Temperature: Raising temperature generally speeds up a reaction, and lowering temperature slows down a reaction. However, extreme high temperatures can cause an enzyme to lose its shape (denature) and stop working. pH: Each enzyme has an optimum pH range. Changing the pH outside of this range will slow enzyme activity.
Q. How does temperature increase reaction rate?
An increase in temperature typically increases the rate of reaction. An increase in temperature will raise the average kinetic energy of the reactant molecules. Therefore, a greater proportion of molecules will have the minimum energy necessary for an effective collision (Figure.
Table of Contents
- Q. How does temperature increase reaction rate?
- Q. Why are some reaction very fast?
- Q. What are the drawbacks of very fast reactions?
- Q. What happens when a reaction stops?
- Q. What does it mean when a reaction is product favored?
- Q. How do you tell if the forward or reverse reaction is faster?
- Q. Why are exothermic reactions favored at low temperatures?
- Q. What happens if you increase the temperature of an exothermic reaction?
Q. Why are some reaction very fast?
Reactions in phases that easily mix, such as gases and liquids, occur much faster than reactions between solids. The extent of mixing of the reactants influences the frequency of molecular collisions – if reactants are more thoroughly mixed, the molecules will collide more often and thus react faster.
Q. What are the drawbacks of very fast reactions?
There are two difficulties with fast reactions. One is that the time that it takes to mix reactants or to change the temperature of the system may be significant in comparison with the half-life, so that the initial time cannot be measured accurately.
Q. What happens when a reaction stops?
If a chemical reaction happens in a container where none of the reactants or products can escape, you have a closed system. Reversible reactions that happen in a closed system eventually reach equilibrium. At equilibrium, the concentrations of reactants and products do not change.
Q. What does it mean when a reaction is product favored?
spontaneous reactions
Q. How do you tell if the forward or reverse reaction is faster?
If the concentrations of the reactants are too large for the reaction to be at equilibrium, the rate of the forward reaction will be faster than the reverse reaction, and some of the reactants will be converted into products until equilibrium is achieved.
Q. Why are exothermic reactions favored at low temperatures?
So, if the reaction is exothermic. This means it produces heat. So, if we decrease the temperature (low temperatures), the equilibrium will tend to counteract this effect and favor the reaction that produces heat to increase the temperaure of the system.
Q. What happens if you increase the temperature of an exothermic reaction?
Therefore if the reaction is exothermic as written, an increase in temperature will cause the reverse reaction to occur, decreasing the amounts of the products and increasing the amounts of reactants. Lowering the temperature will produce the opposite response.
