- #1
wayneo
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explain why the reaction lumps of calcium carbonate is much slower with 0.1 M ethanoic acid than with 0.1 M hydrochloric acid at the same temperature.
any ideas?
any ideas?
The purpose of studying rates of reaction is to understand how quickly a chemical reaction occurs and what factors can affect its speed. In this specific experiment, we are investigating the effect of different acids on the rate of reaction with calcium carbonate.
The concentration of acid directly affects the rate of reaction with calcium carbonate. A higher concentration of acid means there are more acid particles in the solution, increasing the chances of collisions with calcium carbonate particles and therefore increasing the rate of reaction.
The surface area of calcium carbonate affects the rate of reaction with 0.1 M acids. A larger surface area means there are more exposed particles, increasing the chances of collisions with acid particles and therefore increasing the rate of reaction.
Temperature plays a significant role in the rate of reaction between calcium carbonate and 0.1 M acids. An increase in temperature leads to an increase in the kinetic energy of particles, resulting in more frequent and energetic collisions between calcium carbonate and acid particles, thus increasing the rate of reaction.
Potential sources of error in this experiment include inaccurate measurement of reactant quantities, variations in the surface area of calcium carbonate, and fluctuations in temperature. Other factors such as impurities in the reactants or human error during the experiment can also contribute to errors in the results.