In a lab, a scientist calculated that he should produce 12.3 grams of product in his experiment. When he is finished collecting his product, it weighs 10.1 grams. What is his percent yield? * 82.1% 0.82% 10.1% O 12.2%

In a lab, a scientist calculated that he should produce 12.3 grams of product in his experiment. When he is finished collecting his product, it weighs 10.1 grams. What is his percent yield? * 82.1% 0.82% 10.1% O 12.2%

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Related questions

Q: Use the References to access important values if needed for this question. For the following…

A: Step 1: GivenNaCl (aq) + AgNO3 (aq) → AgCl (s) + NaNO3 (aq) Mass of NaCl = 25.3 gMass of AgNO3 =…

Q: A student sets up the following equation to solve a problem in solution stoichiometry. (The ? stands…

Q: Aqueous hydrobromic acid (HBr) reacts with solid sodium hydroxide (NaOH) to produce aqueous sodium…

A: Answer: This question is based on the stoichiometric calculation of the reaction that we have…

Q: How many molecules of carbon dioxide, CO2, are in 4.77 x 10.2 g of the molecule? O1.26 x 1024…

Q: For the following reaction, 3.75 grams of carbon disulfide are mixed with excess chlorine gas. The…

Q: For the following reaction, 4.44 grams of oxygen gas are mixed with excess hydrochloric acid. The…

A: The balanced equation for the reaction is 4 HCl (aq) + O2 (g) ------> 2 H2O (l) + 2 Cl2 (g)…

Q: Use the Conservation of Mass Interactive to answer the question. Consider the reaction. MnS(s) + 2…

Q: During a lab experiment, 10.5 grams of NaNO3 were reacted. The students produced 9.92 grams of…

Q: In the lab, a student generates 0.450 g of a product in an experiment. The student then calculates…

A: Given :- product obtained from an experiment = 0.450 g Theoretical yield of product = 0.398 g To…

Q: As part of the third-year chemistry lab curriculum students synthesize the compound phospbomolybdic…

A: Where WH, Wp, WMo, Wo are atomic weight of hydrogen, phosphorus, molybdenum and oxygen respectively.…

Q: A student begins the experiment with a 0.5287 g sample of aluminum can. At the start of week 2, the…

A: Given: Mass of Al = 0.5287g Mass of Potassium KAl(SO4)2∙12H2O = 5.0109g

Q: grams

Q: For the following reaction, 65.1 grams of barium hydroxide are allowed to react with 40.9 grams of…

A: Mass of Ba(OH)2 = 65.1 gMolar Mass of Ba(OH)2 = 171.34 g/moleNo of moles of Ba(OH)2 = Mass of…

Q: A student is trying to figure out how many moles of potassium chloride are made from 4,0 grams of…

A: To get the anwer we must convert the amount of chlorine gas into moles & then multiply it by 2,…

Q: After working hard all day, a researcher has produced 849.7206 grams of the targeted product. Before…

Q: A chemist is to be carrying out an experiment in which he reacts solid copper with a silver nitrate…

Q: Consider the reaction: NO + Br2 → NOBr For every 75 g NO, Find the mass of Br2 reacted. Find the…

Q: Balance the chemical equation given below, and determine the number of grams of MgO needed to…

Q: NH3, reacts with oxygen gas to form nitrogen monoxide, NO, and water. If an 8.5 g sample of ammonia…

A: The mass of ammonia (NH3) is 8.5 g.The mass of nitrogen monoxide (NO) formed (observed yield) is…

Q: Consider the following unbalanced chemical equation: Al + CuCl → Cu + AlCl3 If 72.8 grams of…

A: Balanced chemicalequation Au(s) + 3 CuCl = 3Cu(s)+ AlCl3 Given 72.8 gram Cucl moles of CuCl =…

Q: A student started with 1.525 grams of copper (II) oxide and produced 3.500 g of copper (II) sulfate.…

Q: A sample of 48.0 g of tetraphosphorous decoxide (P4010) reacts with 46.0 g of water to produce…

Q: Gaseous butane (CH3(CH₂)₂CH3) reacts with gaseous oxygen gas (0₂ to produce gaseous carbon dioxide…

A: To determine the theoretical yield of water formed from the reaction of butane and oxygen gas,

Q: For the following reaction, 11.2 grams of glucose (C6H12O6) are allowed to react with 15.5 grams of…

A: First we need to find the limiting reactant. It is the reactant that gets consumed first. To find…

Q: Methyl salicylate (C₂H8O3) (density = 1.18 g/mL) is dissolved in 100 mL of 6.0 M NaOH, and heated…

A: Theoretical is defined as the maximum amount of the product that can be formed in a given chemical…

Q: Mr. Ragusa asks Hannah to make copper crystals from the following reaction. Cu(NO3)2 + 2Na -->…

A: Here we are required to find the percent yield of the experiment

Q: If 41.9g of oxygen react with 8.7g of hydrogen and experimentally produce 2.3mol of water, what is…

A: The reaction between hydrogen and oxygen produces water. The balanced chemical equation for this…

Q: Consider the reaction of solid aluminum iodide and potassium metal to form solid potassium iodide…

A: Solid aluminum iodide and potassium metal to form solid potassium iodide and aluminum metal. The…

Q: Consider the following data. Determine the percent yield of copper. mass copper turning (g) 0.6929…

A: This can be calculated by using the following formula, Percent Yield = (Actual yield/Theoreticial…

Q: Convert 3.75464287098739e+25 molecules of CO2 to grams of carbon? Convert 2.72106521624284e+25…

A: Given that : 1) We have to convert 3.75464287098739 x 1025 molecules of CO2 to grams of carbon. 2)…

Q: You want to calculate the mass of Reactant B that will react completely with 45 grams of Reactant A.…

A: To calculate the mass of reactant B that will react with the 45 gram of reactant A:

Q: A student begins the experiment with a 0.5287 g sample of aluminum can. At the start of week 2, the…

A: Given: Mass of aluminium = 0.5287 g. And the mass of potassium alum KAI(SO4)2.12H20 produced…

Q: produced

A: The chemical reaction for manufacturing of Methanol is given as; Co + 2H2 ---> CH3OH Mass of CO…

Q: A 23.4 g23.4 g sample of magnesium reacts with excess silver nitrate to produce silver metal and…

A: Given : Mass of magnesium metal i.e Mg taken = 23.4 g And the mass of final mixture of metals = 62.6…

Q: Butane gas, C4H10, is a common fuel found in cigarette lighters. When butane burns, it combines with…

A: Mass of butane = 5 g The balanced reaction is – 2C4H10 g + 13O2 g→8CO2 g+ 10H2Og

Q: 328.8 g SO2(g), 425.3 g CaCO3(s), and 105.7 g 02(g) react as follows: 2 SO2(g) + 2 CaCO3 (s) + 02(g)…

A: Mass of SO2= 328.8 g Mass of CaCO3= 425.3 g Mass of O2=105.7 g

Q: If you react a solution that has 5.6 g of AgNO3 with excess NaCl, what mass of AgCl is produced.…

A: Given reaction AgNO3 (aq) + NaCl(aq) → AgCl(s) + NaNO3(aq)Mass of AgNO3 = 5.6 gMolar mass of…

Q: Aqueous sulfuric acid (H₂SO4) will react with solid sodium hydroxide (NaOH) to produce aqueous…

A: To calculate the maximum mass of sodium sulfate (Na2SO4) that could be produced by the chemical…

Q: Which of the following statement is correct about theoretical and percent yields? Select an answer…

A: Given statements are - a. A percent yield is always smaller than a theoretical yield. b. A…

Q: 4. When propane (C3H3) undergoes complete combustion in oxygen, it produces carbon dioxide and…

Q: Aqueous hydrobromic acid (HBr) reacts with solid sodium hydroxide (NaOH) to produce aqueous sodium…

A: The given data is as follows: The mass of sodium bromide produced = 1.68 g The mass of hydrobromic…

Q: Sodium reacts with oxygen to form sodium oxide according to the reaction below. _Na (s) + _O₂ (g) →…

Q: Safrole, one of the flavor molecules in sassafras, contains only C, H, and O. Combustion of 10.0 g…

A: Given that - Safrole contains only Carbon, Hydrogen and oxygen as constituent elements. On heating…

Q: 4HF (aq) + SiO2 (s) → SiF4 (g) + 2H₂O(1) A chemist needs to know what mass (in grams) of silicon…

Q: For the reaction whose balanced equation is as follows, find how many grams of zinc phosphate will…

A: The balanced chemical equation for the reaction is given as: 3 ZnCl2 + 2 (NH4)3PO4 → Zn3(PO4)2 + 6…

Question

In a lab, a scientist calculated that he
should produce 12.3 grams of
product in his experiment. When he is
finished collecting his product, it
weighs 10.1 grams. What is his
percent yield? *
82.1%
0.82%
10.1%
O 12.2%

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 2 steps

SEE SOLUTION Check out a sample Q&A here

Similar questions

10 KNO3 (s) + 8 C (s) +3 S (s) → 2 K2CO3 (s) + 3 K2SO4 (s) + 6 CO2 (g) + 5 N2 (g) If 75.35 grams of each reactant are combined in a reaction chamber and allowed to react completely, what is the total mass of solids after the reaction is finished? Your calculation should include contributions from reactants that are left over AND products that are formed - but remember, only solids. Answer in grams
A chemist needs to add 3.5 moles NaClNaClto a reaction. How much NaCl should she measure out in grams (g)? Round to two decimal places if necessary. 140.21g NaCl 204.54g NaCl 58.44g NaCl 0.60g NaCl
A student sets up the following equation to solve a problem in solution stoichiometry. (The ? stands for a number the student is going to calculate.) Enter the units of the student's answer. (0.19 L) 1 mL 10-³ 146.86 g mol 1.04 mL = ☐ x10 ロ･ロ X I 00
Let us explore a reaction with a limiting reactant. Here, zinc metal is added to a flask containing aqueous HCl, and H2 gas is a product. The three flasks each contain 0.300 mol of HCl. Zinc is added to each flask in the following quantities: 4.90 g, 9.81 g, 19.6 g. When the reactants are combined, the inflates the balloon attached to the flask. The results are as follows: Flask 1: Balloon inflates completely, but some remains when inflation ceases. Flask 2: Balloon inflates completely. No Zn remains. Flask 3: Balloon does not inflate completely. No Zn remains. What mass of Zn was added to each flask? Mass = ? g (flask 1) Mass = ? g (flask 2) Mass = ? g (flask 3)
[Tutorial: Limiting reactant stoichiometry] This question will walk you through the steps of calculating the mass of products produced based on your determination of the limiting reactant. b) Step 2a: Use dimensional analysis to determine the theoretical yield of the product. Calculate the theoretical yield in grams Al₂O₃ from the complete reaction of 64.7 grams Al according to the following balanced chemical equation: 2 Al(s) + Fe₂O₃(s) → Al₂O₃(s) + 2 Fe(s) c) Calculate the theoretical yield in grams Al₂O₃ from the complete reaction of 201 grams Fe₂O₃ according to the following balanced chemical equation: 2 Al(s) + Fe₂O₃(s) → Al₂O₃(s) + 2 Fe(s) d) Which of the following substances is the limiting reactant? e) What is the mass in grams of the excess Fe₂O₃ remaining after the partial reaction of 201 g Fe₂O₃ with 64.7 g Al? Give your answer to three significant figures.
Consider the recipe for making tomato and garlic pasta. 2 cups noodles +12 tomatoes +3 cloves garlic 4 servings pasta If you have 7 cups of noodles, 27 tomatoes, and 9 cloves of garlic, how many servings pasta can you make? Which ingredient limits the amount of pasta that it is possible to make?
Solutions of sodium carbonate and silver-nitrate react to form solid silver carbonate and a solution of sodium nitrate. A solution containing 8.00 g of sodium carbonate is mixed with one containing 4.00 g of silver nitrate. After the reaction is complete, the solutions are evaporated to dryness, leaving a mixture of salts. How many grams of each of the following compounds are present after the reaction is complete? sodium carbonate 1.52 silver nitrate 0 X 9 sodium nitrate 12.84 ✓ q silver carbonate 6.48 X g X 9 D
zinc + sodium hydroxide + water → sodium zinc hydroxide + hydrogen gas If 180.20 grams of sodium hydroxide are reacted with 5.0 × 1022 particles of water, how many moles of hydrogen gas will be produced if the reaction proceeds with an 82.749% yield? **I already know how to balance the equation. I need help calculating the percent yield with “x” product. Do I find the limiting reagent first and then multiply that by the given % yield?**
Can someone help me out with the conversion aspect of this question? Im getting the answer right but the conversion wrong
A 6.60-g sample of Fe3O4 reacts with O₂ to produce Fe₂O3: 4Fe3O4(s) + O2(g) →→→ 6Fe2O3(s) Determine the number of g of Fe₂O3 produced, assuming that O₂ is in excess. Enter your answer in the provided box. g Fe₂O3
Consider the chemical reaction : 2 Na3PO4 + 3 CaCl2 → Ca3(PO4)2 + 6 NaCl, if the theoretical yield for a reaction is 5.7 grams and the percent yield is 51, what is the actual yield? Round and report your answer to the first decimal place without unit.
Use 1 decimal point for all atomic masses. 12.3 g of NCl3(g) are reacted with 0.605 g of H2(g) by the following reaction NCl3(g) + 3H2(g) --> NH3(g) + 3HCl(g) What is the limiting reagent? NCl3(g) H2(g) Based on the limiting reagent, what should the yield of NH3(g) be? g