Also, calculate the % water/acetone? Due before lab begins. Answer in space prov
ID: 1035566 • Letter: A
Question
Also, calculate the % water/acetone? Due before lab begins. Answer in space provided 1. Consider the following data: 3.00 mL of 0.100 M t-BuCl are mixed with 3.00 mL of 0.01 M NaOH and 3.00 mL of distilled water. a. Calculate the initial molarity of t-BuCI. b. How many moles of t-BuCI will have reacted when bromophenol blue changes color? c. What is the [t-BuCl], in M, when bromophenol blue changes color? d. What will the kinetic equation (x kt) be for this data? (Substitute appropriate values into Eq. 2.) If 650 sec were required for bromophenol blue color to change, then calculate K. e.Explanation / Answer
Ans.a) One mole of t-butyl chloride will produce one mole of HCl.
3mL of 0.1 M of t-BuCl = 0.3 mMol and will produce 0.3 mMol of HCl.
3mL of 0.01 M of NaOH = 0.03 mMol
HCl + NaOH ? NaCl + H2O
hence mMol of t-BuCl remaining = 0.3-0.03 = 0.27
Intial molarity of t-BuCl will be 0.27/3 = 0.09 M
b) Bromophenol blue changes from blue to yellow when the HCl produced in the reaction and will neutralize the known amount of NaOH that was added to the reaction mixture. now 0.03 mMol of NaOH only neutralize by 0.03 mMol of HCl produced in the reaction mixture. And hence 0.03 mMol of t-BuCl required to change the colour.
c.) 0.09 M
d.) The rate at which a reactant is consumed as a function of time.
The reaction of t-butyl chloride with water to give two products are t-butyl alcohol (2-methyl-2-propanol) and hydrochloric acid.
Because step 2 is fast, it is step 1, the slow step, which determines the rate of reaction. Step 1 is dependent only on the concentration of the t-butyl chloride and is, therefore, a unimolecular reaction, a first-order reaction. For a first-order reaction, the rate = k [t-butyl chloride].
e.) t1/2=ln2/k?0.693/k
or K = 0.693/650 = 0.001066 s1-
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