Mass of Zn Mass Relations in Chemical Reactions Lab Data 129 Mass of Pb and Paper 1.45 g 1.88 g Before Reaction: 0.98 g After Reaction: 0.86 g Mass Zn lost: Calculations: 1. What is the ratio of mass of Pb gained to mass of Zn lost? Call this ratio A. Filter Paper: loss Filter Paper + Pb: Mass Pb gained: .43g

Mass of Zn Mass Relations in Chemical Reactions Lab Data 129 Mass of Pb and Paper 1.45 g 1.88 g Before Reaction: 0.98 g After Reaction: 0.86 g Mass Zn lost: Calculations: 1. What is the ratio of mass of Pb gained to mass of Zn lost? Call this ratio A. Filter Paper: loss Filter Paper + Pb: Mass Pb gained: .43g

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 20CR: Solid calcium carbide (CaC2)reacts with liquid water to produce acetylene gas (C2H2)and aqueous...

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Hydrogen peroxide is used as a cleaning agent in the treatment of cuts and abrasions for several reasons. It is an oxidizing agent that can directly kill many microorganisms: It decomposes upon contact with blood, releasing elemental oxygen gas (which inhibits the growth of anaerobic microorganisms); and it foams upon contact with blood, which provides a cleansing action. In the laboratory, small quantities of hydrogen peroxide can be prepared by the action of an acid on an alkaline earth metal peroxide, such as barium peroxide. BaO2(s)+2HCl(aq)H2O2(aq)+BaCl2(aq) What amount of hydrogen peroxide should result when 1.50 g of barium peroxide is treated with 25.0 mL of hydrochloric acid solution containing 0.0272 g of HCI per mL?
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.
You have a chemical in a sealed glass container filled with air. The setup is sitting on a balance as shown below. The chemical is ignited by means of a magnifying glass focusing sunlight on the reactant. After the chemical has completely burned, which of the following is true? Explain your answer. a. The balance will read less than 250.0 g. b. The balance will read 250.0 g. c. The balance will read greater than 250.0 g. d. The scales reading cannot be determined without knowing the identity of the chemical.
It sodium peroxide is added to water, elemental oxygen gas is generated: :math>Na2O2(s)+H2O(l)NaOH(aq)+O2(g) ppose 3.25 g of sodium peroxide is added to a large excess of water. What mass of oxygen gas will be produced?
hat happens to the weight of an iron bar when it rusts? l type='a'> There is no change because mass is always conserved. i>The weight increases. i>The weight increases, hut it the rust is scraped off, the bar has the original weight. i>The weight decreases. stify your choice and, for choices you did not pick, explain what is wrong with them. Explain what it means for something to rust.
The meat from one hazelnut has a mass of 0.985 g. (a) What is the mass of a millionth of a mole (106) of hazelnut meats? (A millionth of a mole is also called a micromole.) (b) How many moles are in a pound of hazelnut meats?
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?
Sulfur can be recovered from the hydrogen sulfide removed from crude oil deposits, a process known as sweetening, by roasting in air and using the sulfur dioxide initially formed to push the reaction to the final product: H2S(g) + O2(g) --> H2O(g) + SO2(g) H2S(g) + SO2(g) --> H2O(g) + S(s) The maximum number of kilograms of sulfur that can be isolated per kilogram of hydrogen sulfide entering the process is __________.
A 0.6447 g portion of manganese dioxide was added to an acidic solution in which 1.1402 g of a chloride containing sample was dissolved. Evolution of chlorine took place as a consequence of the following reaction: MnO2(s) + 2Cl- + 4H+ ® Mn2+ + Cl2(g) + 2H2O After the reaction was complete, the excess MnO2 was collected by filtration, washed, and weighed, and 0.3521 g was recovered. Express the results of this analysis in terms of percent aluminum chloride. (Al:27.0 ; Mn:55.0 ; O:16.0 ; Cl:35.5 ; H:1.0 g/mol)
Mass Salicylic Acid used 0.1498 g Mass Acetic Anhydride used 0.3417 g Mass filter paper/funnel 7.8668g Mass filter paper/funnel/aspirin 28.7045g Mass aspirin synthesized 0.2295 g based on the data given above. what would the theoretical yield of aspirin be?
Acrylonitrile is used in the production of syntheticfibers, plastics, and rubber goods. It can be preparedfrom propylene (propene), ammonia, and oxygen inthe reaction illustrated below.(a) Write a balanced chemical equation for thisreaction.(b) The actual yield of the reaction is 0.73 kg acrylonitrile per kilogram of propylene. What is theminimum mass of ammonia required to produce1.00 metric ton (1000 kg) of acrylonitrile?
Complete, balance, and write the Q expressions: _C3H8(g) + _O2(g) <--> _CO2(g) + _H2O(g) Q = ___________ _NO(g) <---> _N2O (g) + _NO2(g) Q = ___________ _KOH(aq) +_HOAc(aq) <---> _____(aq) + ___(l) Q = ___________ _Al(s)+_CuSO4(aq) <--> _______(aq)+_Cu(s) Q = ___________