* 0∞ LL # m Classify each chemical reaction: type of reaction (check all that apply) reaction combination O precipitation Na, CO, (;) → Na,0(s) + co,(g) single replacement combustion double replacement acid-base decomposition O precipitation O combustion combination single replacement NaC1(aq) + AGNO, (aq) NANO, (ag) + A9C1(s) dd ble replacement acid-base decomposition combination precipitation single replacement combustion (3)o H7 + (8)F0ɔ (8) 07 + (3)*HƆ O decomposition A double replacement 7 acid-base combination precipitation HI(ag) + NaOH (ag) Nal (ag) + H, O(1) single replacement combustion double replacement acid-base decomposition Explanation Check O2022 McGraw H 80 F Cloudy F2 F4 F5 F7 F8 F10 ゴ $ & 5. ) 7. 8. R. H.

The dilution equation, rearranged to solve for ?1 is   ?1=?2?2?1 where ?1 and ?1 are the initial concentration and volume, respectively, and ?2 and ?2 represent the final concentration and volume, respectively. A student needs to prepare 50.0 mL of 1.10 M aqueous H2O2 solution from 4.8 M H2O2 stock solution. Set up an equation to solve for the volume of stock solution needed by plugging the given values into the equation.

Be sure to specify states such as (aq) or (s). If a box is not needed leave it blank. When aqueous solutions of sodium phosphate and calcium iodide are combined, solid calcium phosphate and a solution of sodium iodide are formed. The net ionic equation for this reaction is: + +

Which set of reactants forms a solid precipitate when mixed? O NANO3(aq) and KCI(aq) O Na2CO3(aq) and KOH(aq) O Na2CO3(aq) and CuCl2(aq) O CuCl2(aq) and NaC2H3O2(aq)

What is(are) the classification(s) of the reaction below? (Choose all that applies.) AGNO3(aq) + KCI(aq) → AgCI(s) + KNO3(aq) addition reaction single displacement reaction combustion reaction double displacement reaction acid-base neutralization reaction gas-forming reaction O precipitation reaction redox reaction decomposition reaction

For each of the reactions, calculate the mass (in grams) of the product formed when 15.67 g of the underlined reactant completely reacts. Assume that there is more than enough of the other reactant. 2K(s)+Cl2(g)−−−−−→2KCl(s) 2K(s)+Br2(l)−−−−−→2KBr(s) 4Cr(s)+3O2(g)−−−−−→2Cr2O3(s) 2Sr(s)−−−−+O2(g)→2SrO(s)

Does a reaction occur when aqueous solutions of potassium phosphate and iron(III) nitrate are combined? O yes O no If a reaction does occur, write the net ionic equation. (Use the solubility rules provided in the OWL Preparation Page to determine the solubility of compounds. Be sure to specify states such as (aq) or (s). If a box is not needed leave it blank.) +

How can we complete and balance

Which one of the following is not a redox reaction? O Cl2(g) + 2KBr(aq)Br2() + 2KCI(aq) O Zn(s) + H2SO4laq) → ZnSO4(aq) + H2(g) 2H2(g) + O2(g) → 2H20() O 6FESO4(aq) + K2Cr207(aq)+ 7H2SO4(aq) - Cr2(SO4)3(aq) + 3FE2(SO4)3(aq)+ K2SO4(aq) + 7H20() H20() + NH3(g) → NH4*(aq) + OH (aq) Previous Page Next Page

Classify each chemical reaction: type of reaction (check all that apply) reaction combination precipitation single replacement O combustion HCI(aq) + NaOH (aq) NaCl(aq) + н,о() double replacement acid-base decomposition combination precipitation single replacement O combustion 2Na (s) + F, (g) - 2NaF (s) double replacement acid-base decomposition combination precipitation single replacement combustion 2CH,CH, (g) + 70, (g) 4CO, (g) + 6H,0(g) double replacement acid-base decomposition combination precipitation single replacement combustion Na, S (aq) + FeCl, (aq) → 2NaCI(aq) + FeS (s) double replacement acid-base decomposition ? O O O