potential energy , entropy , life , an exergonic reaction or kinetic energy
120652
http://www.science.siu.edu/microbiology/micr201/chapter8N.html\n\nPotential Energy!  Check it out yourself at the link above.
102564
Work equals the vectors of energy.
326918
The activation energy of a reaction is different for every reaction and is totaly independant of wether the reaction is exothermic or endothermic. For any reaction to proceed the minimum energy must be equal to or higher than the activation energy.\n\nNow where your question can come in is, i think, is if the reaction is reversible. In one direction the reaction will be exothermic and in the opposite direction the reaction will be endothermic. For both the forward and backward reactions the activation energy is the same and there is nothing that can be done to change that.
389082
Reactions can be classified as either exothermic or endothermic.  Exothermic reactions release energy, and cause the surroundings to increase in temperature.  Endothermic reactions absorb energy, and cause the temperature of the surroundings to decrease.
643130
Maybe this can help...all you have to do is a search in Yahoo or Google...\n\nhttp://www.think-energy.com/ThinkEnergy/11-14/activities/EnergyTrans.aspx\n\nTry searching for "energy" or "kinetic energy"
3104
Fire is an exothermic reaction that releases energy in the form of heat.  When a hydrocarbon molecule is split is releases energy
425623
You might just use the formula: \nEntropy of the reaction  = \n(sum of the entropy of products) - (sum of the entropy of reactants)\nIt's as simple as that :)\nThanks.
457641
kinetic energy is the energy possessed by a body in virtue of its motion\npotential energy is for example the energy of water \nat the top of a waterfall before it is\nconverted to kinetic energy after it goes\nover the edge of the waterfall\ngravitational energy is the potential \nenergy possessed by a body\nby virtue of its height above sea level \nan example of this is the space shuttle \nusing the frictional resistance of the \natmosphere to convert the gravitational\nand kinetic energy into heat in order to land\n\ni hope that this helps
647716
They are similar, but not exactly the same as exothermic and endothermic as used in chemistry.\n\nExergonic reactions are defined by a negative delta G, that is they have less free energy at the completion of the reaction than at the beginning. An exergonic reaction may require some input of energy (called activation energy) to start the reaction, but will release more energy than is required to start the reaction. \n\nAn endergonic reaction will have a positive delta G, that is it will have more free energy after the reaction than before it starts. \n\nHere is a good website with graphs that explains this:\nhttp://academic.brooklyn.cuny.edu/biology/bio4fv/page/exergon.htm\n\nHere is another website that explains the similarity between exergonic, exothermic, and endergonic, endothermic. \nhttp://www.mansfield.ohio-state.edu/~sabedon/sta5202.htm
383975
Potential energy is stored energy. Once you'll know the potential energy of things, you can make use of this in many applications. It just like knowing your potential to burp many times, you'll show this off to your friends to be cool. Or knowing the potential of your dog to bark and bully someone, you'll bring your dog to your enemies to scare them away!\n\nOn a more serious side, knowing the potential energy of your food (through calories content) will let you know how much energy can you get if you are going to eat them. So, when you are going to have lots of physical activities, you are going to eat these energy giving foods to keep you going.
220374
Every living cell performs continuously thousands of different chemical reactions. Taken nutrients are transformed into a multitude of cell specific components. In this way, sugars, amino acids and their precursors, organic acids, nucleotides, lipids and other substances are produced. The totality of these reactions is summarized as the cell metabolism. In every chemical reaction, a bond is either formed or broken. This process does generally consume energy, consequently, the cell's metabolism and its energy balance to have be regarded as interdependent parameters. Every covalent bond of a molecule contains energy that is set free upon breaking down and that can subsequently be used for other purposes. It could, for example, be used for the formation of a new bond or it could be transformed into another form of energy like movement, warmth, light or electrical energy. Most chemical bonds and nearly all that occur within a cell are stable under physiological conditions. Hence, activation energy is needed for the break-down of a molecule. In chemical laboratories, high temperatures, high pressures or certain inorganic or organic catalysts are normally used. \n\nThe term activation energy refers to the minimum amount of energy required for a chemical reaction to occur. Most reactions require that atoms and molecules crash into each other with a great deal of force. These violent collisions must occur with enough energy to cause the chemical bonds within the molecules to be weakened or broken. When this occurs, the reactant molecules form an activated complex from which the product molecules are formed. Depending on the strength of the bonds within the reactant molecules the activation energy can be quite large, making the activated complex difficult to form.
454524
Entropy -- the second law of thermodynamics.\n\nThis law states that in the absence of other forces, any system becomes less orderly over time.  This is because of the way energy can be converted to different forms but not lost -- most energy that gets used for work transforms into heat, which radiates into space and can't be used to do useful work ever again.  In other words, energy gets used up, and with no more energy input things fall apart into entropy, or complete disorder.\n\nBUT -- the key there is "in the absence of other forces."  We, for example, on earth have our sun which continuously supplies energy to us with which useful work can be done.  As long as there is an external supply of energy, entropy can be avoided.  Once our sun burns out, however, our solar system is indeed doomed to entropy.
244112
Well, if you get something with the second to lowest potential energy in the world, that energy can go to the lowest potential energy thing in the world and that's it.  Otherthan that, no.  And there's nothing inherent in the material, unless you're talking about chemical reactions, in which case, I just don't know what those two things are.  I hope that's clear.
47682
Potential energy is the energy that is available to do work. For example, a ball at the top of a mountain has the POTENTIAL to do energy by rolling down the hill. Entropy is a measure of disorder and randomness. The Universe is in a constant state of randomness. It ties in with potential energy because as the Universe grows more and more random, it spends and utilizes potential energy, reducing the available amount for work.
471131
The answer is d.) often occurs spontaneously.\n\nThis can be proven from the Gibbs Free Energy equation: \nG = H + TS\n\nwhere G is Gibbs energy, H is enthalpy, T is temperature in Kelvins, and S is the entropy or order of randomness. \nG < 0 is spontaneous\nG > 0 is not spontaneous\n\nIf a reaction releases energy, you can also assume that the reaction is exothermic or releases heat so T (and thus T(S)) in Gibbs equation would be negative, making G < 0, or spontaeous in most cases.
189720
friction\nflow \npath\namps\nbut jedi could be correct
488061
Not sure the level with which you are learning, so feel free to ignore the thermodynamics explanation.  If you just want to answer the question, select D.\n\nLike most test questions, there is not enough conditions specified and truly, we could choose several anwers, but only after making assumptions that less likely to be in the testers mind.  I will assume a high school or intro level college course because above that this should be challenged as too vague.\n\nUse logic to realize that answer choice C is not true. Evaluating the others we realize that A means only heat is given off when bonds form and B means heat is absorbed or added during the formation of bonds.  D means conditions exist in which either situation is possible and E means that final product is in a state that has a higher value for entropy.  This only holds true when both Temp and pressure of a system is held constant, but we will eliminate later as well.\n\nBasically a bond can occur when the system goes from a high energy state to a lower energy state.  Formation of bonds is essentially a chemical reaction.  The Gibbs Free Energy equation:\n\n (delta)G=(delta)H-T(delta)S\n\nT=temp of system in Kelvin\n(delta)H is the heat energy change\n(delta)S is the change in entropy (disorder)\n\ndefines whether a reaction will occur spontaneously or not.  (deltaG) must be negative for this to be true. So we will assume \nusing this equation and recognizing that (delta)H tells us exo or endothermic if it is positive or negative , examination of the possibilities of (delta)H and (delta)S,\n\nIf (delta)H is negative and (delta)S is positive the equation will result in a negative value for (delta)G which means a favorible condition exists for bonding to occur.  Therefore, the condition of (delta)H negative (energy leaves as heat - exothermic) is true.  We can thus eliminate answer choice B.\n\nIf the opposite is true and (delta)H is positive and (delta)S is negative, the result is (delta)G that is positive and therefore not spontaneous.  no reaction or bonding occurs.\n\nIf both (delta)H is positive and (delta)S is positive, only a large enough (delta)S will overcome the positive (delta)H in the equation.  So if both are positive and T(delta)S is greater than (delta)H the bonding will occur.  Therefore, when (delta)H is positive (endothermic) the reaction may occur as well.  We can thus eliminate choice A.\n\nWe have shown that C is a true statement because conditions can be met in which the reaction is both exo or endothermic.  However, please note that in both conditions (delta)S is also positive, indicating an increase in entropy.  For the most part any system will always trend toward an insrease in entropy.  \n\nThe question then arises, what happens when (delta)S is negative (decreased entropy) and (delta)H is negative.  For most situations T(delta)S will be large enough to create a positive (delta)G from our equation.  In very rare cases will (delta)H - T(delta)S result in a negative answer.  However, the equation shows this as a possibility when (delta)G= large negative (delta)H - T x small negative (delta)S => large negative # minus a smaller negative => larger negative + smaller # = negative.  (Hope you follow my train of thought).  Therefore in the right situation - (delta) can be negative and bonding/reaction can occur when entropy decreases.  Eliminate E and C is the correct answer.\n\nCareful what you ask for.  Wikipedia site looks pretty informative but very detailed and you have to use a few different pages.