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the 3 pages deal with limiting reactant and percentage yield. the mixture starts out as a...
Determine the percent yield of copper. 3. What is the theoretical yield of copper produced by this reaction? Materials: Copper (II) chloride • Aluminum foil • Stirring rod • Two 100 ml beakers • Graduated cylinder • Safety glasses • Spatula or scoopula • Balance Filter paper front counter Funnel • Watch glass Ring stand • Iron ring Safety: Safety glasses must be worn at all times! Copper (II) chloride is an irritant and moderately toxic. Avoid inhaling the powder...
can someone fill in the blanks? Procedure: (1) Reaction between sodium iodide and lead (II) nitrate: Note the appearance 1. Weigh approximately 3.55 g of Nal (0.0237) and place it in the 100 beaker. Record the exact mass in the data table below. Note the a of the Nal crystals in the observation section. 2. Add 30 mL of distilled water to the beaker containing the Nal crystals. S the solution until all of the Nal crystals have dissolved. Record...
Preface: Aluminum foil was reacted will hydrochloric acid and copper 2 chloride. The copper solid from the reaction was placed on filter paper and dried. Data obtained from the lab is below Data Table Mass of Aluminum: 0.29g Mass of filter paper: 0.35g Mass of reacted filter paper: 0.49g Final mass of Copper: 0.11g 10mL of CuCl2: 0.100 CuCl2 molarity Volume of Copper Solution: ? Moles of Copper: 0.001g (0.1 molarity x 0.01 liters) Write an equation to represent the...
can anyone help me fill in the table Write the balanced equation: 2C4504 +2NaOH → Cu(OH) at NaOH. Moles of CuSO4, n = M XL mol 5 x 20 Moles of NaOH, n = MxL 39.997 1225 mol Mass of CuSO4 in the solution Mass of NaOH in the solution 1.59609 009 .9 Limiting reagent Excess reagent Theoretical yield of Cu(OH)2 Mass of filter paper 3777 09 Mass of filter paper and solid product 09 1.339 09 Mass of solid...
Objective Find the ratio of moles of reactant to moles of a product for the reaction below. Compare mass and mole amounts of reactants to determine the amount of products that can be/are made. Background Chemical reactions are represented by balanced chemical equations. Proper interpretation of an equation provides a great deal of information about the reaction it represents and about the substances involved in the reaction. For example, the coefficients in a balanced equation indicate the number of moles...
i need to calculate the theortetical yield by finding the limiting reactant of the experiment by converting reactants to product, then calculate the percent yield using the limiting reactant -in my experiment the amout of crystals i obtained was 1.232 g (watch glass + filter paper = 31.228 g and watch glass, filter paper, + crystals = 32.460 g) REACTION SCHEME H сно, ОН- ОСH, CH panisaldehyde acetophenone Molar Mass: 120.15g/mol Molar Mass: 136.15g/mol Molar Mass: 239.30g/mol Density: 1.119g/mL Density:...
help with # 7 Data Table: Reactant 1 Identity_NaCO,H,O 124.00 g/mol Mass 1.02 g Reactant 2 Identity_MnS0, H,0 169.02 g/mol Mass_1.04 g Observation of chemical reaction. Include observations about color of precipitate! Immediately after adding the two aqueous solutions together a pale pink precipitate formed. 1.49 g Mass of filter paper + precipitate Mass of filter paper Mass of precipitate (actual yield) 0.83 g 0.66 g Analysis: 1. Write the balanced chemical equation for this reaction. 2. Use a solubility...
2. what is the limiting reactant if 0.5g Al is reacted with 3.5g CuCl2? Take into account CuCl2 is a dihydrate when calculating the molecular weight is this EC? Limiting Reactant and Percent Yield Lab Objectives: top 5 colors • Learn to determine the limiting reagent of a reaction. • Learn how to calculate theoretical, actual, and percent yield of a reaction. Background: During a chemical reaction when two substances react, often times one reactant will be consumed before the...
Limiting Reactants, Excess Reactant, and % Yield Name H2+Cl2HCI A gaseous mixture containing 7.5 g of H; gas and 9.00 g of Cl2 gas react to form hydrogen chloride gas. а) Which is the limiting reactant? If all the limiting reactant is consumed, how many grams of HCl are produced? How many grams of excess reactant remain un-reacted? b) c) Cl2+3F22CIF Chlorine reacts with fluorine to form gaseous chlorine trifluoride. You start with 50.0g of chlorine and 95.0g of fluorine....
which reactant is limiting? which reactant is in excess? actual yield of NaCl, show the calculation percent yield of NaCl, show calculation Data 50.00 g Mass of beaker: Mass of beaker and sample (NaHCO3): Mass of sample (NaHCO3): s1.00 g 49.57 g 49.57 g Mass of beaker and residue first heating: Mass of beaker and residue second heating: Mass of beaker and residue third heating (if required): Mass of residue: g 0.43 g mL Volume of concentrated HCl added: Calculations...