The molar mass of hydrogen (H) is 1 g/mol, the molar mass of chlorine (CI) is 35g/mol, and the molar mass of zinc (Zn) is 65 g/mol. When 130 grams of zinc reactcompletely in hydrochloric acid (HCI), how much is the total mass of the products?2HCl(aq) + Zn(s) → ZnCl2(aq) + H2(g)○ 270 g○ 144 g274 g130 g

Answered: Image /qna-images/answer/5d3db222-9a4a-4c13-a128-fd1557a277e2.jpg

Answered: The molar mass of hydrogen (H) is 1…

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter4: Stoichiometry

Section: Chapter Questions

Problem 4.16PAE: 4.16 Many metals react with halogens to give metal halides. For example, iron reacts with chlorine...

See similar textbooks

Similar questions

4.24 Ammonia gas can be prepared by the reaction CaO(s)+2NH4Cl(s)2NH3(g)+H2O(g)+CaCl2(s) If 112 g of CaO reacts with 224 g of NH4Cl, how many moles of reactants and products are there when the reaction is complete?
4.69 The pictures below show a molecular-scale view of a chemical reaction between H2 and CO to produce methanol, CH3OH. The box on the left represents the reactants at the instant of mixing, and the box on the right shows what is left once the reaction has gone to completion. Was there a limiting reactant in this reaction? If so, what was it? Write a balanced chemical equation for this reaction. As usual, your equation should use the smallest possible whole number coefficients for all substances.
4.108 Elemental analysis is sometimes carried out by combustion of the sample. For a hydrocarbon, the only products formed are CO2 and H2O. If a 1.36-g sample of an unknown hydrocarbon is burned and 2.21 g of H2O is produced along with 4.07 g of CO2, what is the empirical formula of the hydrocarbon?
4.16 Many metals react with halogens to give metal halides. For example, iron reacts with chlorine to give iron(II) chloride, FeCl2: Fe(s)+Cl2(g)FeCl2(s) Beginning with 10.0 g iron, what mass of Cl2, in grams, is required for complete reaction? What quantity of FeCl2, in motes and in grams, is expected?
You take 1.00 g of an aspirin tablet (a compound consisting solely of carbon, hydrogen, and oxygen), burn it in air, and collect 2.20 g CO2 and 0.400 g H2O. You know that the molar mass of aspirin is between 170 and 190 g/mol. Reacting 1 mole of salicylic acid with I mole of acetic anhydride (C4H6O3) gives you 1 mole of aspirin and 1 mole of acetic acid (C2H4O2). Use this information to determine the molecular formula of salicylic acid.
The final step in the manufacture of platinum metal (for use in automotive catalytic converters and other products) is the reaction 3 (NH4)2PtCl6(s) 3 Pt(s) + 2 NH4Cl(s) + 2 N2(g) + 16 HCl(g) Complete this table of reaction quantities for the reaction of 12.35 g (NH4)2PtCl6.
A titanium ore contains rutile (TiO2) plus some iron oxide and silica. When it is heated with carbon in the presence of chlorine, titanium tetrachloride, TiCl4, is formed. TiO2(s)+C(s)+2Cl2(g)TiCl4(g)+CO2(g) Titanium tetrachloride, a liquid, can be distilled from the mixture. If 35.4 g of titanium tetrachloride is recovered from 18.1 g of crude ore, what is the mass percentage of TiO2 in the ore (assuming all TiO2 reacts)?
The reaction of equal molar amounts of benzene, C6H6, and chlorine, Cl2, carried out under special conditions completely consumes the reactants and yields a gas and a clear liquid. Analysis of the liquid shows that it contains 64.03% carbon, 4.48% hydrogen, and 31.49% chlorine, and has a molar mass of 112.5 g/mol. Write the balanced equation for this reaction.
What mass of HCI, in grams, is required to react with 0.750 g of Al(OH)3? What mass of water, in grams, is produced? Al(OH)3(s) + 3 HCI(aq) AlCl3(aq) + 3 H2O(l)
Disulfur dichloride, S2Cl2, is used to vulcanize rubber. It can be made by treating molten sulfur with gaseous chlorine. S8() + 4 Cl2(g) 4 S2Cl2(g) Complete this table of reaction quantities for the production of 103.5 g S2Cl2.
4.84 Aluminum chloride (AlCl3) is used as a catalyst in the production of polyisobutylene, which is used in automobile tires. Scrap aluminum metal reacts with chlorine gas (Cl2) to produce AlCl3. Suppose that 2.70 g of Al and 7.10 g of Cl2 are mixed. What is the maximum mass of AlCl3 that could be formed?
The pictures below show a molecular-scale view of a chemical reaction between the compounds AB2 and B2. (Green balls represent B atoms and orange balls are A atoms). The box on the left represents the reactants at the instant of mixing, and the box on the right shows what is left once the reaction has gone to completion. Was there a limiting reactant in this reaction? If so, what was it? Write a balanced chemical equation for this reaction. As usual, your equation should use the smallest possible whole number coefficients for all substances.

Recommended textbooks for you

Chemistry for Engineering Students

Chemistry

ISBN:

9781337398909

Author:

Lawrence S. Brown, Tom Holme

Publisher:

Cengage Learning

Chemistry & Chemical Reactivity

Chemistry

ISBN:

9781337399074

Author:

John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:

Cengage Learning

Chemistry & Chemical Reactivity

Chemistry

ISBN:

9781133949640

Author:

John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:

Cengage Learning

Chemistry for Engineering Students

Chemistry

ISBN:

9781337398909

Author:

Lawrence S. Brown, Tom Holme

Publisher:

Cengage Learning

Chemistry & Chemical Reactivity

Chemistry

ISBN:

9781337399074

Author:

John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:

Cengage Learning

Chemistry & Chemical Reactivity

Chemistry

ISBN:

9781133949640

Author:

John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:

Cengage Learning

Chemistry: An Atoms First Approach

Chemistry

ISBN:

9781305079243

Author:

Steven S. Zumdahl, Susan A. Zumdahl

Publisher:

Cengage Learning

Chemistry

ISBN:

9781133611097

Author:

Steven S. Zumdahl

Publisher:

Cengage Learning

Chemistry

ISBN:

9781305957404

Author:

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

Publisher:

Cengage Learning

SEE MORE TEXTBOOKS