The most important is the activation energy.
pressure
The likelihood that two particles will collide in a given time increases. The number of particles per volume increases.
The rate of reaction increases with increasing temperature. When the temperature is increased, the kinetic energy of the reacting particles hence the frequency of effective collisions are also increased. Hence the rate of reaction is faster.
Raising the temperature of reactants will speed up a chemical reaction as it make the achievement of the Activation Energy easier. The temperature of individual atoms/molecules in a gas or liquid follow a normal distribution. Raising the temperature forces more atoms/molecules into the 'reaction worthy' side of the distribution.Sneeky energy pumping. Provide some kind of energy that doesn't raise the temperature but does break-down reactant into more reactive radicals. (light, electric discharge) See the photo-electric effectIntroduce enzymes. Chemicals that aren't consumed in the chemical reaction but provide a lower energy way for the reaction to proceed.Poisons react opposite to enzymes by inhibiting a lower energy alternative and forcing a higher energy path for the reaction.Take is easy,,,,,catalyst increase the rate of chemical reaction and inhibitor decrease it...
No, if you increase the concentration of a substance there is a more likely chance of particle collisions occurring. Meaning the higher the concentration the faster the rate of reaction. Imagine people walking around in an empty room, the more people there are in the room, the more likely it is that they will begin to bump into each other, it's the same with particles. The bumping into each other (or collisions) is what will increase the rate of reaction. Conversely if you lower the concentration, there is a lot less chance that the tiny particles will collide with one another meaning the rate of reaction will decrease. Hope this Helps!
pressure
An increase in the temperature usually increases the rate of reaction by increasing the number of collisions.
pressure
pressure
increasing the concentration in the molecue
The likelihood that two particles will collide in a given time increases. The number of particles per volume increases.
Temperature is the measure of the average kinetic energy of the molecules involved. If the temperature increases, then the kinetic energy of the molecules increases and they move faster. Faster moving molecules have more collisions with other molecules and more forcefully. For a reaction to occur, the molecules have to line up correctly and with adequate force. By increasing the speed of the particles, you are increasing the chance that the two molecules will align and produce a reaction.
Increasing the temperature will cause there to be an increase in kinetic energy. This results in an increase in collision frequency, and eventually an increase in rate of reaction as well.
The rate of reaction increases with increasing temperature. When the temperature is increased, the kinetic energy of the reacting particles hence the frequency of effective collisions are also increased. Hence the rate of reaction is faster.
All chemical reactions must be thought of as collisions between the particles of reactants and products. As the temperature of the reaction increases, the energy of the particles also increases and so there is a greater chance of more collisions occuring, and as a result, in general, an increase in reaction temperature increases the reaction rate
Its activity will increase as there is a greater chance that the drug molecules will be of the right conformation. Its selectivity will also increase as there is less chance that the drug molecules will be of the wrong conformation. However, drug molecules with restricted conformation may take a longer time to synthesise as they tend to be more complex in structure.
A common method is to add a catalyst.