You seem to be assuming the formula of the salt is CuG where G is gluconate. The process that you will use to determine the coefficients is called continuous variations. Most of the elemental copper will be on the aluminum wire. Collect and wash the copper produced in the reaction. The original sample weighed 42. Finding the Simplest Formula 1.
We will not do your homework for you, so don't ask. The best fit gives you a ratio that results from evaluating all the data as a whole, not just choosing the highest value and calling it the best ratio. In a chemical equation, the stoichiometric ratio will allow the reaction to consume as many reactants as possible and form as much product as capable, so when the measurable property during a continuous variations experiment reflects the same idea, it is clear that this method is effective in finding the mole ratio. Wash the copper twice more with small amounts of distilled water. There seems to be some confusion about gluconate.
Note: Report the ratio to the closest whole number. Data Table Mass of crucible g 13. I need to log off for now. During the experiment, a constant volume of reactants was kept to ensure that the total number of moles of the reaction was also constant. Do not overheat the compound.
I am going to refer to you as my chemical engineer friend and quote your last statement to my professor and see what she says. It would have been higher if it weren't for our realization that we were supposed to pour the entire beaker onto the filter paper in the funnel. Measure out about 20 cm of aluminum wire, coil the wire, and place the wire in the beaker of solution so that it is completely immersed in the copper chloride solution. I wasn't given the formula but this is what I have come up with so far. Identifying the mole to mole ratio of the reactants allows further stoichiometric calculations to be made.
The expected product is MgO, so the 1-to-1 mole ratio Mg to O in the product is all that is required. Determine the formula for this hydrate. Remove the filter paper with the copper from the funnel and leave it to dry. Experimental Notes Equipment List Caution: Eye protection is essential. The purpose of this lab is to discover the optimum ratio of the two reactants, meaning that the greatest amount of reactants have been consumed and the greatest amount of product has been formed; this identifies the ratio of moles of reactants in the reaction. Use a glass stirring rod to scrape off as much copper as possible from the Al wire.
Please complete any questions as much as you can before posting. Obtain and wear goggles 2. At some point, you might want to make a fresh post, focussed on specific questions that remain. This is an online chemistry course provided by eScience Labs and so far I am severely disappointed. Lab 2 - Determination of the Empirical Formula of Magnesium Oxide Goal and Overview The quantitative stoichiometric relationships governing mass and amount will be studied using the combustion reaction of magnesium metal. Without knowing being given the information that the chemical formula for gluconate is C12H22O14, there is absolutely no way to determine any more information about the the compound. Mass of magnesium compound 7.
I just don't know where to go from here. I do not know if this is the correct ratio or not, but I think that because it asks where errors could have occurred, that it not being exact is acceptable. Mass of oxygen in the product 8. Neither you, nor the coeditors you shared it with will be able to recover it again. Note the color change, from blue-green to brownish, as the water of hydration is driven out of the crystals.
Moles of Mg 0 00 56355H mole Show calculations. Heating the product again causes the loss of water and conversion of the hydroxide to the oxide. The reaction is exothermic, thus the mixture that generates the most heat energy will be the reaction that completely consumes both the hypochlorite and the thiosulfate ions. The empirical formula of a compound gives the lowest whole-number ratio of the constituent atoms that is consistent with the mass ratios measured by experiment. After heating to remove the waters of hydration, the sample weighed 27. It is also important that you describe the specific part of the problem you are struggling with. The lack of a gluconate structure or even formula is especially disturbing.
I happened to note that point. Gently swirl the beaker to completely dissolve the solid. This reactant is completely consumed, and it therefore limits the amount of product that can be formed. Typically the mole ratios of reactants and products can be found from a balanced chemical equation, however when the formulas of the products are unknown, experiments can be conducted to discover this ratio. During the chemical reaction, these reactants will produce some sort of measurable property, be it color, a precipitate, or in this instance, heat.
I think we may have hit a dead end. Mass of empty crucible+ cover 7 384 2. You will use this mixture to establish the coefficients, and therefore the mole ratio, for the reaction. As previously stated, when given a balanced chemical equation the mole ratios of reactants and products is expressed by the coefficients of those formulas. This ensured that the temperature change had to be a result of the quantity of reactants being consumed, because there would be the same total volume of reactants.