If 25.0 g potassium metal are reacted with 25.0 g oxygen gas to yield 17.98 g potassium oxide, whatis the percent yield of this reaction?耳99+ahpJETPACKDepartment of Health Care SevicesPO. Box 2088Rancho Cordova, CA 95741-2088ORIALA STANIKZAMOUCAMONGA CA

4K + O2 ---> 2K2O Mass of K2O formed by 25 g of potassium metal = 25 g K × (1 mol K/39.0983 g K)…

Answered: If 25.0 g potassium metal are reacted…

If 25.0 g potassium metal are reacted with 25.0 g oxygen gas to yield 17.98 g potassium oxide, what is the percent yield of this reaction?

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter3: Chemical Reactions

Section: Chapter Questions

Problem 71QRT

See similar textbooks

Related questions

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

Q: Calculate the percent yield of a reaction?

A: Yield is the measure of the quantity of moles of product formed in relation to the product consumed…

Q: For a theoretical yield of 2.54 g and percent yield of 82.8583%, calculate the actual yield for a…

A: Given data, Theoretical yield = 2.54 g % yield = 82.8583% Then, Actual yield = ?

Q: If 30. g of a 67% by mass solution of potassium hydroxide reacts with 20. g of aluminum nitrate,…

Q: If the theoretical yield of a reaction is 0.118 g and the actual yield is 0.104 g, what is the…

A: The given data contains, Theoretical yield = 0.118 g. Actual yield = 0.104 g.

Q: Nitrogen and oxygen react as follows: N₂(g) +202(g) → 2NO₂(g) Suppose 1.85 mol of N₂ and 48.0 g of…

A: The correct answer is given below

Q: What is the theoretical yield (in grams) of potassium chloride when 2.500 grams of potassium metal…

A: Potassium metal reacts with chlorine gas to produce potassium chloride. The mass of potassium is =…

Q: 13.0 g of aqueous sodium phosphate reacts with 35.0 g of aqueous barium nitrate. If 17.0 g of…

A: The Question is based on the concept of Reaction Stoichiometry. First , we have to identify the…

Q: The theoretical yield for a reaction was 150 grams and actually 126 grams of the product were made,…

A: Given: Theoretical yield of the reaction = 150 g. Actual yield of the reaction = 126 g. We have to…

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: Copper(II) carbonate was used by artists as a pigment due to its bright green-blue colour. It can be…

Q: For the following reaction, 0.173 moles of nitrogen gas are mixed with 0.453 moles of hydrogen gas.…

A: Given,

Q: For the following reaction, 4.95 grams of nitrogen gas are allowed to react with 4.11 grams of…

Q: An excess of oxygen reacts with 451.4 g of lead, forming 366.9 g of lead(II) oxide. Calculate the…

Q: For the following reaction, 0.271 moles of nitrogen gas are mixed with 0.565 moles of hydrogen gas.…

A: To find limitng reagent mole-mole analysis is applied on balanced chemical reaction.

Q: What is the percent yield of a reaction if it had a theoretical yield of 125g but an actual yield of…

A: The equation for percent yield is: percent yield = (actual yield/theoretical yield) x 100% Where:…

Q: For the following reaction, 4.52 grams of hydrogen gas are mixed with excess iodine. The reaction…

A: Given :- hydrogen(g) + Iodine(s) → Hydrogen iodide (g) mass of Hydrogen = 4.52 g actual yield of…

Q: It is desired to produce 7.05 grams of bromine monochloride by the following reaction. If the…

A: Given : Percent yield of reaction = 92.7 % Mass of product required = 7.05 g We need to determine…

Q: For the following reaction, 6.09 grams of hydrogen sulfide are mixed with excess oxygen gas. The…

A: Interpretation- Here given 6.09g of hydrogen sulfide are mixed with excess of oxygen gas . The…

Q: The percent yield for a given reaction is 75%. If the theoretical amount is predicted to be 3.58g,…

A: Percent yield of the reaction is equal to the ratio of actual yield and theoretical yield multiplied…

Q: For the following reaction, 5.06 grams of bromine are mixed with excess chlorine gas . The reaction…

Q: If 101 g of CaO and 280. g of NH4Cl are mixed, what is the limiting reactant, and what mass of NH3…

A: Given:Mass of CaO = 101 gMass of NH4Cl = 280.0 gBalanced chemical reaction is given by,

Q: Calcium carbonate decomposes on heating as shown in the chemical equation. When 50 g of calcium…

A: Recall the equation %yield = (Experimental yield/Theoretical yield)×100

Q: For the following reaction, 6.63 grams of nitrogen gas are mixed with excess oxygen gas . The…

Q: For the following reaction, 6.18 grams of nitrogen gas are mixed with excess hydrogen gas . The…

A: To solve this problem first we have to write the balanced chemical equation then according to the…

Q: How many moles of sodium sulfate are produced when 120 g of sodium hydroxide reacts with sulfuric…

A: Dear student, since you have asked multiple questions but according to guidelines we will solve 1st…

Q: How many moles of O2 are produced when 1.26 moles of H,O is reacted?

A: 2 H2O -----> 2 H2 + O2 2 moles of H2O react to produce 2 moles of H2 and 1 mole of O2.

Q: The percent yield for a given reaction is 60%. If the theoretical amount is predicted to be 8.33 g,…

A: Given: Percent yield= 60% Theoretical yield= 8.33 g

Q: If 25 g of iron (II) chloride reacts with 48 g of sodium phosphate, what is the limiting reagent?…

A: This is done via Mole Mole analysis and By finding out limiting Reagent.

Q: For the following reaction, 3.77 grams of chlorine gas are mixed with excess iron. The reaction…

Q: The theoretical yield of product for a particular reaction is 32.03 g. A very meticulous student…

Q: If 67 grams of ammonium perchlorate were to react with 10 grams of aluminum: i. Which material would…

Q: In a reaction to produce sulfuric acid, the theoretical yield is 300. g. What is the percent yield…

A: Therotical yield of H2SO4 = 300 g Actual yield of H2SO4= 111.4 g

Q: If 25.0 g potassium metal are reacted with 25.0 g oxygen gas to yield 22.37 g potassium oxide, what…

A: A numerical problem based on mole concept, which is to be accomplished.

Q: For the following reaction, 5.92 grams of hydrogen gas are mixed with excess nitrogen gas . The…

Q: For the following reaction, 6.87 grams of iodine are mixed with excess hydrogen gas . The reaction…

Q: Consider the following unbalanced equation for the combustion of pentane: if a 20.4 g sample of…

A: Given that 20.4 g pentane react with excess oxygen.

Q: If 5.3 g of hydrogen gas is reacted with 12.6 g of oxygen gas to produce water, which reactant is…

A: Given, mass of hydrogen = 5.3 g mass of oxygen = 12.6 g

Q: Barium and sulfur react with each other in a synthesis reaction. If 0.7850 g of sulfur reacts with…

Q: For the following reaction, 28.1 grams of bromine are allowed to react with 17.1 grams of chlorine…

A: We have Br2(g) + Cl2(g)→2BrCl(g) Here 28.1 g of bromine are allowed to react with 17.1 g of…

Q: Magnesium metal reacts with hydrochloric acid to for magnesium chloride and hydrogen gas according…

A: Given data,Mass of Mg=0.5003gGiven reaction,Mg+2HCl→MgCl2+H2

Q: According to the following reaction, how many grams of calcium oxide will be formed upon the…

Q: If 23 grams of iron (II) chloride reacts with 41 grams of sodium phosphate, what is the limiting…

A: Given: Mass of iron (II) chloride (FeCl2) = 23 g Mass of sodium phosphate (Na3PO4) = 41 g Molar mass…

Q: For the following reaction, 33.5 grams of iron are allowed to react with 18.8 grams of oxygen gas.…

A: 4Fe + 3O2 → 2 Fe2O3Molecular weight of…

Q: 56 grams of iron (III) sulfate reacts with 24 grams of lead (IV) nitrate a. Calculate the mass of…

A: As per our company guidelines we are supposed to answer only first three sub-parts. kindly repost…

Q: If the yield of the picric acid synthesis reaction is 65% what mass of picric acid what mass will it…

A: The synthesis of picric acid reaction is as follows,

Q: if 15.0 mol of iron combines with excess chlorine gas, and 12.2 mol of FeCl3 is produced. what is…

A: Given Number of mole of iron = 15 mole Number of mole of FeCl3 = 12.2 mole % yield = ?

Q: Barium and phosphorus react with each other in a synthesis reaction. If 0.2856 g of phosphorus…

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

If 25.0 g potassium metal are reacted with 25.0 g oxygen gas to yield 17.98 g potassium oxide, what
is the percent yield of this reaction?
耳
99+
a
hp
JETPACK
Department of Health Care Sevices
PO. Box 2088
Rancho Cordova, CA 95741-2088
ORIALA STANIKZA
MOUCAMONGA CA

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

VIEW

Step 2

VIEW

Step 3

VIEW

Step by step

Solved in 3 steps

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

Consider the following mixture of SO2(g) and O2(g). If SO2(g) and O2(g) react to form SO3(g), draw a representation of the product mixture assuming the reaction goes to completion. What is the limiting reactant in the reaction? If 96.0 g of SO2 react with 32.0 g O2, what mass o f product will form?
Consider the hypothetical reaction between A2 and AB pictured below. What is the balanced equation? lf 2.50 moles of A2 are reacted with excess AB, what amount (moles) of product will form? If the mass of AB is 30.0 u and the mass of A2 are 40.0 u, what is the mass of the product? If 15.0 g of AB is reacted, what mass of A2 is required to react with all of the AB, and what mass of product is formed?
The reaction of methane and water is one way to prepare hydrogen for use as a fuel: CH4(g) + H2O(g) CO(g) + 3 H2(g) If this reaction has a 37% yield under certain conditions, what mass of CH4 is required to produce 15 g of H2?
Write the balanced chemical equation for the complete combustion of adipic acid, an organic acid containing 49.31% C, 6.90% H, and the remainder O, by mass.
DDT, an insecticide harmful to fish, birds, and humans, is produced by the following reaction: In a government lab, 1142 g of chlorobenzene is reacted with 485 g of chloral. a. What mass of DDT is formed, assuming 100% yield? b. Which reactant is limiting? Which is in excess? c. What mass of the excess reactant is left over? d. If the actual yield of DDT is 200.0 g, what is the percent yield?
Ammonia gas can be prepared by the following reaction: CaO(s) + 2 NH4Cl(s) 2 NH3(g) + H2O(g) + CaCl2(s) If 112 g of CaO and 224 g of NH4Cl are mixed, the theoretical yield of NH3 is 68.0 g (Study Question 12). If only 16.3 g of NH3 is actually obtained, what is its percent yield?
One mol of ammonia reacts with 1.00 mol of oxygen to form nitrogen oxide and water according to the reaction 4NH3(g)+5O2(g)4NO(g)+6H2O(l)State which statements are true about the reaction and make the false statements true. (a) All the oxygen is consumed. (b) 4.00 mol NO are produced. (c) 1.50 mol H2O are produced. (d) The description of the experiment does not provide enough information to determine percent yield. (e) Three moles of water are produced for every two moles of NO obtained.
In Example 4.2, you found that a particular mixture of CO and H2 could produce 407 g CH3OH. CO(g) + 2H2(g) CH3OH (l) If only 332 g of CH3OH is actually produced, what is the percent yield of the compound?
4.44 Industrial production of hydrogen gas uses the reaction shown below. If 1.00 metric ton of propane reacting with excess water yields 270 kg of H2, what is the percentage yield? C3H8(g)+3H2O(l)3CO(g)+7H2(g)
Phosphine gas reacts with oxygen according to the following equation: 4PH3(g)+8O2(g)P4O10(s)+6H2O(g) Calculate (a) the mass of tetraphosphorus decaoxide produced from 12.43 mol of phosphine. (b) the mass of PH3 required to form 0.739 mol of steam. (c) the mass of oxygen gas that yields 1.000 g of steam. (d) the mass of oxygen required to react with 20.50 g of hosphine.
Methane (CH4) is the main component of marsh gas. Heating methane in the presence of sulfur produces carbon disulfide and hydrogen sulfide as the only products. a. Write the balanced chemical equation for the reaction of methane and sulfur. b. Calculate the theoretical yield of carbon disulfide when 120. g of methane is reacted with an equal mass of sulfur.