OWLV2 |.- E My Black Documen Sign in to UMasso ot [References) A few hydrogen and oxygen molecules are introduced into a container in the quantities depicted in the following drawing. The gases are then ignited by a spark, causing them to react and form H2o. - H, D - 0, a. Write a balanced chemical equation for the reaction, (Use the lowest possible coefficients. Omit states of matter.) b. What is the limiting reactant? OThere is no limiting reactant. OH2 O02 imber of water molecules that can be formed in the chemical reaction? c. What is the water molecules 8 item attempts remaining Submit Answer Try Another Version

11. Mrs. Parris demonstrates a reaction between a metal and a dissolved salt (aqueous). Balance the equation below and determine the mass of nickel produced when 15.4 grams of magnesium reacts with 20.0 grams of Ni(NO,), to produce Mg(NO,), Label the theoretical yield and limiting and excess reactant. (6.42 g Ni = ty, Ni(NO,), = LR) 3D Mg 15.4 grams _Ni(NO,), → 20.0 grams Ni + _Mg(NO,); +

Report Sheet: Exp. 15: PERIODIC PROPERTIES NOTE: All chemical equations must be balanced and must include physical states or phases. Name of partner: I. Reactivity with Water A. Lithium, Sodium and Potassium Describe the reaction of each metal with water. Include specific identification of the products formed. Na and H6₂0 Q-1 Q-2 feezing k and H₂0 feezing Li aindl H₂0 feezing Write the balanced chemical equation for each reaction: Q-3 and Q-4 turn smoke andl Pink ignition turn Pink Clear Rank:

II AM Lab data percent yield carbon dioxide.pdf Name Sect Percent Yield of Carbon Dioxide To predict the amount of carbon dioxide gas that should be produced in a Purpose: chemical reaction. Then calculate the amount of carbon dioxide actually produced and determine the percent yield. The reaction is represented in the equation below: CH,COOH + NaHCO, → NaCH,C00 + H20 + CO2 Materials: sodium bicarbonate (aka baking soda), acetic acid solution (aka vinegar), Erlenmeyer flasks, balance .Procedure: 1. Measure and record the mass of a 250-mL Erlenmeyer flask. Label it as flask A. 2. Add approximately 7.5 g of sodium bicarbonate to flask A. 3. Measure and record the mass of a second 250-ml Erlenmeyer flask. Call it flask B. 4. Add approximately 75 g of acetic acid solution to flask B. 5. Slowly add acetic acid to flask A until the reaction has stopped. Do not add all of the vinegar; just enough to complete the reaction. 6. After the reaction has stopped, measure and record the masses of…