Explain four factors that can change the rate of reactions. How does each factor change the rate?
92261
1.  Heat speeds up a reaction by increasing vibrations and energy of the reactants.\n\n2.  Concentration speeds us a reaction by making more reactants available in a unit volume.\n\n3.  Catylists speed up a reaction (without being used up) by allowing reactants to come into closer proximity.\n\n4.  Increased surface area (by grinding, etc.) speeds up reactions by making more reactants exposed to reaction.
909068
Collision theory predicts that rate of reaction will increase with increasing reactant concentration, because the higher the concentration the greater the number of particles and hence the greater number of collisions. If there are MORE collisions then the number (NOT the proportion) of successful collisions will also increase, therefore rate will increase.\nSo if you're plotting reaction rate vs acid concentration your graph will have a positive gradient and each incremental increase in concentration will have the same effect on the rate of reaction.
732503
U CAN MAKE A PROJ ON REACTIONS ON THE FOLLOWING PTS  .\n INTRO OF REACTIONS\nDEFINITION OF A REACTION\n TYPES OF REACTIONS\n THEN, DESCRIBE THEM SEPARATELY
367815
Try finding the standard reduction potential for Cu and NO first then use those poteintial rxn equ to form the above full reaction afterwhich simply add or substract the poteinital u find to get E for the above reaction. \n\nSince E is proportional to the rate constate, u can use the above concentration as well as partial pressure to calculate the rate constant and hence E. Taking care that rate constant is the concentration/partial pressure of the reactant over the product!
377199
B.  A catalyst speeds up the reaction, as said in the question.  It's mostly just narrowing it down.  Obviously it provides a lower energy pathway if it speeds the reaction up, so it's not C or D.  It's not A, obviously.  Why would you want something that speeds the back reaction from products to reactants up? Well, unless specifically looking for it, I guess.   \nSo, B.
944088
CS2 (g) +4H2 (g) <----> CH4 (g) +2H2S(g) \n\na) pressure of CS2 increase,    -  NO\nb) pressure of CH4 decrease,   - NO\nc) pressure of H2 decrease,     -  YES\nd) pressure of H2S decrease,   -  NO\ne) all the pressures will decrease  -  NO
467240
Given that a certain type of molecule is small enough to permeate through the cell membrane, the most important factor influencing the rate of diffusion is the concentration gradient.  This is simply the difference in concentration levels of the substance between the outside and the inside of the cell.  The larger the difference in concentrations, the greater the rate of diffusion.
66886
GO to wikipedia.com and type in chemical reaction.  That is kind of a tough definition, so I will help to break it down a little for you.  Basically, you got something, and it changes into a whole new a different thing.  That is a chemical reaction.  It could be 2 things coming together to make 1 thing, or vice versa.  Or two things could lead to 2 new things.  The most important part of a chemical reaction is that substances change to NEW substances that have serperate properties and characteristics from the original.\nOn wikipedia there is a link to an IUPAC definition.  IUPAC is pretty much in charge of defining stuff in chemistry, so their definition is the one you're looking for, however, it might be a little complicated.  If this didn't help, maybe you should repost your question.
304629
You can see how enzymes affect the rates of reaction. You can test how varying concentrations of enzyme and substrates affect how fast reactions occur. For example you can study how Peroxidase breaks down Hydrogen Peroxide into water and oxygen. This happens in cells when they metabolize. Hydrogen Peroxide forms as a by-product when this happens, so Peroxidase comes in and breaks the Peroxide down since it is very toxic to the cell.
980488
Hmm. Maybe all you need is the guideline to balance it?\n\nFor beginners, this is probably the best way. After some time, you can omit the unnecessary steps.\n\nFirst, list down the number of atoms of elements present on both sides of equation: reactants vs products. In this case, 1S,4O vs 1S,3O.\n\nSecond, find a common number of atom(s) of an element on either side. Knowing that there is 1S on both sides, the reacting O2 molecule will thus have a stoichiometric coefficient of 1/2. This will ensure 3O on either side.\n\nThird, multiply throughout with 2 since since fractions are not preferred.\n\nOf course, math enthusiasts usually get the hang of this faster by looking for common factor and this method is exceptionally effective (faster) when reactions become complex.\n\nBut the best way is still, of course, to practice XD
975858
1. potential\n2. kinetic\n3. it left at 0\n4. friction\n5. the greater the mass, the less  distance\n\nYour source of errors and improvements must come from your lab
97497
There are temperature changes is most reactions becuase there is heat generated, known as the heat of reaction.
418418
Hopefully this diagram can answer your questions:\nhttp://fachschaft.cup.uni-muenchen.de/~schleifi/reaktion/reaction/stobbe.html
398060
As the previous answerer stated, there is, in general, no relationship between the standard Gibbs free energy change of a reaction, ∆Gº, and the reaction rate.  The reason is that most reactions involve an energy "barrier" between the reactants and products that must be overcome in order for the reaction to proceed.  The higher this barrier, the less likely it is that statistical fluctuations in the energy of the reactant molecules will enable them to surmount the barrier and the slower the rate.  Conversely, a low energy barrier leads to a fast reaction rate.  The free energy change for the overall reaction simply tells you what the difference in energy is between the products and reactants, and not how high an energy barrier separates them.\n\nThese concepts are embodied in a theory of kinetics called "transition state theory", in which a reaction is described by a continuous transition from the unreacted reactants to the fully reacted products.  Every state in this transition process has a free energy associated with it, and a reaction follows a lowest energy path from reactants to products.  The state of the system that has the highest free energy along this path is called the "transition state" (or "activated complex").  This state corresponds to the "energy barrier" described in the previous paragraph.\n\nIf one assumes that there can be a thermodynamic equilibrium between the reactants and the transition state , and that the rate of a chemical reaction is proportional to the concentration of species in the transition state, then one can show that the log of the reaction rate is proportional to Gibbs free energy difference between the transition state and the reactants, ∆G*.  This relationship is given by the Eyring equation:\n\nrate ~ (kT/h) exp (–∆G*/RT)\n\nwhere\n\nk is Boltzmann's constant\nT is the absolute temperature\nh is Plank's constant\nR is the gas constant\n∆G* is the Gibbs free energy difference between the activated complex and the reactants\n\nThus, there *is* a relationship between Gibbs free energy and reaction rates, but the free energy involved is not the free energy change of the overall reaction, but instead, the free energy change associated with going from reactants to the species present at the highest energy point on the reaction path.\n\nSee sources for more details.
209054
Effect of enzyme on reaction
1057769
I'm a teacher and i always give the students the "Rope example"\n\nimagine equilibrium as a rope pulled with the same force both ways! \n\nnow if you look at the your chemical reaction energy (heath) is release from the reaction -----> so if you take the heath out (so you cool the system) the reaction ------> will be more power full so equilibrium will be moved in C and D direction.\n\nIf you heath the system (you'll have a lot of heath that needs to go somehow --- and the only way it can go is by the <--------- reaction -- which is a reaction that use heath ).\n\nThe same with pressure (but you need to have different amounts of molecules -- in your reaction you have the same -- 5 in the reaction ----> and 5 in the reaction <----)\n\nif you speak about concentration use the rope example. You put more of A(increase the concentration of A) , that A need to be consumed in order to keep the equilibrium.\n\nif you take A out of system (so reduce the concentration of A) you'll encourage the <---- reaction (reaction that release more A)\n\nI don't know if you'll understand my spelling and grammar (I'm not the aching chemistry in English). \nI'm just curious what grade are you on? because  I teach this subject to 10th grade students (16 years old )\n\nIf you want me to try to rephrase this answer just let me know \njustplaincornnel@yahoo.com
974075
the larger the size, the greater the surface area, the greater the reaction rate.\n\nsize is the independent variable, the rate of the reaction depends on the size, so rate is the dependent variable