Can the Charge of Iron be Calculated in a Single Replacement Reaction With Copper (II) Sulfate, and Can a Hydrate be Predicted From an Initial and Final Mass? Sometimes atoms have more or less electrons than they do protons. These atoms are known as ions, any atom or molecule that has an ionic charge. Some atoms or molecules have “common” ionic charges, or a number of electrons that is normal for them. An example of this is sulfate, or which has an ionic charge of 2-, which means it has 2 more electrons than protons. Now atoms that have negative ionic charges are known as “anions”. Atoms that have positive ionic charges are known as “cations”. Cations and anions will bond to usually form ionic charges of 0. In two of our experiments, we used copper (II) sulfate, or CuS. Since copper has a charge of 2+, and sulfate has a charge of 2-, the new charge of copper (II) sulfate is 0. Copper is the cation, and sulfate is the anion. In some reactions, possibly involving sulfate, one cation is replaced by another. This is only possible when the latter cation is more reactive than the original. This occurred in our first experiment, where iron replaced copper because iron is more reactive. Another compound associated with bonds and reactions is a hydrate. A hydrate is a compound or element that has bonded with water. There is a ratio between the water molecules and the elemental molecules. These definitions are very interesting, but not very useful unless stoichiometry is studied. Stoichiometry is the relationship between substances in an equation or reaction. Stoichiometry primarily uses moles to calculate masses, volumes, and amounts of substances. By finding the relationship between two substances, the amount of each specific substance can then be calculated. These terms and definitions are key in the experiments conducted in this report, and crucial in both parts. PART 1 INTRO: After the aforementioned definitions and terms were defined, a problem arose. If iron was added to copper (II) sulfate in a single replacement reaction, and the final copper was found, could the charge of the iron be found? So essentially, if in a single replacement reaction, the final standalone cation’s mass was known and the initial standalone cation’s mass was known, could one calculate the charge of the initial cation? In equation form this appears as such: . The charge of the iron ion was unknown. Iron only has two common charges, 2+ and 3+. If in this reaction iron (II) was used then the full chemical equation and reaction would occur as:. Now we knew the initial iron we would be using in this reaction, 2.00 g of iron filings. However, we didn’t know the charge. So if 2g of iron were used and the iron in question was iron (II), then we could expect a certain amount of copper using these equations: 2g Fe/55.845 (g/mol) Fe = .03581 moles. 55.845 (g/mol) is the molar mass of iron. So we would have .03581 moles of iron. Then, .03581 moles Fe * 1 mol Cu/1 mol Fe = .03581 moles Cu. We multiplied the moles of iron by 1 over 1 because there is 1 mole of iron for every mole of copper. Then, .03581 moles Cu * 63.556 (g/mol) Cu = 2.2756 g Cu. 63.556 (g/mol) is the molar mass of copper. If the iron was iron (II), then 2.2756 grams of copper would be produced from the reaction. Now if the iron was iron (III), then a new equation can be formed: . To calculate the amount of copper in this experiment, these equations were used: 2g Fe/111.69 (g/mol) Fe = .01791. 55.845 (g/mol) is the molar mass of iron, and there are two moles of iron. So we would have .01791 moles of iron. Then, .01791 moles Cu * 190.638 (g/mol) Cu = 3.4143 g Cu. 63.556 (g/mol) is the molar mass of copper, and there are 3 moles of copper. So if the iron was iron (III), then 3.4143 grams of copper would be produced as a result. Our hypothesis was that the iron would be iron (II) and produce 2.2756 grams of copper as a result. In this experiment, iron was the independent
Stoichiometry Lab Report
Karla WadeChoza, Jonathan Guerrero, Luis Martinez
March 11, 2013
In this lab, we mixed together the reactants, 0.05 moles of baking soda and some vinegar into a flask. The
products were the carbon dioxide, water, and sodium acetate. After mixing these chemicals together, we
boiled the flask until all the liquid in the solution was gone.
The purpose of doing this experiment was to practice using stoichiometry in a real lab…
The term stoichiometry is derived from the Greek words στοιχεῖον stoicheion "element" and μέτρον metron "measure". In patristic Greek, the word Stoichiometria was used by Nicephorus to refer to the number of line counts of the canonical New Testament and some of the Apocrypha.
Stoichiometry rests upon the very basic laws that help to understand it better, i.e., law…
Title: The Reaction between Iron Power & Copper (II) Sulfate which Produces Iron (II) Sulfate & Copper Metal when Placed on a Hot Plate Mixed with Distilled Water. – Lab #4
Purpose/Problem: To determine the percent yield of copper using the theoretical yield and the actual yield from the experiment.
Hypothesis: If this experiment is conducted correctly then it will be easy to be able to produce the correct actual yield and be able to figure out the percent yield.
quantitative analysis technique that potentially could be used for the determination of the amount of copper in a sample. Using a two-step reaction sequence, copper(II) oxide will be synthesized from a weighed amount of copper(II) sulfate pentahydrate.
Stoichiometry allows us to use the balanced equation to calculate the amounts of product and/or reactant involved in a reaction. Because the starting material will be a pure compound, it will be possible - to check the validity of the technique by comparing…
SOLUTION STOICHIOMETRY (EXP. #1)
Maria Ann Di Stefano
October 2nd 2014
In this experiment, there will be evaluation of the solution stoichiometry of the reaction between calcium chloride ( CaCl2) and sodium carbonate (Na2CO3) carried out in a aqueous solution.
Here, aliquots of sodium carbonate and calcium chloride solutions are mixed to gives us the following reaction equation:
Na2CO3 (aq) + CaCl2 (aq)…