The percent yield of this reaction is 77.0%. 2Al(s) + 3 F2 (g) →→→ 2AIF3 (s) - Determine the mass, in grams, of the actual (experimental) yield of the product, if excess fluorine gas reacts with 134.0 g of aluminum metal. Round to the nearest whole number. Answer:

The percent yield of this reaction is 77.0%. 2Al(s) + 3 F2 (g) →→→ 2AIF3 (s) - Determine the mass, in grams, of the actual (experimental) yield of the product, if excess fluorine gas reacts with 134.0 g of aluminum metal. Round to the nearest whole number. Answer:

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: For the following unbalanced chemical equation, suppose 10.6 g of each reactant is taken. Show by…

Q: Time's Up! This question will walk you through the steps of determining which reactant is limiting…

A: Given values -> Weight of O2 = 81.7gm Molar mass of O2 = 32gm/mole Molar mass of CO2=…

Q: For the following reaction, 0.308 moles of hydrogen gas are mixed with 0.189 moles of ethylene (C2…

Q: (2)For the following balanced reaction use the mass of the chemical provided to solve the mass of…

Q: 5. A student reacts 6.00 g of ammonium sulfide with 6.00 g of zinc (II) acetate. Upon completion of…

A: Limiting reactant :- A reactant which is present in lesser number of molrs than required as per…

Q: For the following unbalanced chemical equation, suppose 10.1 g of each reactant is taken. Show by…

A: We have been given a reaction and we have been given mass of each reactant =10.1g.We have been asked…

Q: Part A - Calculate the mass (in grams) of the product formed when 15.30 g g of Cr completely reacts.…

Q: Find the mass of O2 required to also burn.

Q: 2. A student performed the synthesis of wintergreen oil and recorded the following data. Mass…

Q: indicate that the coefficients indicate the number of moles that combine and are formed in the…

A: Given, that the coefficients indicate the number of moles that combine and are formed in the…

Q: This question will walk you through the steps of determining which reactant is limiting based on a…

A: “Since you have posted a question with multiple sub-parts, we will solve first three sub-parts for…

Q: Suppose 16.04g of methane is burnt in oxygen gas. a)what are the products of the reaction? b)what…

A: We have given that Mass of methane = 16.04g To find the mass of oxygen need to burn the methane gas…

Q: Consider the following balanced reaction: Al2O3 + 3H20 → 2Al(OH)3 If 2.44 x 1020 Al203 formula units…

A: Number of moles is calculated by dividing given mass with molecular mass.

Q: Consider the balanced equation SiO2(s)+3C(s)→SiC(s)+2CO(g) Complete the following table showing the…

A: The balanced chemical reaction is given below.

Q: TUTOR Limiting Reactants: Compare Reactant Moles The theoretical yield of a reaction is the amount…

A: Welcome to bartleby !

Q: 5. Consider the reaction between HCI and O2: 4 HCI (9) + 02 (9) → 2 H2O (1) + 2 Cl2 (g) When 63.1 g…

Q: A student is asked to balance the reaction: CH4 + O2 CO₂ + H₂O What convention of balancing is…

A: A balanced chemical equation is an equation in which equal number of atoms of each type are present…

Q: 1.05 gg H2H2 is allowed to react with 10.3 gg N2N2, producing 1.09 gg NH3NH3. Part A What is the…

A: For this question, first calculate moles for both reactant. Then use mol to mol ratio for reactant…

Q: (b) Aluminium reacts with chlorine gas to produce aluminium chloride. Al(s) + Ch(g) → AICh(/) i)…

A: Aluminium reacts with chlorine to form aluminium chloride. the equation for the chemical reaction is…

Q: Consider the following two-step reaction sequence. 2HCI + CaCO3 → CaCl2 + CO2 + H2O 2NazPO4 + 3CaCl2…

Q: consider the following balanced equation. N2O4(l) + 2 N2H4(l) → 3 N2(g) + 4 H2O(g) Determine the…

A: Given, N2O4(l) + 2 N2H4(l) → 3 N2(g) + 4 H2O(g) Given, mass of N2O4 react = 60.0 g mass of N2H4…

Q: 6. Magnesium oxide can be produced by heating magnesium metal in the presence of oxygen. The…

A: The balance chemical reaction : 2Mg(s) + O2(g) ---> 2MgO(s) Mass of Mg = 10.1 g Mass of O2 =…

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

Q: .A balanced chemical reaction and an incomplete reaction map are hown below. What number is missing…

A: 2NaN3 = 3N2+2Na

Q: Determine the Limiting Reactant if 10.0 g of Copper (1) oxide reacts with 5.00 g of oxygen according…

A: Limiting reagent is those reactant which is completely consumed in the chemical reaction . Or,which…

Q: Consider the following reaction: 4 NH3 +3 02 → 2 N2 + 6H₂O A researcher begins by placing 6.1 g of…

A: mass of NH3 = 6.1 gmolar mass of NH3 = 17.03 g/molmass of O2 = 7.8 gmolar mass of O2 = 32.00…

Q: 6) Oxygen gas and hydrogen gas combine to make water according to the following chemical reaction.…

A: Limiting reagent is the reagent which is consumed in the chemical reaction completely. It decides…

Q: n dioxide reacts with elemental carl SiO2(s) + 3 C(s) → Si SiO2 reacts with excess carbon, 7.2 first…

Q: The drawing below shows a mixture of molecules: carbon nitrogen oxygen key hydrogen sulfur chlorine…

A: Supposed the following chemical reaction take place in this mixture:2H2(g) + O2(g) ---->…

Q: The reaction between aluminum and iron(III) oxide can generate temperatures approaching 3000°C and…

Q: a. For the following unbalanced chemical equation, suppose 10.3 g of each reactant is taken. Show by…

A: Given : The unbalanced reaction The mass of each reactant To find : Write the balanced chemical…

Q: For the following reaction, 0.343 moles of sulfuric acid are mixed with 0.223 moles of calcium…

A: Given :- Sulfuric acid (aq) + calcium hydroxide (s) → calcium sulfate (s) + water (l) No.of moles…

Q: Ammonia can be generated by heating together the solids NH4Cl and Ca(OH)2. Other products of the…

A: Given, The mass of NH4Cl = 33.0 g. The mass of Ca(OH)2 = 33.0 g. The percentage yield of ammonia =…

Q: a. For the following unbalanced chemical equation, suppose 10.4 g of each reactant is taken. Show by…

A: The answer for this problem is provided below in great details within the attached figure.

Q: - Consider a 3.52-g sample of CaCO3 (99.87% pure) in a flask and a 100.0 mL sample of vinegar (5%…

Q: For the following reaction, 20.1 grams of iron are allowed to react with 32.2 grams of chlorine gas.…

Q: The theoretical yield of a reaction is the amount of product obtained if the limiting reactant is…

Q: Consider the Haber-Bosch process for the synthesis of ammonia from its elements. Calculate the…

A: Given reaction is, N2 (g) + 3 H2 (g) → 2 NH3 (g) Amount of N2 = 59.8 g H2 is present in excess

Q: If 5.45 g of potassium chlorate are decomposed to form potassium chloride, 1.75 g of oxygen gas are…

A: Step 1:Step 2:

Q: Use the References to access important values if needed for this qu For the following reaction,…

Q: 5.0 g of nitrogen is reacted with 5.0 g of hydrogen to produce ammonia according to the chemical…

A: In the given question->Weight of N2 = 5.0 gmWeight of H2 = 5.0 gm-> first of all we calculate…

Q: A sample of a substance (containing only C, H, and N) is burned in oxygen. 2.341 g of CO₂,…

A: Mass of the initial sample burned = (mass of C) + (mass of H) + (mass of N) Mass of C(MW = 12.01…

Q: determine the theoretical yield of the product. Calculate the theoretical yield in grams Al₂O₃ from…

Q: the reaction starts out with 352 particles of A and 315 particles of B, what is the ideal…

Q: a. For the following unbalanced chemical equation, suppose 10.6 g of each reactant is taken. Show by…

A: a) Limiting reactant: A reactant that is totally consumed when the chemical reaction is completed is…

Concept explainers

Stoichiometry

Stoichiometry is a chemical division that evaluates the quantitative content of the chemical process with the help of the reacting molecules or products taking part in the reaction. The term “stoicheion” in “Stoichiometry”, is an old Greek term for "element" whereas “metron” means "measure".

Question

The percent yield of this reaction is 77.0%.
2Al(s) + 3 F2 (g) → 2AlF3 (s)
Determine the mass, in grams, of the actual (experimental) yield of the product, if excess
fluorine gas reacts with 134.0 g of aluminum metal.
Round to the nearest whole number.
Answer:
SAN J
0.0

Expert Solution

This question has been solved!

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

SEE SOLUTION Check out a sample Q&A here

Step 1: Formula for percent yield

VIEW

Step 2: Calculate actual yield

VIEW

Solution

VIEW

Step by step

Solved in 3 steps with 3 images

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

The reaction between aluminum and iron(III) oxide can generate temperatures approaching 3000°C and is used in welding metals: 2Al + Fe2O3 Al2O3 + 2Fe. In one process, 148 g of Al is reacted with 601 g of Fe₂O3. Calculate the mass (in grams) of Al2O3 formed, and determine the amount of excess reagent left at the end of the reaction. Mass of Al2O3 formed: g Amount of excess reagent: g of What is the limiting reactant?
Calculate the theoretical yield of the product in moles for each of the initial quantities of reactants. Ti(s) + 2Cl2(g) -> TiCl4(s)
An excess of sodium carbonate, Na2CO3, in solution is added to a solution containing 17.87 g CaCl2. After performing the experiment, 12.51 g of calcium carbonate, CaCO3, is produced. Calculate the percent yield of this reaction.
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?**
Enter the coefficients directly from the balanced chemical equation. Do not reduce to lowest terms. For example: If 3 moles H2 react with 3 moles 02, enter "3" for each, not "1". According to the following reaction: 2Na (s) + 2H20 (I) –→ 2NaOH (aq) + H2 (g) What would you multiply "moles of sodium" by to convert to the units "moles of hydrogen" ? (number) (unit) = moles H2 moles Na (number) (unit)
Solve this exercise without using a calculator. The reaction 6 ClO₂(g) + 2 BrF3 (1) →6 ClO₂F(s) + Br₂ (1) is carried out with 12 mol ClO₂ and 5 mol BrF3. (a) Identify the excess reactant. (b) Estimate how many moles of each product will be produced and how many moles of the excess reactant will remain.
I would need help to answer the following question. In the chemical industry, determining the quantity of substances to be produced in chemical reactions is considered extremely important. The area of chemistry that determines the amount of reactants to be used and the amount of products to be obtained in chemical reactions is Stoichiometry. Considering the context above and your knowledge acquired during classes, for the reaction below calculate the amount of oxygen gas required to produce 13.5 moles of water, H2O(g), in the complete combustion of acetylene, C2H2(g)? C2H2(g) + O2(g) → CO2(g) + H2O(v)
Below is a combustion reaction that is not completed nor balanced. Water and carbon dioxide are produced. Complete and balance the reaction first. C4H10 (g) + O₂(g) → How many molecules of butane (C4H10) are used when 0.887 g of oxygen gas is consumed? Upload an image or PDF file that clearly shows all work with units and labels where necessary. Include: • The completed and balanced equation The 4-step stoichiometry calculation
For the following reaction, 0.224 moles of sulfuric acid are mixed with 0.417 moles of calcium hydroxide. sulfuric acid (aq) + calcium hydroxide(s) → calcium sulfate(s) + water() What is the formula for the limiting reagent? Limiting reagent: What is the maximum amount of calcium sulfate that can be produced? Amount = moles
For the following reaction, 0.472 moles of carbon (graphite) are mixed with 0.594 moles of oxygen gas. carbon (graphite)(s) + oxygen(g) → carbon dioxide(g) What is the formula for the limiting reagent? What is the maximum amount of carbon dioxide that can be produced? moles
how do I do this step by step?
Give a clear handwritten answer