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of HCL Which solution reacted fastest CONCENTRATION You reacted zine with three

ID: 1041228 • Letter: O

Question

of HCL Which solution reacted fastest CONCENTRATION You reacted zine with three different concentrations expected? Clearly explain why or why not. which reacted slowest (List the order of concentrations in order of fastest to slowest). Wst ane TEMPERATURE You reacted zinc with 2 M HCI at three different temperatures. What order did the solutions react (list in order: fastest first, slowest last). Was this the expected order based upon what you know of the effects of temperature on the rate of a reaction? Clearly explain why (or why not) this was expected SURFACE AREA You compared the reaction of mossy zinc with zinc granules. Which reacted fastest? Which had the greatest surface area? Did these two types (particle sizes) of zinc react in the order you would have predicted prior to the experiment? Explain why the granules may have reacted slower? Did you notice any change in the apparent rate of reaction once the metal in both tubes had begun reacting? If so, why was this expected? Factors that Inflgen

Explanation / Answer

A product is formed when the reactant molecules undergo effective collision.

(1).zinc reacts very slowly with dil:HCl and fastly with conc:Hcl.That is, rate of reaction increases with increase in conc: of acids. However in some cases, increase in concentration of one of the species may be reverse that of expected. As the concentration increases, no of molecules per unit volume increases, and hence the chance of colliding HCl molecules with Zn increases. Hence rate of reaction increases with increasing concentration.

(2): the rate of reaction increases with increase in temperature. As temperature increases, molecules will attain more kinetic energy, so that more fastly the molecules will move and more often the molecules collide. Most of this collision will be effective and product will form.

(3) Rate of reaction increases with increase in surface area of solid reactants. As surface are increases ,more particles are exposed to other reactants. Chances for effective collision increases. And hence rate increases.

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