Chemistry

In a lab we are trying to find the percent yield of NaCl collected after evaporating the water off an NaCl solution. We made up a .100 M NaCl solution, and used 10. mL of it in our experiment.
We know that the empty evaporating dish and cover mass 68.9132 +/- .0003 g, and after our final trial our evaporating dish, cover, and NaCl mass 68.9695 +/- .0003 g.

We calculated our theoretical yield as such..
10. mL +/- .2% x (.100 sub 0 mol +/- .6 % / 1 L) x ( 1 L/ 1000 mL) x (58.77 g / 1 mol) = .058 +/- .001 g

I calculated our actual yeild as such..
68.9695 +/- .0003 g -> 68.9695 +/- .0004 sub 3 %
- 68.9132 +/- .0003 g -> 68.9132 +/- .0004 sub 4%
= .0563 +/- .00008 sub 7 %

Going by these calculations, I calculate the percent yield to be
(.0563 +/- .0008 sub 7 %) / (.058 +/- 1.sub 7 %) = 97 +/- 2 (absolute) %

However, my partner got 97 +/- 3%, and since I haven't done error calculations in a while I'm trusting that her answer is correct. Can someone help me find what I did wrong?


I get one percent error on the measured mass, and two percent on the theoretical.

Stick with your three percent. The precision of the known solutions (molarity and volume) as you have cited is beyond what most college labs do.

  1. 👍
  2. 👎
  3. 👁

Respond to this Question

First Name

Your Response

Similar Questions

  1. Chemistry

    1.Chlorine gas can be produced commercially by passing an electric current through a concentrated solution of sodium chloride (brine). The unbalanced equation is NaCl(aq) + H2O(ℓ) → NaOH(aq) + Cl2(g) + H2(g). If the brine

  2. Chem

    A 25.0 mL aliquot of a well-shaken and filtered sample of river is pipetted into an evaporating dish. The sample was heated to dryness. Assume the density of the river water was 1.01g/mL. The following data were collected for

  3. Chemistry

    The combustion of liquid ethanol (C2H5OH) produces carbon dioxide and water. After 4.60mL of ethanol (density=0.789g/ml) was allowed to burn in the presence of 15.45g of oxygen gas, 3.70mL of water (density=1.00g/ml) was

  4. Chemistry

    H3PO4 + 3KOH = K3PO4 + 3 H2O What would be the percent yield if you reacted 49.0g of H3PO4 with 112g of potassium hydroxide, and collected 25.0g of water?

  1. chemistry

    What is the percent yield of NaCl if 31.0 g of CuCl2 reacts with excess NaNO3 to produce 21.2 g of NaCl?

  2. chemistry

    Consider the following reaction: 2H2S (g) + 3O2 (g) --> 2SO2 (g) + 2H2O (g) If O2 was the excess reagent, 1.3 moles of H2S were consumed, and 18.7 g of wat were collected after the reaction has gone to completion, what is the

  3. chemistry

    What is the percent yield of NaCl if 31.0 g of CuCl2 reacts with excess NaNO3 to produce 21.2 g of NaCl

  4. 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

  1. chemistry

    Determine the theoretical and percent yield of hydrogen gas is 36 g of water undergoes electrolysis to produce hydrogen and oxygen and 3.8 g of hydrogen is collected.

  2. Chemistry

    lime, Ca(OH)2 can be used to neutralize an acid spill.A 5.06-g sample of Ca(OH)reacts with excess of hydrochloric acid:6.74 g of calcium chloride is collected what is the percent yield of this experiment Ca(OH)2 + 2HCI ====> CaCl2

  3. 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

  4. 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)

You can view more similar questions or ask a new question.