reaction rates double every 10 degree change in temperature. under what conditions is this reasonable?
149491
This is a "rule of thumb" that is the average of a lot of kinetic data.  To blindly apply it is unwise, but as a zero order estimate, it should work OK.  Detailed measurements must be done on your system of interest to find out true kinetic parameters and their sensitivity.
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.
97497
There are temperature changes is most reactions becuase there is heat generated, known as the heat of reaction.
708100
Substrate Concentration: If all other conditions are held constant, the rate of the reaction should increase with increasing concentrations of substrate. At very low values of substrate the reaction rate will increase very rapidly. At higher substrate concentrations the rate begins to level off. Eventually the maximum rate for that reaction will be achieved and further increases in substrate concentration will have no effect\n\n\nHope this helps :)
1136926
A simple solution is to mulitply the celsius temperature by 2 and then add 31 (32 - 1). It's not the exact science, but It will give you the right answer 97% of the time.
872856
It will eventually melt at 2572C, and it will boil at 2850C.\n\nHeat does not cause it to react, typically.
675016
This is a calorimetry problem! There is an equation for it:       \nq = mc(change in temperature)\n\nq = the heat required \nm= mass\nc= specific heat \n\nAlso, write out the reaction and products.
177825
theoretically, at any temperature above absolute zero, a reaction can occur.  There are very few reactions that are likely to take place at that temperature, but none that are impossible.
129663
Please do your own home work.\n\nI suspect you are missing a symbol, it probably should be,\nN2O4  <==>  2NO2\n\nThink about how each of the changes will effect the equilibrium of the reaction.
970108
it will speed up the reaction since the heat rises the temperature.\nit will also decompose a compound to its elements--decomposition reaction.
837930
Q10 is a ratio:\n\nHow fast an enzyme works at (T+10) C / How fast the enzyme works at T C\n\nIn other words, by how much does the rate of enzyme action increase when the temperature is raised by 10oC.\n\nMost school texts give it as 2, but it's never been 2 in any experiments my classes have done!
908077
A high temperature will only favour those reactions which are endothermic. To be spontaneous, endothermic reactions require there to be an increase in entropy. You can understand this from the Gibbs Free Energy equation deltaG = deltaH - TdeltaS.  deltaG will tend to become negative as T increases.\nHowever, all reactions proceed faster with an increase in temperature, since a greater proportion of molecules have the minimum energy required to react - the activation energy.\nA low temperature will favour exothermic reactions, and will slow down all reactions.\n\nI do think that the question you are trying to answer is not a particularly good one.
155966
yeah, it means the reaction reaches equilibrium faster
871220
The second one:\nAF + H --> AFM + TM\n\nActivation E: +10KJ/mol is moderate\nHeat of Rx= +5.2 KJ/mol is positive, making this an endothermic reaction (requires the input of heat or energy to accomplish).\n\nSee the site below:
701443
1 - the reaction is reversed and multiplied by 4, so the enthalpy change is 11508 kJ\n\n2 - The reaction is a combination of the other three (I'll label them A, B and C, in the order you have them listed, for simplicity)\nThe original reaction = 2A - 2B -2C (the first one is just doubled, the next two are doubles and reversed), so 2*321.8 - 2*571.7 - 2*288.6 = -2542.2 kJ\n\n3 - This one is done similarly to question 2.  A - 0.5B + 1.5C\n180.8 - 0.5*(-906.2) + 1.5*(-483.6) = -91.5 kJ\n\nHope this helps
747557
A reaction tends to be spontaneous if  it causes an increase in the entropy of the system, and/or a decrease in the enthalpy of the system \n\nBoth reactions are endothermic (increase in enthalpy) becuase of positive delta H values.\nBoth have an increase in entropy (positive delta S value for the first one, production of a gas for the second)\n\nSo I'd say statements ll and lll are true.
341402
Specific heat does not apply to reactions, only actual chemicals.  You are probably thinking of the heat of reaction, or enthalpy.  The change in enthalpy of a reaction (written as delta H, delta as the Greek letter that looks like a little triangle) flips its sign when the reaction is run in the reverse direction.  So a positive delta H value becomes negative when the reaction is run in reverse direction, and a negative delta H value becomes positive.