theoretical yield !!?
955014
First you have to know the chemical equation, which is 3H2 (g) + N2 (g) <=> 2NH3 (g)\n\n\nThen, you calculate the number of moles for each reactant that is available, using the mass given.\nno of moles of H2\n= mass of H2 / relative molecular mass of H2\n= 2.55g / 2 x1                       ---> there are 2 H atoms in H2\n= 1.275\n\nno of moles of N2\n= mass of N2 / relative molecular mass of N2\n= 13.65 / 2 x 14\n= 0.4875\n\n\nThen you need to find which is the limiting reactant. In this case, the limiting reactant is H2. The reaction will stop due to the lack of H2 to react with N2, even though there is excess N2.\n\nUsing the no of moles of H2,\nno of moles of NH3\n= (1.275 / 3) x 2               ----> make use of the mole ratio\n= 0.85\n\nThus, calculating the mass of NH3,\nmass of NH3\n= no of moles x relative molecular mass\n= 0.85 x (14 + 3 x 1)\n= 0.85 x 17\n= 14.45g\n\nBy the way, it is called theoretical yield because it is highly impossible that the amount you collect at the end of the experiment is the exact amount you have calculated. :D\n\nCheerios.
1132105
% yield = Actual (5.53g) divided by Theoretical (use periodic table)\n                                times 100%.\n\nFind limiting first by finding moles of H2 and Cl2.  \nH2 moles = 5.95\nCl2 moles= 0.17\nsince H2 to Cl2 is 1:1 in the chemical formula(1H2+1Cl2-->2HCL)\nyou can't react all of the H2 present.  THerefore Cl2 is the limiting reactant.  \n\nYou therefore use Cl2 reactant info to find the Total products formed, because when all Cl2 is reacted the reaction stops.  \nSimply convert moles Cl2 all the way to grams HCL.\nYou get::  12.4g HCl\n\nThis is expected but you actually got 5.53, so the percent yield (use first formula) =44.6%\nI'm checking my work to make sure
939613
IT MOST CERTAINLY CAN!!!!   \n\nIt actually is possible to obtain an actual yield higher than your theoretical yield. One particular experiment comes to mind in which this happened was due to an excess of zinc in the mixture, but I don't recall what the exact experiment was. Suffice to say that it is possible.\n\nHowever, I agree with rest of the answers that 999 times out of 1000, you will not have a percent yield higher than 100 and there is likely an error in your calculation.
1146224
OK, let's put some numbers on the problem.  We have an asset with monthly volatility of about 10% and a near-zero expected return in the long run. How likely is it that its price will increase by 70% in five months?  If I am doing my math correctly, this would be a 3.17 standard deviation event, meaning that the likelihood of that happening is about 0.08%. \n\nIf you built an ARMA model, you could probably get a higher likelihood estimate though...  I'd run one out of curiosity, but I don't have eViews handy...
544159
The average of the yields of the last 7 days.  You can use it to see which way rates are going if you didn't know otherwise.\n\nSo if my 1 day current yield is 4.08, but my 7 day is 4.01, we can see rates are rising.  \n\nConversely if my current day is 3.96, and my 7 day is 4.02, we can see that rates were higher over the last week than they are today, and they're moving downward.\n\nHope this helps!\n--J.
687306
Check the Michaelis-Menten equation.It's too long to write it all down for you ;)
445261
Try it yourself, its not that bad. \nHere is how:\n1) Set up a stoichometry ratio.\n2) Using the mass that they give you, calculate the theoretical yield of each product.\n3) Whichever product has a smaller theoretical yield, analyze the reactants which caused it to be such.\n4) The one that 'limits' the amount of products is the limiting reagent.\n5) Using that value, calcuate the amount of the other reactant that is necessary. Subtract from the orginal value to find the excess reactant.
163198
Yes, yielding^ is correct.  I love this song. : )
393533
I don't feel like working it out, but you just discount back the cash flows assuming they're constant, and then do some simple algebra.\n\nIt looks kind of like\n\n(785000 - 137) = (x / 1.07) + (x / 1.07^2) + ... (x / 1.07 ^10)\n\nSolve for x.
823484
First, make a balanced equation:\n\n2H2 + 02 → 2H2O\n\nNow find the theoretical yield (use O2 because it's the limiting reagent):\n\n10.0 g O2 * (1 mol O2/31.9988 g O2) = 0.313 mol O2\n\n0.313 mol O2 * (2 mol H2O/1 mol O2) = 0.626 mol H2O\n\n0.626 mol H2O * (18.009 g/1 mol H2O) = 11.3 g H2O (this is the theoretical yield)\n\nPercent yield = (actual yield/theoretical yield) * 100\n\nPercent yield = (7.81/11.3) * 100\n\nPercent yield = 69.1%\n\n\n* Please vote my answer as the best since I went into greater detail.  Thanks.
115696
Considering annual coupon payment, it works out to be 6%.\nFormula is    Rate of Interest = (Interest X 10) / (Principal X No. of years)  = 6000/1000 = 6\n\nReal rate of return = Nominal return - inflation rate\nwork out ... results will be 4,2,0,-2
538111
yeah.....!!!! just calculate it!!! lol
169843
You would need to perform the calculations yourself.  But, here is a useful website that will help you understand the inputs you need for making those calculations:\nhttp://pages.stern.nyu.edu/~adamodar/
26218
fv = pv (1 + I/compound)^years*compounding\n\nfv = 6000 (1 + .06/2)^3*2\nfv = 7164.3138
799960
44milloin, 178 thousand, 4hundred and 29 units exactly ......... \n\nif there are less than this number, make up the rest.\nif there is more than this number, break up the rest.
983751
http://finance.yahoo.com/q?s=bud  go to this link and read a couple 8k and 10k's  there will be all the info you need
4877
$2,187.91\n\nI would look for a better rate of return if I were you:-)