Identifying precipitation, combustion and acid-base reactions. Classify each chemical reaction:type of reaction(check all that apply)reactioncombinationprecipitationsingle replacementcombustion2Na (s) + F, (g)2Na F (s)double replacementacid-basedecompositioncombinationprecipitationHCI (aq) + NaOH (aq) → NaCI (aq) + H,0(1)NaCI (aq) + н,о(0single replacementcombustiondouble replacementacid-basedecompositioncombinationprecipitationMg (C1o,), («) →Mg Cl, (s) + 30, (g)single replacement O combustiondouble replacementacid-basedecompositioncombinationprecipitationMgl, (a9) + Pb (NO,), (aq) → Me (NO,), (ae) + Pbl,(-)single replacement O combustion2double replacementacid-basedecomposition000 000 000 000O000O00

According to the answering guidelines, I'm posting the solution for the first 3 problems. Kindly…

Classify each chemical reaction: type of reaction (check all that apply) reaction combination precipitation single replacement O combustion 2Na (s) + F, (g) 2Na F (s) double replacement O acid-base decomposition combination precipitation single replacement O combustion H C1 (aq) + Na OH (aq) Na CI (aq) + H,0 (1) double replacement acid-base decomposition combination precipitation O combustion Mg (C10,),(«) single replacement → M&C1, (6) + 30,(g) double replacement acid-base decomposition 000

Classify each chemical reaction: type of reaction (check all that apply) reaction combination precipitation single replacement O combustion 2Na (s) + F, (g) 2Na F (s) double replacement O acid-base decomposition combination precipitation single replacement O combustion H C1 (aq) + Na OH (aq) Na CI (aq) + H,0 (1) double replacement acid-base decomposition combination precipitation O combustion Mg (C10,),(«) single replacement → M&C1, (6) + 30,(g) double replacement acid-base decomposition 000

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

Similar questions

Complete and balance the following acid-base and acid-carbonate reactions. (Use the lowest possible whole number coefficients.) (a) HCl + Ba(OH)2 → (b) HCl + Al2(CO3)3 → (c) H3PO4 + LiHCO3 → (d) Al(OH)3 + H2SO4 →
Magnesium oxide is sometimes used as an antacid to help with indigestion and stomach upset caused by excess stomach acid (hydrochloric acid). Write two balanced chemical equations to explain how this works. One should be a synthesis and the other a neutralization.
A precipitation reaction involves the formation of a precipitate when aqueous solutions are mixed. Not all combinations of aqueous solutions produce precipitates, and it is important to be able to predict the ones that do. A) Complete and balance the molecular equation for the reaction between aqueous solutions of lithium fluoride and potassium chloride, and use the states of matter to show if a precipitate forms. B) Write the complete ionic equation for the reaction that takes place when aqueous solutions of lithium fluoride and potassium chloride are mixed. C) Write the net ionic equation for the precipitation reaction, if any, that may occur when aqueous solutions of lithium fluoride and potassium chloride are mixed. If there is no net ionic equation, simply write "none."
Solving for a gaseous reactant.
Write the balanced neutralization reaction that occurs between sodium hydroxide and acetic acid.
4. Write an equation for the reaction of aqueous sulfuric acid and aqueous barium hydroxide. Indicate the physical states of all reactants and products. 5. Write an equation for the reaction of aqueous phosphoric acid and magnesium metal. Indicate the physical states of all reactants and products. 6. Write an equation for the reaction of aqueous phosphoric acid and aqueous sodium bicarbonate. Indicate the physical states of all reactants and products.
Solving for a gaseous reactant.
Define and give an example of each of the following classes of reactions: precipitation, acid–base, gas evolution, redox (noncombustion), and combustion. Each group member can do one, and then present his or her reaction to the group.
Nitrogen dioxide dissolves in water to form nitric acid and nitric oxide.
Define and give an example of each of the following classes of reactions: precipitation, acid–base, gas evolution, redox (noncombustion), and combustion. Each group member can do one and then present the reaction to the group.
Write balanced chemical equations for each of the following reactions (including states of matter). Classify each reaction as a combination reaction, decomposition reaction, single or double displacement reaction, hydrocarbon or metal combustion reaction. The products copper metal and water vapor are produced when copper(II) oxide reacts with hydrogen gas.