Hey, thanks for coming :-)
So I'm getting confused about this.. if I have substances A + B --> C + 180 kJ is the forward reaction exothermic or endothermic?
If I have substances A + B --> C -180 kJ is the forward reaction exothermic or endothermic?
THANKS I REALLY APPRECIATE IT :-)
Kelly :-)
So I'm getting confused about this.. if I have substances A + B --> C + 180 kJ is the forward reaction exothermic or endothermic?
If I have substances A + B --> C -180 kJ is the forward reaction exothermic or endothermic?
THANKS I REALLY APPRECIATE IT :-)
Kelly :-)
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A + B ->C + 180kJ This one is exothermic. The + indicates that energy has been given out the the surrounding area (commonly in the form of heat).
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There are two common ways to indicate if a reaction is exo or endothermic.
Method 1 is to put the energy term in the chemical equation as in your first example. When the heat term is on the product side then heat is "produced" = exothermic. If you wanted to show the reaction was endothermic you would put the heat term on the reactant side as in A + B + 180 kJ = C
The second method is to indicate the "change in heat", known as delta H (the "delta" is actually a triangle), somewhere off to the side. I THINK that is what you are trying to show in your second example but it isn't exactly clear. You would write the reaction: A + B = C and then you would put, off to one side,
"delta"H = - 180 KJ. If you wanted to show the reaction was endothermic the "delta" H would be a +180 KJ
You don't normally see an equation with the heat term written as a negative as in your second example.,
Method 1 is to put the energy term in the chemical equation as in your first example. When the heat term is on the product side then heat is "produced" = exothermic. If you wanted to show the reaction was endothermic you would put the heat term on the reactant side as in A + B + 180 kJ = C
The second method is to indicate the "change in heat", known as delta H (the "delta" is actually a triangle), somewhere off to the side. I THINK that is what you are trying to show in your second example but it isn't exactly clear. You would write the reaction: A + B = C and then you would put, off to one side,
"delta"H = - 180 KJ. If you wanted to show the reaction was endothermic the "delta" H would be a +180 KJ
You don't normally see an equation with the heat term written as a negative as in your second example.,
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When its positive, it means energy has been added to the reaction, aka u used some energy, so its endothermic.
When its negative, u released energy and its exothermic.
Right?
When its negative, u released energy and its exothermic.
Right?
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Exothermic means there is a release of energy in the equation.
Endothermic means there is a consumption of energy in the equation, meaning the area around it gets cold when the reaction occurs.
Endothermic means there is a consumption of energy in the equation, meaning the area around it gets cold when the reaction occurs.
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Endo is IN
Exo is OUT
When you squish a sponge and put it in the water, it sucks up water. Thats Endo
When you take it out and squish it and all the water blasts out, thats exo.
Exo is OUT
When you squish a sponge and put it in the water, it sucks up water. Thats Endo
When you take it out and squish it and all the water blasts out, thats exo.
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Endothermic reactions consume energy. Exothermic reactions emit energy.
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Sorry, I needed 2 points.