Chemistry Experiment 6 Mole Ratio in a Chemical Reaction Background: Mole ratios of reactants are often times figured out by the use of the other products in a chemical equation. However‚ in the instance that the products’ mole ratios are unknown‚ it can be determined through the experiment. This method is called continuous variations. In this lab‚ I determined the mole ratio between Sodium Hypochlorite and Sodium Thiosulfate by using continuous variations of ratios in a given volume. This reaction
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Determination of the mole ratio of a chemical reaction The method of continuous variations is a means of determining the stoichiometric mole ratio of the reactants in a chemical reaction. The stoichiometric ratio‚ as given by the coefficients in the balanced chemical equation‚ represents the ratio at which chemicals must be combined to produce all product with no excess reactant. Since there is no “wasted” reactant‚ the maximum amount of product is made for the given amount of both reactants
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Mole Ratios Lab October 10‚ 2013 Mrs. Oliver Noah Kent AP Chemistry Block 3/4 Laboratory #4: Mole Ratios I. Hypothesis: If copper wire is placed in an aqueous solution with silver nitrate‚ then silver crystals will grow on the wire surface and the solution will gradually take on the color of Copper (II) ions. The relative quantities of reactants and products in this chemical reaction can be determined by measuring the mass of copper wire consumed in the reaction and the mass of silver crystals
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Reactions Objective In this lab we took Fe(NO3)3 and NaOH and mixed 7 different mole ratios in graduated cylinders to determine what the mole ratio is. We also did the same thing with solutions of CuCl2 and Na3PO4. We determine the mole ratios by graphing the volume of reactant #1 vs. volume of precipitate for each reaction. Data Part 1.) Cylinder 1 2 3 4 5 6 7 Fe(NO3)3‚ 0.1 M‚ ml 5 10 12 15 17 20 24 NaOH‚ 0.1 M‚ ml 55 50 48 45 43 40 36 Fe:OH mole ratio 1:11 1:5 1:4 1:3
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Convert from grams to moles using molar mass. To get moles from grams of potassium chlorate (KClO3): [molar mass = 122.55 g/mol] 138.6 g KClO3 X ( 1 mol / 122.55 g ) = 1.131 mol KClO3 3. Determine the limiting reagent [if necessary] (Use mole ratios to figure out.) * Not necessary to determine because there is only 1 reactant in this decomposition reaction. 4. Use ratios to find the moles of the reactant or product
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Mole Ratio of a Chemical Reaction: Copper & Silver Nitrate Lab #4 OBJECTIVE In this experiment‚ you will determine the number of moles of reactants and products present in the reaction of copper and silver nitrate‚ and calculate their mole-to-mole ratio. The mole-to-mole ratio relating to the disappearance of copper and the formation of silver metal will be used to write the balanced equation for the reaction. The reaction of copper metal with silver nitrate solution is a single
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Shawn Dubbs Lab 1 The Mole Concept of and the Chemical Formula of a Hydrate Abstract: The objective of this lab was to conduct an experiment to analyze the molar components in alum. This was conducted by heating the alum till the water had evaporated and then determining the number of moles for each component. Then using the these amounts to figure out the empirical formula for alum. Results: In order to determine how much of each separate component a total mass was taken before hand for
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2013 Determining the Mole Ratios in a Chemical Reaction Introduction The purpose of this lab was to determine the mole ratios of the reactants hypochlorite ion (OCI ) and thiosulfate (S O ) when reacted in a chemical reaction. A chemical equation gives the mole ratios of the reactants and products involved in the chemical reaction. When some formulas of the products are not known‚ experimental measurements can be made to determine those ratios. During this reaction‚ hypochlorite
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Name Mole Lab Exercises I. Pre Lab Questions Answer the following questions. (Hint: Your textbook will be helpful.) 1. ‘s number is the number of carbon atoms that are present in 12 g of 12C. 2. How many molecules of a compound are in one mole of that compound? 3. Write out the formula for finding percent by mass. 4. Write out the formula for finding Molarity. 5. The Formula Weight of a compound is equal to mole of that compound.
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Name _________________________________________ Date ______________ Period ______________ Chemistry Lab Mole: Measuring Mass as a Means of Counting Purpose: Determine the number of atoms that fit on one tea spoon. 1. Use one clean and dry 50 mL beaker. Place on a balance and press the zero button until the display shows 0.00. 2. Place one level teaspoon of sodium chloride (NaCl) into the beaker‚ determine the mass and record in the table (row 1). 3. Repeat steps 1-2 for CaCO3 4. Repeat steps 1-2
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