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What is a reactant surface area?
Reactant surface area refers to the total area of a substance available for chemical reactions to occur. It plays a crucial role in determining the rate of a chemical reaction as it affects the frequency of collisions between reactant molecules. Increasing the surface area typically leads to a faster reaction rate as it provides more contact points for particles to interact.
Will increasing the surface area of a reactant decrease the rate of a chemical reaction?
No, increasing the surface area of a reactant will not decrease the rate of a chemical reaction; in fact, it typically increases the reaction rate. A larger surface area allows for more collisions between reactant particles, facilitating more frequent interactions that can lead to a reaction. This is why powdered solids often react faster than larger chunks of the same material.
How is the rate of a reaction affected by reactant surface area?
That there is a bigger area of a solid exposed, so there is a greater chance of collisions causing a reaction.
Why does surface area of a reactant influence the rate of the of the reaction?
by pooing on the leg
How does increasing the surface area of a solid reactant affect the energy of molecular collisions?
Reactions depend on molecular collisions. If a solid reactant is a solid, grinding it into smaller particles will increase the surface area. The more surface area, the faster the molecular collisions, which in turn increases the rate of reaction.
Is this sentence true inceasing the surface area of a reactant exposes more of it to the reaction taking place?
true
Why does surface area of a reactant influence the rate of the reactions?
A chemical reaction is nothing but the conversion of the reactant molecules into product molecules. By increasing the surface area of the reactants more number of reactant molecules are exposed which eventually increases the rate of the reaction...for example, powdered chalk piece dissolves faster in water than a piece of chalk.
Why does surface of a reactant influence the rate of the reaction?
A chemical reaction is nothing but the conversion of the reactant molecules into product molecules. By increasing the surface area of the reactants more number of reactant molecules are exposed which eventually increases the rate of the reaction...for example, powdered chalk piece dissolves faster in water than a piece of chalk.
How does surface area affect the rate of reaction?
The rate of a chemical reaction can be raised by increasing the surface area of a solid reactant. This is done by cutting the substance into small pieces, or by grinding it into a powder. If the surface area of a reactant is increased: More particles are exposed to the other reactant, there are more collisions, the rate of reaction increases.
How does the surface area affect the rate of a reaction?
The powdered solid has a greater surface area than the single lump of solid. So the larger the surface area of the solid, the faster the reaction will be. Increasing the surface area of the solid increases the chances of collision taking place between the molecules of reactants, if it is a reaction in liquid or gaseous phase.
You can speed up a reaction if you break the solid reactant into smaller pieces what factor does this describe?
When you break up a solid into smaller pieces it dissolves faster when you have big pieces of the solid you have to wait for the substance that is dissolving it ti be picked up by the object that is being dissolved but when the pieces are smaller it dissolves faster because their smaller and the substance dissolving the object get picked up much faster
What do concentration surface area and temperature have in common?
Concentration, surface area, and temperature all affect the rate of chemical reactions. Increasing concentration increases the number of reactant particles colliding, larger surface area allows for more contact between reactants, and higher temperature provides more energy for particles to react.
