Can anybody explain to me how to determine the endormicity and exormicity in a reaction and where does the equilibrium shift. Pls. give an example of it. Iwas reading my book and trying to understand but i really can't comprehend it. Now I'm stuck here i can't answer my post lab experiment. Pls anybody thanks. Just a simple explanation please.
It ALWAYS helps if you give us an example and let us show you how to do it. Our examples may not fit your needs.
A + B ==> C delta H = -235 kJ.
This reaction has a - delta H; that means it is EXOTHERMIC. I prefer to rewrite the equation this way.
A + B ==> C + heat.
Le Chatelier's Principle, in very simple language, tells us that a system in equilibrium will try to undo what we do to it. Suppose then that we add heat to the reaction. It will try to undo that meaning it will try to get rid of the extra heat we've added. How can it do that? (There are only three choices; i.e., shift to the right, shift to the left, neither). To get rid of the heat C reacts to produce A + B BECAUSE that uses the heat we have added (meaning that the reaction shifts to the left). Or if we lower the temperature, the
reaction tries to undo that by producing heat. How can it produce it. Of course by A + B ==> C gives us heat.
For endothermic reaction delta H is +. If we have
X + Y = Z and delta H = +285 kJ, I prefer to rewrite it as
X + Y + heat = Z.
In our experiment they gave us this eguilibrium to investigate:
H2CO3(aq)=H2O(l)+CO2(g)
We put soda in a syringe when we push the plunger (increase pressure) there was less bubbles formed but when we pulled the plunger (decrease the pressure) the was more bubbles formed. With this observation and on the equation how will i be able to determine or where will i be able to base the thermicity endothermic or exothermic of equation. Pls. DrBob222 need an answer, thanks.
Sure, I can help explain the concepts of endothermicity and exothermicity in a reaction, as well as how to determine which direction the equilibrium shifts.
Firstly, let's understand what endothermicity and exothermicity mean in the context of a reaction.
- Endothermic reaction: This type of reaction absorbs heat energy from the surroundings, resulting in a decrease in temperature. In other words, energy is being taken in or gained by the system. The reactants have a lower energy level than the products, so the energy is absorbed to reach a higher energy state.
- Exothermic reaction: This type of reaction releases heat energy into the surroundings, causing an increase in temperature. In other words, energy is being given off or lost by the system. The reactants have a higher energy level than the products, so the energy is released to reach a lower energy state.
To determine whether a reaction is endothermic or exothermic, you can look at the overall temperature change that occurs during the reaction. If the temperature decreases, it is endothermic. If the temperature increases, it is exothermic.
Now, let's discuss how to determine the direction in which the equilibrium of a reaction shifts.
Equilibrium is a state in a chemical reaction where the concentrations of reactants and products remain constant over time. The equilibrium position can be shifted by changing the conditions of the reaction, such as temperature, pressure, or concentration.
- Le Chatelier's principle is commonly used to predict the direction of shift in equilibrium. It states that if a system at equilibrium is subjected to a change, the system will adjust to counteract that change and restore equilibrium.
For example, let's consider the reaction:
A + B ⇌ C + D
If more A and B are added to the system, the equilibrium will shift to the right to consume the additional A and B and produce more C and D.
If more C and D are added, the equilibrium will shift to the left to consume the additional C and D and produce more A and B.
Similarly, changes in temperature and pressure can also affect the equilibrium position. If the temperature is increased in an endothermic reaction, the equilibrium will shift towards the products to absorb the excess heat. If the temperature is increased in an exothermic reaction, the equilibrium will shift towards the reactants to compensate for the excess heat.
It is important to note that equilibrium shifts do not necessarily change the concentrations of reactants and products, but rather, their relative proportions.
I hope this explanation helps you in understanding endothermicity, exothermicity, and the shift of equilibrium in a reaction.