sunday, October 7, 2007 at 11:00pm by DrBob222

Chem
How are these values used to determine percent? actual yield is quantity of a product found to be formed in a chemical reaction and theoretical yield is the amount of product predicted theoretical yield is larger because in experiments reactions might not always go to ...
Sunday, July 18, 2010 at 5:25pm by Gregg

AP Chem
2) For a theoretical yield of 19 g and actual yield of 11 g, calculate the percent yield for a chemical reaction. Answer in units of %. 11 g / 19 g times 100 = 57.89% in your 2 sigfig problem, you might be expected to round off to 58% ======================================... ...
Monday, October 28, 2013 at 9:20pm by Anonymous

chem
Also I forgot to ask how to get the percent yield. I'm not sure but I guess I could calculate the percent yield of both camphor produced and isoborneol produced. What is getting to me is the ratios... I added the sodium hypochorite and also the glacial acetic acid but I'm not ...
Saturday, November 24, 2007 at 7:40pm by ~christina~

College Chemistry
I see two things wrong, one which is just a typo, I think, and the other which is why the problem is wrong. 1. The typo is you wrote .783/100 when you meant 78.3/100. You value of 175 shows you didn't use the 100 and 175 is right (for the numbers you have). 2. The problem is ...
Wednesday, March 31, 2010 at 12:59am by DrBob222

Chemistry
Another LR problem. Follow that last problem I did for you to calculate mass CO2. This is the theoretical yield. b. For % yield = (actual yield/theor yield)*100 = ?
Monday, October 7, 2013 at 6:58pm by DrBob222

math
how do you calculate theoretical yield of something? I don't know where to find the formula You go to the balanced chemical equation, and look at the mole ratio between the reactants and products. The theoretical yield is the value calculated from stoichiometry of a reaction. ...
Wednesday, January 31, 2007 at 12:58pm by james

AP CHEMISTRY
Theoretical yield is the amount calculated from the stoichiometry of the reaction. For example, suppose we wanted to calculate the theoretical yield of CO2 from the reaction C + O2 ==> CO2 if we had 24 g carbon initially. 24 g C = 24/12 = 2 mols C. 2 mols C produces 2 mol ...
Thursday, January 31, 2008 at 8:40pm by DrBob222

chemistry
So I did an experiment at school in which we had to form 2.00 grams of precipitate by mixing 2 hydrated compounds. So for the products, obviously one of it is water, and the other 2 products are compounds, one of which, is insoluble. So when I measured the amount of ...
Sunday, September 15, 2013 at 12:43pm by K

Chem. Percent Yield
This is a limiting reagent problem as well as a percent yield. Write the balance equation. Convert grams TiCl4 to moles. moles = grams/molar mass. Do the same for Mg. Using the coefficients in the balanced equation, convert moles of TiCl4 to moles of the product. Do the same ...
Monday, February 28, 2011 at 12:22am by DrBob222

chem
1.You need the balanced equation. 2.Convert grams of the starting material to moles. moles = grams/molar mass. Be sure to use as the starting material the one that was NOT in excess. 3.Using the coefficients in the balanced equation, convert moles of the starting material to ...
Friday, February 13, 2009 at 9:22pm by DrBob222

chem
The burning of 18.0 g of carbon produces 55.0 g of carbon dioxide. What is the theoretical yield of CO2? Calculate the percent yield of CO2.
Sunday, June 1, 2008 at 8:44pm by Anonymous

Organic Chem
Bromine will react with limonene according to this reaction (there's a picture, but I can't get that on here. So I'll do my best to write it out). 136.23 g/mol + Br2 ------> 296.04 g/mol Suppose 627 mg of limonene was reacted with 3.7 mL of a 7.7% (v/v) solution of Br2 in ...
Wednesday, November 2, 2011 at 7:39pm by Marvin

Chemistry
This is just a twist to the usual stoichiometry problem. 1. Write and balance the equation. 2. Convert g you have (in this case 8.85 g Fe) to moles. moles = grams/atomic mass. 3. Using the coefficients in the balanced equation, convert moles Fe to moles H2. 4. Now convert ...
Sunday, January 10, 2010 at 4:14pm by DrBob222

Chemistry I
iF THE THEORETICAL YIELD IF A REACTION IS 0.121G AND THE ACTUAL YIELD IS 0.112G WHAT IS THE PERCENT YIELD
Saturday, April 9, 2011 at 12:55pm by tammy

chemistry
supposed the theoritical yield in a reaction is 68.8g, and the percent yield is 66.0%, what is the actual yield of product obtained?
Saturday, March 24, 2012 at 3:45pm by kims

Chemistry
I have a problem that has been driving me crazy trying to solve, and I was wondering if someone could help. The problem is this: "Given the reaction: CuSO4 + 4 NH3 ----> Cu(NH3)4SO4, if 10 grams of CuSO4 reacts with 30 grams of NH3, what is the theoretical yield of Cu(NH3)...
Thursday, August 23, 2007 at 1:10pm by Josh

finance
the corner grocer has a 7-year, 6 percent annual coupon bond outstanding with a $1,000 par value. the bond has a yield to maturity of 5.5 percent. Which one of the following statements is correct if the market yield suddenly increases to 6.5 percent? The bond price will ...
Wednesday, March 5, 2014 at 7:39pm by carol

finance
the corner grocer has a 7-year, 6 percent annual coupon bond outstanding with a $1,000 par value. the bond has a yield to maturity of 5.5 percent. Which one of the following statements is correct if the market yield suddenly increases to 6.5 percent? The bond price will ...
Wednesday, March 5, 2014 at 8:33pm by carol

finance
The Corner Grocer has a 7-year, 6 percent annual coupon bond outstanding with a $1,000 par value. The bond has a yield to maturity of 5.5 percent. Which one of the following statements is correct if the market yield suddenly increases to 6.5 percent? The bond price will ...
Wednesday, March 5, 2014 at 9:08pm by geof

CHEM
why should the maximum percent yield never be above 100%
Sunday, August 5, 2012 at 3:43am by amira

chemistry!!!Need helpp!!!
how do you find percent yield of a rxn, and how do you find mmol of something? percent yield = 100 * (actual yield/predicted yield) find the number of moles, and then conver it to milimeter. millimols = mols x 1000 OR mols = grams/molar mass OR millimols = milligrams/molar ...
Sunday, December 3, 2006 at 10:22pm by day

chemistry
1) a student used 3.50 g of salicylic acid. calculate theoretical yield 2) the actual yield (from experiment) was found to be 1.50 g less than the theoretic yield (mass), calculate the percent yield 3) t
Wednesday, July 18, 2012 at 6:27am by ama

Chemistry
Percent yield = (actual yield/theoretical yield) *100 = ?
Wednesday, March 20, 2013 at 6:22pm by DrBob222

Chemistry--To c
For the new numbers you quoted, I get 49.6 g Au possible with percent Au = (49.6/126.5) *100 = ?? For percent, in this case, you are asking for percent gold in the 126.5 grams sample of ore, not percent yield. The percent figure obtained assumes the yield of the chemical ...
Tuesday, February 9, 2010 at 6:42pm by DrBob222

organic chemistry
how do u find the percent yield of 4.0g of acetanilide AND 31.12G OF 4-bromoacetanilide. calculate the percent yield of 4-bromoacetanilide
Tuesday, November 23, 2010 at 6:21pm by georgie

Chem
This is a limiting reagent and a percent yield problem rolled into one. I know it is limiting reagent because amounts are given for BOTH reactants. N2 + 2H2 ==> 2NH3 mols N2 = grams/molar mass mols H2 = grams/molar mass Using the coefficients in the balanced equation, ...
Thursday, March 7, 2013 at 5:03pm by DrBob222

Chemistry
I have a problem that has been driving me crazy trying to solve, and I was wondering if someone could help. The problem is this: "Given the reaction: CuSO4 + 4 NH3 ----> Cu(NH3)4SO4, if 10 grams of CuSO4 reacts with 30 grams of NH3, what is the theoretical yield of Cu(NH3)...
Thursday, August 23, 2007 at 9:29pm by Josh

chemistry
You must always have a balanced equation and you have that. Convert 50 g methanol to moles. moles = grams/molar mass Using the coefficients in the balanced equation, convert moles methanol to moles H2O. Now convert moles H2O to grams. g = moles x molar mass. This is the ...
Monday, March 22, 2010 at 6:30pm by DrBob222

financial management
current yield for annual payments bonds have 25 years remaining to maturity. the bonds have a face value of $1000 and a yield to maturity of 7 percent. they pay interest annually and have a 11 percent coupon rate. what is their current yield?
Tuesday, December 29, 2009 at 4:55pm by judy

Chemistry
You know from your first post about 7.0 g propane how to do stoichiometry. The number you obtained in that process is called the theoretical yield (if you had determined either CO2 or H2O). Do this one the same way. The answer you obtain will be the theoretical yield. Then %...
Wednesday, May 12, 2010 at 10:08am by DrBob222

chemistry - synthesis of aspirin
No. Mass of acetic acid = mols acetic acid x molar mass acetic acid and that is the theoretical yield of acetic acid in grams. I don't know the exact instructions you have but if I were asked to calculate grams acetic acid produced I would do as above then multiply by the ...
Saturday, April 7, 2012 at 8:32pm by DrBob222

chem
theoretical yield and actual yield. Instead of theoretical yield, if you knew the name of the metal, an equation could be written and the theoretical yield could be calculated.
Thursday, April 8, 2010 at 3:58pm by DrBob222

Chemistry
Consider the following reaction: 2 SO2 (g) + O2 (g)----> 2 SO3 (g) If 285.3 mL of SO2 is allowed to react with 158.9 mL of O2 (both measured at 315 K and 50.0 mmHg), what is the limiting reactant and theoretical yield of SO3 in moles? If 187.2 mL of SO3 is collected (...
Wednesday, October 27, 2010 at 10:07pm by Jarrod

chemistry 101
Limiting reagent problem, I think, are easiest to do if you do TWO simple stoichiometry problems. The first time you use CaO and determine moles CaCO3 produced. The second time use 13.8 g CO2 and determine moles CaCO3 produced. The correct answer, in limiting reagent problems...
Friday, July 8, 2011 at 9:12pm by DrBob222

FINANCE
Current yield and yield to maturity A bond has a $1,000 par value, 10 years to maturity, a 7 percent annual coupon, and sells for $985. a. What is its current yield? b. What is its yield to maturity (YTM)? c. Assume that the yield to maturity remains constant for the next 3 ...
Tuesday, September 18, 2007 at 7:14pm by Mel

chem
Write the equation which you have BUT you have omitted the yield sign and and + signs. No way to know the difference between reactants and products. Convert 100.0 g AgCl to mols. Using the coefficients in the balanced equation, convert mols AgCl to mols Ag. Convert mols Ag to ...
Sunday, June 1, 2008 at 8:44pm by DrBob222

chem
consider the following balance chemical equation: 2NH3(g)+3CuO(s)=N2(g)+3Cu(s)+3H2O(g) if 18.1grams of ammonia reacts with 90.4 grams of copper(II) oxide, which is the limitting reagent?? what is the theorectical yield of nitrogen gasd? if 8.52 g of N2 are formed, what is the...
Monday, November 15, 2010 at 5:49pm by julia-Drboob22

chem
consider the following balance chemical equation: 2NH3(g)+3CuO(s)=N2(g)+3Cu(s)+3H2O(g) if 18.1grams of ammonia reacts with 90.4 grams of copper(II) oxide, which is the limitting reagent?? what is the theorectical yield of nitrogen gasd? if 8.52 g of N2 are formed, what is the...
Monday, November 15, 2010 at 9:50pm by julia

chem
change the mass to moles for all three. Now divide the moles of C2H2, O2, and CO2 by the coefficents 2,5, 4 Which is the lowest number? That is the limiting reageant. WHY? For yield, how many moles of the limiting reageant so you have. You should get the ratio of coefficents ...
Sunday, September 29, 2013 at 8:06pm by bobpursley

chem/DrBob22
consider the following balance chemical equation: 2NH3(g)+3CuO(s)=N2(g)+3Cu(s)+3H2O(g) if 18.1grams of ammonia reacts with 90.4 grams of copper(II) oxide, which is the limitting reagent?? what is the theorectical yield of nitrogen gasd? if 8.52 g of N2 are formed, what is the...
Monday, November 15, 2010 at 6:23pm by julia

Chemistry
For my theortical yield I got 1.1173 g For my actual yield I got 0.27 g I need to find my percent yield and percent error. Did I do this right? % Yield = (0.27/1.1173) * 100 = 24 % % Error = [(0.27-1.1173)/1.1173] * 100 = -76 %
Wednesday, November 5, 2008 at 10:09pm by Lena

Chemistry
No, you didn't do the percent yield correctly. You must use the 3.22 g salicylic acid with which you started to calculate how much aspirin you should have obtained if the reaction was 100% efficient. I hastily went through it and it is approximately 4 grams but you need to go ...
Monday, March 30, 2009 at 10:19pm by DrBob222

chemistry
The theoretical yield of a reaction is 78.5 grams of product and the actual yield is 66.3 grams. What is the percent yield?
Tuesday, December 11, 2012 at 5:42pm by Anonymous

Organic Chem/ Calculate Yield
How would you calculate the percent yield for a reaction that began with 10 moles of acetone and 16 moles of benzaldehyde which yielded 6 moles of dibenzalacetone as the product? The molecular weights are as follows (acetone = 58.08 g/mole), (benzaldehyde = 106.2 g/mole), (...
Thursday, March 8, 2007 at 5:00pm by Steve

chemistry check my work
C7H6O3+CH3OH→C8H8O3+H2O In any experiment, 1.50g of salicyclic acid is reacted with 11.20g of methanol. The yield of methyl salicylate, C8H8O3, is 1.31g. What is the percent yield? percent is 77.l1% is this correct?
Thursday, April 15, 2010 at 8:14am by Molly

science
Suppose 65.8 g of Carbon monoxide reacts with 8.6 g of hydrogen. What is the limiting reagent? What is the theoretical yield of the product in moles and grams? If the actual yield of the product is 3.57 g, what is the percent yield?
Tuesday, October 5, 2010 at 7:23pm by Anonymous

chemistry
The answer probably is yes but I need to know more about what you're doing. Note: Actual yield usually is not calculated. Damp paper certainly will affect percent yield but not calculated theoretical yield.
Monday, November 19, 2012 at 11:26am by DrBob222

Chem 104
The reaction of 2.30g N2 with excess H2 produces 2.00g NH3. The percent yield of this reaaction is?
Thursday, July 21, 2011 at 11:15pm by Zoria

CHEM
1. How many moles of water can be made from 4 moles of oxygen gas and 16 moles of hydrogen gas? What is the limiting reagent? 2. Calculate the mass of water produced from the reaction of 24.0 g of H2 and 160.0 g of O2. What is the limiting reagent? 3. The burning of 18.0 g of...
Sunday, June 1, 2008 at 9:05pm by Anonymous

Chem. Percent Yield
Titanium, a strong, lightweight metal used in many applications, is prepared by the reaction of titanium(IV) chloride with molten magnesium metal. 3.45 x 10^7g of titanium(IV) chloride is reacted with 1.13 x 10^7g of magnesium, 7.91 x 10^6g of titanium metal are obtained. What...
Monday, February 28, 2011 at 12:22am by Toni Jones

Corporate Finance
The yield-to-maturity on a bond is the interest rate you earn on your investment if interest rates do not change. If you actually sell the bond before it matures, your realized return is known as the holding period yield. Suppose that today, you buy a 12 percent annual coupon ...
Thursday, April 21, 2011 at 12:08am by Nik

Chem
Determine the percent yeild of: KCl3(s)--> KCl(s)+ O2(g) 2.14g of KCl3 produces 0.67 of O2 I get 123% when the correct answer is 80% My work: KCl3: mm = 122.45, n =0.017 Theoretical yield: .017mol * 32g/mol Pecent Yield: 0.67g/ 0.544g *100% = 123%
Wednesday, October 7, 2009 at 11:02pm by Sara

chemistry
10Cl2 + P4 ==> 4PCl5 Convert 2.5 mol Cl2 to mols PCl5 using the coefficients in the balanced equation. That is the theoretical yield of the reaction. Then % yield = [theoretical yield/actual yield]*100. The actual yield is given in the problem as 0.5 mol.
Tuesday, December 11, 2007 at 12:47am by DrBob222

Chemistry
A student begins with 9.7 mL of a 0.26 M Cu(NO3)2 solution and performs copper cycle lab. She recovers 0.075 grams of copper metal. A) What is the Theoretical Yield B) What is the Actual Yield C) What is the Percent Yield
Monday, February 10, 2014 at 6:57pm by C

chem
I'm not up to answering most of the first question; however, I suspect you did not oxidize anything with NaCl. As for the limiting reagent second part, forget about the limiting reagent. All of the glacial acetic acid, hypochlorite, sodium borohydride and those other things ...
Saturday, November 24, 2007 at 7:40pm by DrBob222

Chemistry:Important!!!!!!!
A student begins with 9.7 mL of a 0.26 M Cu(NO3)2 solution and performs copper cycle lab. She recovers 0.075 grams of copper metal. A) What is the Theoretical Yield B) What is the Actual Yield C) What is the Percent Yield
Monday, February 10, 2014 at 7:55pm by B

chem
Calculate the percent yield of Cl2(g) in the electrolytic decomposition of hydrogen chloride if 25.8 g of HCl produces 13.6 g of chlorine gas.
Sunday, June 1, 2008 at 8:44pm by Anonymous

chem
For a combination reaction, you have A + B ==> C A = 7.59g + B of 4.88 = 12.47 grams as the theoretical yield. %yield = (mass product/theoretical yield)*100 = ??
Wednesday, November 10, 2010 at 8:03pm by DrBob222

chemistry2
1. You have the balanced equation. 2. Convert 160 g Al to moles. moles = grams/molar mass. 3. Using the coefficients in the balanced equation, convert moles Al to moles Al2O3. 4. Now convert moles Al to grams. g = moles x molar mass. This is the theoretical yield in grams. 5. ...
Wednesday, May 5, 2010 at 6:53pm by DrBob222

chem
what is the percent yield if 27 g of h20 obtained when 33 g of c3h8 reacts with 56 L of 02 at STP.The secong product of reaction is CO2
Wednesday, March 13, 2013 at 6:38pm by percent

chemistry
Would a damp filter paper affect the theoritical yield, calculated actual yield and calculated percent yield. Please help. Chemistry is hard.
Monday, November 19, 2012 at 11:26am by Anonymous

Chem- Percent Yield
2HgO ==> 2Hg + O2 mol HgO = 70.1g/molar mass HgO = ? Use the coefficients to convert mols HgO to mols Hg. The ratio is 2:2 which is 1:1; therefore, mols HgO = mols Hg. Convert mols Hg to grams. g = mols x atomic mass. This is the theoretical yield (TY). The actual yeld (AY...
Thursday, October 11, 2012 at 1:03am by DrBob222

Chemistry
A percent yield/100 = fractional yield. For example, a 25% yield is a fractional yield of 0.25.
Friday, March 5, 2010 at 1:03pm by DrBob222

chemistry
1. Chlorobenzene, C6H5Cl, is used in the production of chemicals such as aspirin and dyes. One way that chlorobenzene is prepared is by reacting benzene, C6H6, with chlorine gas according to the following BALANCED equation. C6H6 (l) + Cl2 (g) nC6H5Cl (s) + HCl (g) a. What ...
Wednesday, March 31, 2010 at 7:35pm by Michael

Chemistry
Could someone check my answers? 1. Why was 95% ethanol alcohol added when titrating aspirin in an experiment? Because it helps the aspirin dry quicker and become pure while the titration is going on. 2. Would the following mistakes cause the calculated percent yield to be ...
Tuesday, March 27, 2007 at 1:25am by Jim

Chemistry HELP ME!!!!
Ca(NO3)2(aq) + 2NH4F(aq) ==> CaF2(s) + 2NH4NO3(aq) 2. moles = M x L 3. moles = M x L 4. Using the coefficients in the balanced equation, convert mole of Ca(NO3)2 to moles CaF2. With the same procedure, convert moles NH4F to moles CaF2. The smaller number of moles will be ...
Wednesday, February 10, 2010 at 2:51pm by DrBob222

Chemistry
CH4 + 2Cl2 ==> CH2Cl2 + 2HCl This is a limiting reagent problem. Remember how do to this type problem. Most are alike. 2a. Convert 6.00 g CH4 to moles. moles = grams/molar mass. 2b. Convert 6.00 g Cl2 to moles. Same formula. 3a. Using the coefficients in the balanced ...
Sunday, March 28, 2010 at 11:04am by DrBob222

chem 11
The stoichiometric amount of NaCl is the theoretical yield. Convert 25 NaBr to moles. moles = grams/molar mass. Using the coefficients in the balanced equation, convert moles NaBr to moles NaCl. Now convert moles NaCl to grams. g = moles x molar mass. This is the theoretical ...
Wednesday, July 21, 2010 at 7:37pm by DrBob222

accounting
Midland Oil has $1,000 par value bonds outstanding at 8 percent interest. The bonds will mature in 25 years. Compute the current price of the bonds if the present yield to maturity is: A. 7 percent. B. 10 percent. C. 13 percent.
Sunday, January 10, 2010 at 9:53pm by Cindy

math
Midland Oil has $1,000 par value bonds outstanding at 8 percent interest. The bonds will mature in 25 years. Compute the current price of the bonds if the present yield to maturity is: A. 7 percent. B. 10 percent. C. 13 percent.
Monday, January 11, 2010 at 11:53am by Robert

Chemistry
18.85 g CO2 is the theoretical yield. Actual yield is 16.34. Percent yield, although you didn'task for it, is %Yield = (16.34/18.85)*100 = ?
Sunday, July 8, 2012 at 4:17pm by DrBob222

chem
Write the equation. Convert 18.0 g C to mols. Covert mols C to mols CO2 using the coefficients in the balanced equation. Convert mols CO2 to grams. That will give you the theoretical yield. Then percent yield = [actual amount/theoretical] * 100 Post your work if you get stuck.
Sunday, June 1, 2008 at 8:44pm by DrBob222

financial
2. A bank is considering an investment in a municipal security that offer a yield of 6 percent. What is the securitys tax equivalent yield if the banks tax rate is 35 percent
Wednesday, November 28, 2012 at 3:01pm by sandra

Chemistry
First, start with a balanced equation. Then, use stoichiometry to determine the limiting reactant and then how much product (AgCl) is produced. Use this (theoretical yield) and the actual yield (33.6g) to determine the percent yield.
Tuesday, June 23, 2009 at 1:27pm by David

Chemistry
A chemist ran the reaction and obtained 5.70 of ethyl butyrate. What was the percent yield? How do I solve this problem?
Tuesday, December 6, 2011 at 8:26am by Nancy

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