You determined the theoretical yield for Znl2 if 0.5 moles of zinc is used to form Znl2. Determine the percent yield if 189.6 g of Znl2 product is recovered. Zn +12 → _Znl2
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- A chemist setup a synthesis of phosphorus trichloride by mixing 12.0gP with 35.0gCl _(2) and obtained 42.4gPCl _(3). Calculate the percentage yield of this compound. P(s)+Cl_(2)(g)->PCl _(3)(l) Please type answer note write by hendA natural brine found in Arkansas has a bromide ion concentration of 5.00 × 10−3 M. If 210. g Cl2 were added to 1.00 × 103 L of the brine, determine the limiting reactant. calculate the theoretical yield of Br2 (d = 3.12 g/mL).A sample of 70.5 g of potassium phosphate is added to silver nitrate, resulting in the formation of solid Ag3PO4. Calculate the percent yield, if you conduct this reaction and you are able to isolate 66.0 g of the precipitate that forms. Group of answer choices: 50.0% 62.9% 93.6% 47.5%
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- Which substance can not produced in the reaction between three substances: C2H5Cl, C3H7Cl and Na? Select one:a. C5H12b. C7H16c. C6H14d. C4H10In the reaction between CO and Fe3O4 , the theoretical yield in an experiment is calculated to be 47.2 g Fe. When a careless chemistry student carries out the experiment, the actual yield is 42.9 g Fe. Calculate the percentage yield. Is this correct answer 90.9%?The following information was recorded by a student team working to prepare nickel sulfate. Plan: Prepare NiSO4 by reacting NiO with 6 M H2SO4 The expected product is NiSO4·6H2O. We will filter the crystals from the reaction solution to get the product. NiO + H2SO4 --> NiSO4 + H2O molar mass of NiO: 74.69 g/molmolar mass of NiSO4: 154.75 g/mol molar mass of NiSO4·6H2O: 262.85 g/mol mass of NiO used: 7.5 gvolume of 6M H2SO4 used: 50 mL heated the solution for 30 minutes, cool and filtered the crystals mass of product: 17.4 g Two students calculated percent yield using this data. One student got 66.2% and another got 112%. Based on this information, which of the following statements are true. One or more statements are correct. Group of answer choices The percent yield of 112% was calculated using the molar mass for the hydrated product. The percent yield of 66.2% was calculated using the molar mass for the anhydrous product. Both percent yields are incorrect because…
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