A student measures out 1.50 mL of pure t-butyl chloride and dilutes it with the

Question

A student measures out 1.50 mL of pure t-butyl chloride and dilutes it with the solvent mixture to 100 mL in a volumetric flask. What is the molarity of the (CH3)3CCI? Alter 10.0 minutes, the student takes a 10.0 mL aliquot of the reaction mixture and quenches the reaction with isopropyl alcohol. Titration of the resulting solution with 0.0500 M NaOH to the phenolphthalein end point required 5.40 mL. How many moles of HCl were produced? What was the ((CH3)3CCl] after 10.0 minutes? Assuming this is a zero order reaction, what would you predict the concentration to be after 20.0 minutes? Assuming first order, the expected concentration should be what? Assuming second order, the expected concentration should be what?

Explanation / Answer

density of pure t butyl chloride = 0.840g/cc

wt of pure t butyl chloride =92.57 g/mol

molarity of pure t butyl chloride = 840/92.57=9.07 M

now

M1V1=M2V2

9.07*1.5 = M2*100

M2 = 0.136 M

Related Questions

Navigate

• Browse (All)
• Browse A
• Subjects

---

---

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.