Dynamic Equilibrium and Le Chatelier’s Principle

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

Le Chatelier’s Principle (8 points)

Chemical equilibrium can be determined using different methods. Chemical equilibrium exists when the rate of both sides are equal. Once equilibrium has been reached, the amounts of products and reactants are constant, but if one of the products or reactant concentration can be measured, it can then be used to determine the remaining concentrations and find the equilibrium constant.

To reach equilibrium, hypotonic solutions will move towards hypertonic solutions so that there will be an even concentration of solutes between the two solutions. When a potato cylinder is placed in a solution that is hypotonic (has a lower concentration of solutes than it), water in the hypotonic solution will move toward the more hypertonic potato. However, solutions that have a higher concentration of solutes (hypertonic) than the potato, will force water out of the potato. Therefore, if a potato is placed in a solution of sucrose that is hypotonic compared to the potato it will gain weight. If the potato is placed in a solution of sucrose that has a higher concentration of solutes or is hypertonic to it, then the potato will lose weight. I predict that as the solution become more concentrated with

Equilibrium is when a reaction ratio becomes unbalanced. In the reaction, it does not affect the outcome if the reactants like chromate & hydrogen chloride are not equal to the product water, dichromate, and chloride ion. As long as the reaction maintains the same ratio it won't matter if it's a forward or reverse 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.

According to Le Chatelier's principle, adding additional reactants to a system will shift the equilibrium to the right. Similarly, reducing the concentration of any product will also shift the equilibrium to the right. The opposite is also true,if more products were added or if some reactants were removed ,the equilibrium will be shifted to the left. A example of this is the reaction of carbon monoxide and hydrogen gas to form methanol. If the concentration of carbon monoxide increased, the amount of methanol will

Pablo S. - Pablo’s developing skills in english can cause confusion when discussing and learning thermodynamic principles. The complex vocabulary can confuse Pablo. In order to ensure that Pablo learns from this experiment, I will provide Pablo a procedure and have a meeting with him to discuss any terms or phrases within the procedure that cause some confusion. During this meeting, Pablo will record the discussion points in his lab notebook. This will ensure that when Pablo is completing the lab he will have access to the information from our conversation on the confusing terms associated with the experiment. This information will hopefully aid Pablo during the experiment. If not, Pablo can ask me questions during the experiment.

It is Boyle's Law for which he remains most famous. This states that if the volume of a gas is decreased, the pressure increases proportionally. Understanding that his results could be explained if all gases were made of tiny particles, Boyle tried to construct a universal 'corpuscular theory' of chemistry. He defined the modern idea of an 'element', as well as introducing the litmus test to tell acids from bases, and introduced many other standard chemical

The point of this experiment is to calculate an equilibrium constant for a chemical reaction by watching “Le Chatelier’s Principle” works in this experiment with iron (II) thiocynate. Le Chatelier's Principle is defined as, “A change in one of the variables that describe a system at equilibrium produces a shift in the position of the equilibrium that counteracts the effect of this change” (Purdue Web). Two things can happen within these shifts to relieve stress: The first one is the product concentration increases while the reactant concentration decreases, causing it to shift to the right. The second one is the product concentration decreases while reactant concentration increases, causing it to shift to the left (Purdue Web). In this experiment, iron (II) thiocyanate is the complex ion that is mixed with other solutions. Depending on which solution is mixed together with iron (II) thiocyanate that, will determine the color change trying to reach its equilibrium point. Equilibrium will be observed in the reaction of the iron ion and the thiocyanate ion. When color changes, it represents a “shift” in the chemical reaction. You can determine a shift in the solution by a color change. By observing this reaction at its equilibrium state, FeSCN 2+ can have either a shift to the right or to the left. FeSCN 2+

A common principle I have come across a plethora of times in Science classes, is that everything has a balance. However, that delicate balance can be grossly disrupted by the smallest change.

“When a change is made to an equilibrium system, the system moves to minimise the imposed change and restore the system to equilibrium.”

For the five solutions (Beakers A~E) of CoCl2, 2-propanol, and methanol are approximately at the same temperature 24.5℃, but each beaker contains a different amount of methanol and 2-propanol. As we add more methanol, the dark blue 2-propanol solution becomes a lighter blue because the concentration of octahedral complex also increases upon addition of methanol. While the concentration of the octahedral increases, the concentration of tetrahedral complex decreases until equilibrium is reestablished. According to Le Chatelier’s principle, when an equilibrium system is disturbed, the concentrations of reactants and products shift to establish a new equilibrium position, and equilibrium constant remains the same unless we change the temperature.

The results found from completing this experiment gave insight on how Le Châtelier’s principle reigns true. By viewing the color change of the different substances under temperature changes, and the physical properties change, it showed that predictions of the final equilibrium are accurate. For instance, viewing the clear NH4Cl crystalizing once HCl is added proved that this equilibrium of NH4+ and Cl- reach a state where there is enough aqueous solution and solid moving back and forth between forms and balance out. When viewing it settle into equilibrium, when it was heated in the hot water bath, the cloudy substance hardens on the bottom, with clear liquid floating on top of it. Viewing this in a broader perspective, this can be done for different types of reactions. But, things are subject to change if not only the temperature or concentration changes, but the pressure and volume. These three trials were done by changing concentrations, and then the temperature.

Collision theory is the cause of all reactions between particles (atoms). For a reaction to occur the atoms have to collide with each other. Not just collide, but collide each other in the correct place and the correct orientation for the reaction to occur. These atoms then need to exceed activation energy; there are certain ways to increase all these. One of these ways is to increase the concentration of the solutions being reacted with each other because the higher the concentration, the higher the amount of atoms present therefore