Mix Reactants Lab

In the study of chemical reactions, chemistry students first study reactions that go to completion. Inherent in these familiar problems—such as calculation of theoretical yield, limiting reactant, and percent yield—is the assumption that the reaction can consume all of one or more reactants to produce products. In fact, most reactions do not behave this way. Instead, reactions reach a state where, after mixing the reactants, a stable mixture of reactants

In chemical reactions, the significance of knowing the limiting reactant is high. In order to increase the percent yield of product, increasing the limiting reactant, possibly, is the most effective. In this experiment we were able to calculate limiting reactants from the reaction of CaCl2. 2H2O + K2C2O4.H2O(aq).

A chemical reaction is when substances (reactants) change into other substances (products). The five general types of chemical reactions are synthesis (also known as direct combination), decomposition, single replacement (also known as single displacement), double replacement (also known as double displacement), and combustion. In this lab, the five general types of chemical reactions were conducted and observations were taken before, during, and after the reaction. Then the reactants and observations were used to determine the products to form a balanced chemical equation. The purpose of this lab was to learn and answer the question: How can observations be used to determine the identity of substances produced in a chemical reaction?

The purpose of this lab was to determine the limiting reactant in a reaction between copper sulfate and iron. Using the reaction between copper sulfate and iron, the reaction was observed to see the reaction and transformation of matter. The copper sulfate was placed into a beaker, as the excess reactant, then iron filings added until the heated solution was completely reacted. This reaction created an excess of leftover. The law of conservation of mass can be observed in this reaction, and using the data found, the percent yield calculated.

What is the percentage yield of the reaction of iron and copper chloride when steel wool and copper chloride dehydrate are used as reactions?

The study of the quantitative relationships between the amounts of reactants used and the amounts of products formed by a chemical reaction is called stoichiometry.

Both experiments were able to determine the yield of hydrogen gas by testing the effect of limiting reactants, balanced equations, stoichiometry, mole ratios and molar masses. Balanced equations are equations that have a balanced number of moles of each element on both sides of the equation. Molar mass is the sum of the atomic masses of all elements combined in a chemical substance. Mole rations can be determined using the coefficients of the reactants and products in the balanced equation. Mole ratios can be used to relate moles of product formed from a certain number of moles of a reactant. Stoichiometry is the method of using the relationship between two or more substances in a chemical reaction. The limiting reactant of a chemical reaction is the reactant that is used up first in the reaction and limits how much of the product can be formed. In experiment 2-1, a company wanted to know if magnesium or aluminum would be practical to use as an alternative to zinc to produce a given volume of hydrogen gas. In experiment 2-2, the company wants to know how to optimize the production of hydrogen gas and whether hydrochloric or sulfuric acids are reasonable alternatives for gas production. The The reactions performed in experiment 2-1

To learn about balancing chemical equations and law of conservation of mass in chemical reactions

The purpose of this experiment is to distinguish the relationships between reactants and products, in addition to expanding on concepts such as single displacement reactions, mole ratio values, moles to mass, theoretical yields, limiting reactants, excess, stoichiometric relationships and percentage errors.

A chemical equation demonstrates the quantity of atoms of every component that make up the compound. The atomic proportion of components in the compound is the same as the molar proportion of those components. This information can be applied to solve for the mass of one mole of a compound by including the molar masses of the constituent components.

This unti we learned about chemical reactions and this unit we mostly did labs and learned from that. There many ways to be able to get a chemical reactions. There are reaction rates and evidence for a chemical reaction. This unit the quession was what can I observe from a chemical reaction. There are many things you can observe when there is a chemical reaction.

After about an hour of reaction time, the mixture was isolated via vacuum filtration and was then acidified with 6 M HCl during the work up step. The reaction mixture was initially basic because of the sodium bicarbonate added during the beginning of the reaction. This was confirmed by a litmus paper test, with the reaction mixture spot showing up green which correlates to a pH of 8. However, the incorporation of HCl into the reaction mixture greatly acidified the solution. The litmus paper was spotted with the resulting reaction mixture and appeared red, which suggests a pH of about 2.

The aim of this experiment is to use separation techniques to separate a mixture containing polystyrene beads, salt, sand, gravel and iron filings.

In this lab relating to the Law of Conservation of Mass, the mass changed because the gas was released from the chemical reaction. The Law of Conservation of Mass demonstrates that before and after the chemical reaction, the mass of reactants and the mass of products have to be the same.

Stoichiometry has many uses in the real world. In the chemical industry and in professional scientific experiments, scientists use stoichiometry to save money. Scientists use stoichiometric calculations to determine the amount of a substance they need to purchase for a specific reaction. There are four possible reactions that can occur when sodium bicarbonate thermally decomposes. In this lab, stoichiometry was used to find out which balanced chemical equation out the four best represents the thermal decomposition of sodium bicarbonate.