I'm having a hard time understanding Endothermic and Exothermic reactions, like their standard format and stuff. For Exothermic reactions the heat is getting released into the surroundings, the products will be less than the reactants, so I would assume the products to be like negative, but for Exothermic its:
2H2(g)+O2(g)->2H2O(g)+483.6kJ
^ I don't get why 483>6kJ is positive on the products side, by looking at that I would assume it's endothermic, but its not :|
For endothermic its:
2CO2(g)+566kJ->2CO(g)+O2(g)
^ I thought that this would be exothermic because for exothermic the reactants side is more than the products. And for endothermic the reactants side is less than the products side. I am confused about exothermic and endothermic reactions.
exothermic: heat is given off, so it is on the right side as a +, ie, heat is a product.
for endothermic: heat is absorbed, so it is on the reactant side as a add.
Now later on, it gets confusing, but not now.
Alright but since heat is released wouldn't it be negative? the H notation?
I understand your confusion. Let me explain the concepts of exothermic and endothermic reactions and clarify your doubts.
Exothermic reactions are those where energy is released from the system (reactants) to the surroundings (products). In an exothermic reaction, the products have less energy than the reactants, and the overall energy change is negative (-ΔH). The negative sign denotes the release of energy.
In the reaction: 2H2(g) + O2(g) -> 2H2O(g) + 483.6 kJ, the positive value of 483.6 kJ represents the energy released during the reaction. It doesn't indicate that the products have more energy than the reactants. Instead, it shows the energy released from the reaction, making it exothermic.
On the other hand, endothermic reactions are those where energy is absorbed from the surroundings into the system. In an endothermic reaction, the products have more energy than the reactants, and the overall energy change is positive (+ΔH). The positive sign indicates the absorption of energy.
In the reaction: 2CO2(g) + 566 kJ -> 2CO(g) + O2(g), the positive value of 566 kJ represents the energy absorbed during the reaction. This indicates that the reaction is endothermic since it requires the input of energy for the reaction to occur.
Remember, the signs (+/-) in the reaction equations reflect the energy change, not the actual values or magnitudes of energy. Exothermic reactions release energy, resulting in negative ΔH values, while endothermic reactions absorb energy, leading to positive ΔH values.
I hope this explanation clears up your confusion about exothermic and endothermic reactions. Let me know if you have any further questions!
I understand your confusion. Endothermic and exothermic reactions can be a bit tricky to wrap your head around at first. When analyzing whether a reaction is endothermic or exothermic, it's important to consider the direction in which heat is transferred.
In your first example:
2H2(g) + O2(g) -> 2H2O(g) + 483.6 kJ
The positive value of 483.6 kJ indicates that heat is being released into the surroundings. This means that the reaction is exothermic. The products, in this case, have more energy than the reactants, and the excess energy is being released as heat.
On the other hand, in your second example:
2CO2(g) + 566 kJ -> 2CO(g) + O2(g)
The positive value of 566 kJ indicates that heat is being absorbed from the surroundings. This means that the reaction is endothermic. The reactants, in this case, have less energy than the products, and they absorb energy from the surroundings to compensate for this energy difference.
To summarize:
- Exothermic reactions release heat into the surroundings, so the heat value appears on the product side of the equation as a positive value.
- Endothermic reactions absorb heat from the surroundings, so the heat value appears on the reactant side of the equation as a positive value.
Remember that the signs (+/-) of the heat values alone do not determine whether a reaction is endothermic or exothermic. The direction of heat transfer is the key factor in identifying the nature of the reaction.