Classify each chemical reaction: 2CH₂CH₂(g) +70, (g) → 4CO₂(g) + 6H₂O(g) KOH(aq) + HBrO (aq) reaction → KBrO₂ (aq) + H₂O(1) Mgl₂(aq) + Pb(NO3)₂ (aq) → Mg(NO3)₂(aq) + PbI₂ (s) KOH(aq) + HBrO (aq) → KBrO (aq) + H₂O(1) type of reaction (check all that apply) combination single replacement double replacement decomposition combination Osingle replacement double replacement Odecomposition combination Osingle replacement O double replacement decomposition combination O single replacement double replacement Odecomposition X precipitation combustion acid-base Oprecipitation combustion acid-base precipitation combustion acid-base precipitation combustion acid-base

From the chemical equation below, what is the oxidizing agent? 2Cr^3+(aq) + 6Cl^1-(aq) --> 2Cr(S) + 3Cl2 (g)

Write the balanced equation for the reaction that occurs:   Pb(NO3​)2​(aq)+Na2​SO4​(aq)-->   Write the overall ionic equation for the balanced equation you wrote above.   Write the net ionic equation for this reaction.

A 4.50 g sample of limestone (impure CaCO3) was dissolved in 0.1M HCl solution according to the following equation.   CaCO3(s) + 2HCl(aq) → CaCl2 (aq) + CO2 (g) + H2O (l)   Excess of (NH4)2C2O4(aq), was added to the resulting solution to precipitate the calcium ions as calcium oxalate, CaC2O4(s). Ca2+(aq) + C2O42-(aq) → CaC2O4 (s)   The precipitate was filtered, dried and weighed at 2.15 g.   (Show your work)                                                                                                 a)    Determine the percentage by mass of calcium carbonate (CaCO3) in the limestone sample. (MM of CaCO3 is 100.09 g/mol)   b) Why we need to dry the precipitate until we get a constant mass?   c) Is the precipitate of calcium oxalate (CaC2O4) stable and in the final form or not? Explain.