If u use 4 g of calcium carbonate in excess acid,instead of 2 g.They find that the rate of the reaction increases.why the rate increases?
If the calcium carbonate is in powder form, the surface area available for reaction is larger, thus a higher probability of reaction contact.
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To understand why the rate of the reaction increases when using 4 g of calcium carbonate instead of 2 g in excess acid, we need to consider the concept of reactant concentration and its effect on reaction rate.
In a chemical reaction, the rate is determined by the rate at which reactant particles collide with each other. Increasing the concentration of a reactant increases the likelihood of successful collisions, leading to an increase in the reaction rate.
In this case, by doubling the amount of calcium carbonate from 2 g to 4 g, we are effectively doubling the concentration of the reactant in the reaction mixture. As a result, there will be more calcium carbonate particles available for collisions with the acid particles. The increased concentration of calcium carbonate increases the chances of collisions and, consequently, the reaction rate.
It's important to note that the increase in reaction rate may not be proportionate to the increase in reactant concentration. The reaction rate may eventually plateau, as the acid will eventually become the limiting reactant, meaning there is an excess of calcium carbonate that cannot react any further.