Graded Assignment: Chemistry

The objective of the experiment is to apply Le Chatelier's Principle, which is a system that responds to an external stress and then adjusts itself in order to alleviate the stress when it is at equilibrium. A reactant is added, and the equilibrium is reestablished, resulting in more products and fewer reactants, and thus, the position of equilibrium is shifted to the right. When a product is added, the equilibrium position is shifted to the left because there are more reactants and fewer products.

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).

I believe the type of reaction to have occurred to be a condensation reaction as H2O has been produced as a by-product.

Write a balanced chemical equation for the reaction of carbon dioxide with limewater. The formula for the active substance in limewater is on the pipet, and the products of the reaction are calcium carbonate and water.

Is this reaction endothermic or exothermic? What does that mean and how do you know? (~3 sentences)

Purpose: The purpose of this experiment is to observe a variety of chemical reactions and to identify patterns in the conversion of reactants into products.

Upon heating, CaCO3 decomposes to CaO and CO2. What change in the hybridization of carbon occurs in this reaction?

This cooling reaction occurs instantaneously but lasts for about an hour. How does this reaction sustain itself for twenty minutes? This question will be answered later in this explanation.

This reaction is exothermic, as heat is given out. This is because the amount reactant energy is more than the product energy the difference between this is ΔH, therefore some energy has been given out in the form of

Background Information: We are going to use our knowledge of the Le Chatelier’s principle in order to observe this experiment. The principle states that the equilibrium will shift in the direction that will minimize the effects of the change.

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?

As told at the beginning of this lab report, our aim of this experiment was to test the validity of Hess’s law which suggests that the enthalpy change of a reaction must be equal to the sum of the enthalpy changes of the other reactions that relate to the original reaction. Our result achieved from this experiment is the simple proof of Hess’s Law’s validity.

What started out as an April Fools’ Joke of a topic turned into a serious chemistry examination all thanks to a video from Scientific American. This video and article discusses a group of beetles called Bombardier Beetles. This insect has a very interesting and has a unique defense mechanism that gives the group it’s common name. They spray a very hot toxic liquid to discourage predators. Interestingly, the bug doesn’t use muscular contractions to discharge the deterrent, it uses an explosion inside its body. (Augenbraun,2016). There are three concepts that can be addressed regarding this explosive reaction that we have covered in our class: chemical reactions, catalysts, and gas laws.

In terms of Le Chatelier’s Principle, there are changes in concentration, temperature, volume and pressure that can occur to

“These processes react in a state of equilibrium where the rates of the forward and reverse reactions are equal so that the reactants and products are created at the same rate.”