A question about exothermic and endothermic reactions?
Endothermic and Exothermic Reactions:---- Many chemical reactions launch potential contained in this variety of warmth, gentle, or sound. those are exothermic reactions. Exothermic reactions would happen spontaneously and effect in bigger randomness or entropy (?S > 0) of the device. they are denoted by making use of a destructive warmth flow (warmth is lost to our surroundings) and shrink in enthalpy (?H < 0). interior the lab, exothermic reactions produce warmth or is additionally explosive. There are different chemical reactions which could take in potential with the intention to proceed. those are endothermic reactions. Endothermic reactions can not happen spontaneously. artwork could be completed with the intention to get those reactions to happen. whilst endothermic reactions take in potential, a temperature drop is measured throughout the time of the reaction. Endothermic reactions are characterised by making use of useful warmth flow (into the reaction) and an improve in enthalpy (+?H). Examples of Endothermic and Exothermic methods Photosynthesis is an occasion of an endothermic chemical reaction. in this technique, flora use the potential from the sunlight to transform carbon dioxide and water into glucose and oxygen. This reaction demands 15MJ of potential (sunlight) for each kilogram of glucose this is produced: sunlight + 6CO2(g) + H2O(l) = C6H12O6(aq) + 6O2(g) An occasion of an exothermic reaction is the aggregate of sodium and chlorine to yield table salt. This reaction produces 411 kJ of potential for each mole of salt this is produced: Na(s) + 0.5Cl2(s) = NaCl(s) Demonstrations you may carry out Many exothermic and endothermic reactions contain poisonous chemical compounds, extreme warmth or chilly, or messy disposal methods. those demonstrations are secure and uncomplicated: * secure Endothermic reaction * secure Exothermic reaction * warm Ice - Exothermic reaction
In an endothermic reaction on an energy diagram, how do the energies of the reactants and products compare?
In an endothermic reaction on an energy diagram, how do the energies of the reactants and products compare? The reactant's energy is less than the products. The reactant's energy is greater than the products. The reactant's energy is equal to the products. The reactant's energy fluctuates.
How are endothermic and exothermic reactions represented in a diagram?
endothermic reactions means it gains energy and exothermic reactions means it releases energy. so you draw an energy diagram, and you have the energy before the reaction and if it's endothermic then you put the next value about the first
It shows you everything! Is the reaction exothermic? Is it endothermic? Are there a lot of intermediates? Is the activation energy high/low? The list can go on and on!So let's say you have an exothermic reaction. The energy diagram would show you that the reactant starts higher in energy than the product. If you didn't know the reaction is exothermic, you would instantly conclude that yourself based on the energy change as there would energy difference between the reactant and the product. You'd know that the bonds you made are stronger, or maybe that entropy wins in this case, or that you released ring strain energy, and so on. That's significant!Why does this matter though?It helps you understand your reactions. Your reactions are your friends, best friends actually. Our whole life is reactions. Breathing, moving, looking, keeping our hearts beating… everything! You know what happens and what doesn't, what needs energy and what doesn't. That also helps you know what to do and how to do things in lab, where drug synthesis occurs of course. Without the numerous medications and vaccines we have, humans' average age would go back to 40 ish years as it was in the 1700's (or whenever). That, my dear, is very important!Bless you beautiful energy diagrams!!
Chemistry applications on exothermic and endothermic question!?
I don't have any examples for you, but in an exothermic reaction, the product(s) has(/have) less energy than the reactant(s)- energy is released during the reaction... and in an endothermic reaction the reactant(s) has(/have) less energy than the product(s)- energy is gained during the reaction.
Before you can even answer this question,you have to first understand what is the definition of Endothermic and Exothermic reactionsAn Exothermic Reaction will have an Exothermic change, whereby energy (In the form of heat) is release/given out to the surrounding. Delta H (△H) = -ve (Negative) and the (Reactant’s Energy > Product’s Energy)An Endothermic Reaction will have an Endothermic change, whereby energy (In the form of heat) is absorb from the surrounding. Delta H (△H) = +ve (Positive) and the (Product’s Energy > Reactant Energy)Evaporation, is a physical process whereby water in liquid state becomes water vapour (gaseous) . The Following Equation can sum up EvaporationH₂O (l)—→ H₂O (g)As you can see, the water molecule ,in liquid state is held by hydrogen bonds (A type of covalent bond ,Intermolecular force). When it evaporates and become water vapour , the bond will be broken first before it become gaseous state.Think of it this way , imagine yourself breaking a pencil, you will require energy to break one. Just like water to water vapour , energy is Taken in/Absorbed to break the bond before it becomes gas.Since Energy is Absorbed to break the bonds before it can become a gas ,that makes Evaporation an Endothermic Process.Take Note : Evaporation is a Physical Process , The Strong Covalent bonds of the Water, that holds Two Hydrogen and One Oxygen Atom is not broken.Only the hydrogen bond is as This is not Electrolysis (Also Endothermic by the way)Just like Boiling, Where water becomes steam , it is also an endothermic process, together with melting and sublimation.Hope I’ve answered your question , Correct me if I'm wrongGood luck!*This answer was edited on the 30/4/18 , Previous Answer was not as in Depth
Photosynthesis is one of the more unusual endothermic reactions, but it certainly is one. The basic formula for photosynthesis is this:6CO[math]_2+[/math]6H[math]_2[/math]O → C[math]_6[/math]H[math]_{12}[/math]O[math]_6[/math] + 6O[math]_2[/math]During photosynthesis, the plant absorbs energy from sunlight, which helps it produce glucose and oxygen from the initial reactants, carbon dioxide and water. The energy produced remains in the glucose molecules.Here’s an energy diagram depicting this kind of reaction:As you can see, the energy level of the end products (oxygen and glucose) is higher than that of the reactants (carbon dioxide and water), indicating that the reaction ‘took in’ energy instead of giving it off.
Good observation, but the diagram is not meant to be qualitative. I suspect the artist has simply mirror reversed a curve.The activation energy can be very small or very large, as can the difference between the energies of the reactants and products, so the curve can vary enormously. I am not aware of any general rule: it just depends on the particular reaction. (The activation energy can also be affected by catalysts, and is dependent on the intermediate arrangement of molecular species on the way to the new molecular form.)
What's the difference between an endothermic and exothermic reaction?
Exothermic release energy/heat and endothermic absorbs energy/heat. Exo=outside, endo=inside.
Graphs like these are plotted as chemical potential energy over a reaction coordinate.As you see in these examples, as an endothermic reaction progresses, potential energy increases and ends in a higher state. The opposite is true for exothermic reactions, as shown by the graph.