Solid CaCO_3 reacts with HCI(aq) according to the equation given below. A studen

Question

Solid CaCO_3 reacts with HCI(aq) according to the equation given below. A student is tasked with determining the reaction's rate, which may be monitor via collection of CO_2 gas in a large syringe. CaCO_3(s) + 2HCI(aq) rightarrow CaCI_2(aq) + H_2O(l) + CO_2(g) a. In a typical experiment, the amount of CO_2 increases rapidly at first and in a linear fashion but then begins to level off after some time. Justify this observation. b. The reaction of CaCO_3 with HCI takes place in an Erlenmeyer flask to which a syringe is affixed with a rubber adapter. Upon addition of the HCI to the solid CaCO_3 care must be taken to very quickly affix the rubber adapter/syringe to the flask. Why is this the case? c. Write a general rate law, i.e., one with reaction orders represented by letters, to describe this heterogeneous reaction. d. Reaction rates are typically temperature dependent. Explain why temperature increases typically lead to reaction rate increases. e. The CaCO_3 is ground to a fine powder. Will the rate of the reaction increase, decrease, or stay the same? Justify your answer. f. Describe an alternative method for monitoring the rate of CaCO_3 decomposition.

Explanation / Answer

a. HCl being strong acid and reactive, the reaction starts immediately and as it proceeds CO2 is rapidly collected, quantity of CO2 starts increases linearly at same rate as CaCO3 decreases. As reactants start depleting CO2 levels off.

b. In order to get accurate quantity measure of CO2 formed, the syringe needs to be affixed quickly as reaction proceeds very fast as soon as HCl is added to CaCO3.

c. K[A]^m [B]^n

d. Increase in temperature increases frequency of collisions between particals thus increasing kinetic energy. The more the collisions more probable they are to have sufficient proper energy and orientation for the particular reaction hence rate of reaction increases.

e. Using Powdered CaCO3 rate of reaction will increase as surface area is more in powdered form.

f. Stoichiometric analysis can be used to determine the rate of this reaction as coefficients of CO2 and CaCO3 are same , rate of appearance of CO2 = rate of decomposition of CaCO3.

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