If actual amount of alum obtained from 5.502 grams of potassium aluminum sulfate is 3.405 g , what the percent yield of alum? Use exact MM from periodic table, and include a % sign as the unit of your answer.

If actual amount of alum obtained from 5.502 grams of potassium aluminum sulfate is 3.405 g , what the percent yield of alum? Use exact MM from periodic table, and include a % sign as the unit of your answer.

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter9: Chemical Quantities

Section: Chapter Questions

Problem 80AP: Using the average atomic masses given inside the front cover of the text, calculate the mass in...

See similar textbooks

Related questions

Q: Which of the following statements is true? O A The smallest mass of reactant in a chemical reaction…

A: A) option A is not correct because we can not compare amount of substance reacting in terms of it's…

Q: Is the following statement true or false? If you think the statement is flase, rewrite it to make it…

A: The statement given is "The compound or element that is greater in terms of the molar amount is the…

Q: Consider the following unbalanced equation: ___ Na2SiF6(s) + ___…

A: Step -1 Unbalanced equation Na2SiF6 + Na(s)→Si(s)+NaF(s) Find out Mass of NaF produced if 3.75 of…

Q: How many molecules (not moles) of NH3 are produced from 5.01x10-*g of H2? Express your answer…

A: Given: Mass of H2 = 5.01×10-4 g. Balanced chemical reaction is given by,

Q: If 4.0 g of sodium iodide and 4.0 g of chlorine gas react, what are the theoretical yields of both…

Q: Gaseous methane (CH,) reacts with gaseous oxygen gas (0,) to produce gaseous carbon dioxide (CO,)…

A: Given, Gaseous methane (CH4) react with gaseous Oxygen (O2) gas to produce gaseous carbon dioxide…

Q: Question - Balance the following chemical equations: NaClO3 ---> NaCl + O2 When you complete…

A: Given, NaClO3 NaCl + O2 Required, Balance the above chemical…

Q: How many molecules (not moles) of NH3 are produced from 7.04×10−4 g of H2?Express your answer…

A: The balanced chemical equation for the formation of ammonia, NH3 from its constituents nitrogen, N2…

Q: Question - Balance the following chemical equations: C8H18 + O2 ---> CO2 + H2O When you complete and…

Q: When 3.05 moles of CH 4 are mixed with 5.03 moles of O 2 the limiting reactant is?

A: Interpretation- To determine the limiting reagent when 3.05 moles of CH4 are mixed with 5.03 moles…

Q: If the theoretical yield is 3.2 g of product and the percent yield is 79.0% how many grams were…

Q: In the reaction between 7.0 moles of Na and 4.0 moles of Chlorine, to produce NaCl, which of the two…

Q: or the following reaction, 0.549 moles of sulfur dioxide are mixed with 0.192 moles sulfur…

A: The limiting reagent is reactant which is used up in the reaction completely.

Q: Given the experiment shown below, and a product yield of 3.45g. Calculate the theoretical yield and…

A: Note: If u know the molecular weight of starting material and molecular weight of product then you…

Q: What factors during the experiment caused the percent yield to be different than 100%? What…

A: Interpretation: To spot the impurities in the IR data of the product i.e. cyclohexene. The…

Q: If 108.1 grams of water are predicted in a chemical equation that starts with 77.6 grams of H2, but…

A: Given in the question , Mass of water predicted= 108.1 gm Mass of hydrogen used = 77.6 gm Mass of…

Q: What is the percent yield if 5.27 g of copper are produced when 1.87 g of aluminum react with an…

A: Given that: mass of copper = 5.27 g mass of aluminium = 1.87 g The reaction is, 2Al (s) + 3CuSO4…

Q: How many grams of Hz are needed to produce 12.14 g of NH3? Express your answer numerically in grams.

A: Haber process: The Haber Process is used to produce ammonia from nitrogen and hydrogen. The method…

Q: (29) When 35.0 kg of SiO2 reacts with 25.3 kg of carbol recovered, what is the percent yield for the…

Q: When 12 g of carbon is burned in oxygen during an experiment, only 34.9 g of carbon dioxide was…

A: The relation to calculate the percentage yield is shown below.

Q: What is the percent yield of sodium carbonate if 1.330 g of sodium hydrogen carbonate (84.01 g/mol)…

A: Given Reaction :- 2NaHCO3(s) --> Na2CO3(s) + H2O(g) + CO2(g) given amount of NaHCO3(s) = 1.330…

Q: What is the theoretical yield of sodium oxide if you start with 35g of calcium oxide? NaCI Сао CaCl,…

A: Theoretical yield of sodium oxide can be find using mole concept. We can see from reaction that 1…

Q: 5.00 g magnesium is combined with 10.0 g of gaseous chlorine, show by calculation which substance is…

A: Reaction of magnesium with chlorine is: Mg + Cl2 ....> MgCl2 Mass of Mg = 5.00g Molar mass of Mg…

Q: When 12.0 g of carbon is burned in oxygen during an experiment, only 23.6 g of carbon dioxide was…

A: The reaction is C+ O2 --> CO2

Q: what would the slopes of the lines be for a graph of the moles of product versus mole of each…

A: Given Reaction:- 2H2 + O2 ------------> 2H2O Graph is drawn as y versus x. Here we have to draw…

Q: When 12.0 g of carbon is burned in oxygen during an experiment, only 26.1g of carbon dioxide was…

A: The percentage of yield of a reaction= experimental yieldtheoritical yield×100 % The theoretical…

Q: what is the percent yield?

A: Given :- theoretical yield = 9.4 g actual yield = 1.2 g To calculate :- percent…

Q: a) Iron is the main ingredient of steel, an alloy used in many building structures. As oxygen reacts…

A: a) The balanced equation for the reaction of iron with oxygen to form iron (III) oxide. The general…

Q: what is the percent yield?

A: Given :- Actual yield of MgO = 2.48 g Theoretical yield of MgO = 4.13 g To calculate :- Percent…

Q: When the following equation is balanced, the coefficients are NH3 (g) + 02 (g) → NO2 (g) + H2O (g)

A: A chemical equation is said to be balanced when the number of atoms of each element on the left hand…

Q: Balance the chemical equation below using the smallest possible whole number N, (g) + H,(g) NH, (g)

A: This reaction is of formation of ammonia. Known as Haber-bosch process.

Q: Using the number of grams of alum that you actually obtained, calculate the percentage yield of alum…

A: From the 1 mol of Al, 1 mol of alum can be produced if the efficiency is 100 % or yield is 100%. The…

Q: Mg + Cl2 --> MgCl2 If 5.00g of magnesium is combined with 10.0g of chlorine. Calculate the…

A: Determine limiting reagent:

Q: NaC((s) + H,SO,(aq) – Na,so,(s) + _ HCI(g) Balance the equation above. If 32.5 g NaCl and 24.5 g…

A: Mass of NaCl = 32.5 g Mass of H2SO4 = 24.5 g Mass of HCl = 15.5 g

Q: How many grams of sodium sulfide are actually formed if 1.80 g of hydrogen sulfide is bubbled into…

A: Given,Mass of hydrogen sulfide, H2S = 1.80 gMass of sodium hydroxide, NaOH = 2.40 gMoles of H2S and…

Q: The following chemical reaction has helped to shape the Earth's crust: 3 SiO2(s) + 2 Fe3O4(s) →3…

Q: What is the percent yield if 2.08 g of copper are produced when 1.87 g of aluminum react with an…

Q: Use the balanced equation below to answer the question that follows. Al2(50,)3 + 3 MgCl2 2 AICI, + 3…

A: The complete balanced equation =2AlCl3 + 3MgSO4 →Al2(SO4)3 + 3MgCl2Moles of AlCl3 = 8 molesMoles of…

Q: Balance chemical equation given below. HoW much lithium nitride is produced when 20 g of lithium and…

A: In Balanced chemical equation number of atoms of each species are equal on both reactant and…

Q: 90. Phosgene (COCI,) reacts with ammonia (NH,), as shown in this reaction. If 1.2 grams of COCI, are…

A: The reactant which is present in less amount and finished first during the reaction is called…

Q: Consider the following reaction: N: + H: - How many moles of ammonia are produced when 6 moles of…

A: • The given balanced chemical equation is, N2 + 3 H2 → 2 NH3 • The values provided…

Q: What is the percent yield if 4.55 g of copper are produced when 1.87 g of aluminum react with an…

Q: The percentage yield of a reaction is 74.1%. If a calculated value of product that should from using…

A: It is percent ratio of actual yield to the theoretical yield, from Balanced chemical equation.

Q: For the following reaction, 0.141 moles of benzene (C6 H6) are mixed with 0.270 moles of oxygen ga…

A: 2C6H6 (l) + 15O2 (g) --->12CO2 (g) + 6H2O (g) THIS WILL BE THE RXN. O2 WILL BE THE LIMITING…

Q: Methanol can be formed by the following UNBALANCED equation below. How many grams of methanol can be…

Q: Mass of aluminum (g): 0.25g Mass of alum crystals (g): 0.27g 1. Using your starting mass of…

A: Answer: To calculate theoretical yield, we will use the given molar ratio and by equating the ratio…

Q: Balance and complete the following combustion reaction. Enter the sum of the balanced coefficients…

A: Chemical reactions are those reactions which undergo any chemical change. Chemical reaction is…

Question

How do I solve this?

If actual amount of alum obtained from 5.502 grams of potassium aluminum sulfate is 3.405 g , what
the percent yield of alum? Use exact MM from periodic table, and include a % sign as the unit of
your answer.

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

Step 2

Step 3

Step 4

Step 5

Trending now

This is a popular solution!

Step by step

Solved in 5 steps with 2 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

A student isolated 25 g of a compound following a procedure that would theoretically yield 81 g. What was his percent yield?
The text explains that one reason why the actual yield for a reaction may be less than the theoretical yield is side reactions. Suggest some other reasons why the percent yield for a reaction might not be 100%.
For each of the following balanced equations, indicate how many moles of the product could be produced by complete reaction of 1.00 g of the reactant indicated in boldface. Indicate clearly the mole ratio used for the conversion. msp;NH3(g)+HCl(g)NH4Cl(s) msp;CaO(s)+CO2(g)CaCO3(s) msp;4Na(s)+O2(g)2Na2O(s) msp;2P(s)+3Cl2(g)2PCl3(l)
An air bag is deployed by utilizing the following re tion the nitrogen gas produced inflates the air bag): :math>2NaN3(s)2Na(s)+3N2(g) 10.5 g of NaN1 is decomposed, what theoretical mass of sodium should be produced? If only 2.84 g of sodium is actually collected, what is the percent yield?
Solid calcium carbide (CaC2)reacts with liquid water to produce acetylene gas (C2H2)and aqueous calcium hydroxide. l type='a'> Write the balanced equation for the reaction that is (occurring. including all phases. If a 100.0-g sample of calcium carbide (CaC2)is initially reacted with 50.0 g of water, which reactant is limiting? Prove that mass is conserved for the reactant amounts used in pan b.
Using the average atomic masses given inside the front cover of the text, calculate the mass in grams of each of the following samples. l type='a'> 5.0 moles of nitric acid 0.000305 mole of mercury 2.31105mole of potassium chromate 10.5 moles of’ aluminum chloride 4.9104moles of sulfur hexafluoride 1 25 moles of ammonia 0.01205 mole of sodium peroxide
Explain how one determines which reactant in a process is the limiting reactant. Does this depend only on the masses of the reactant present? Give an example of how to determine the limiting reactant by using a Before-Change-After (RCA) table with a balanced chemical equation and reactant starling amounts.
For each of the following unbalanced chemical equations, suppose exactly 5.0 g of each reactant is taken. Determine which reactant is limiting, and calculate what mass of each product is expected, assuming that the limiting reactant is completely consumed. msp;Na(s)+Br2(l)NaBr(s) msp;Zn(s)+CuSO4(aq)ZnSO4(aq)+Cu(s) msp;NH4Cl(aq)+NaOH(aq)NH3(g)+H2O(l)+NaCl(aq) msp;Fe2O3(s)+CO(g)Fe(s)+CO2(g)
The phosphorus pentoxide used to produce phosphoric acid for cola soft drinks is prepared by burning phosphorus in oxygen. (a) What is the limiting reactant when 0.200 mol of P4 and 0.200 mol of 02 react according to P4+5O2P4O10 (b) Calculate the percent yield if 10.0 g of P4O10 is isolated from the reaction.