Question

hi can You please solve [t-BuCl] remaining for my table

the concentration of it remaining

I only used time trial attempt 1

heres my data with the table thats not filled in on the picture:

for % t-BuCl remaining for trials 2-4:

I got 85 % trial 2, 90 % trial 3, and 95% trial 4

for trials 1-4 for time 1st attempt I got

87 seconds trial 1

72 seconds trial 2

35 seconds trial 3

7 seconds trial 4

im confused on how to solve for concentration of t-BuCl remaining

explanation/ answers please

provided are data table and formulas

O* the solution to go from blue to yellow. Record a table similar to the following in your lab notebook and fill in the empty cells. Trial! t-BuCI! NaOHI water! %rxn | 96 t-Buci | [t-Buci] | Time (s) | Time (s) soln Soln (mL) completion remaining remaining 1 attemptnd attempt (mL) (ml) 1 3.000.60 6.40 2 3.00 0.45 6.55 3 3.00 0.30 6.70 4 3.00 0.15 6.85 0.024 20 15 10 80 After completing one set of reactions (Trials 1-4) look at the resulting times observed for each reaction. Consult with your TA to see if a second set of Trials or specific Trials are necessary. Has the color changed in the 2-chlorobutane/water mixture with bromophenol yet? Treatment of Recultc E3 Fullscrees Review The reaction rate for this process can be expressed as either the disappearance of t-BuCl or the appearance of t-BuOH (see equation below). Referring back to the overall net equation, HCl(aq) is also a product. Because of our familiarity with measuring acid strength (pH) in the lab, monitoring the appearance of HCl(aq) during the reaction would be the most convenient method to study kinetic changes during the reaction. rate=--[t- dt dt dt eq. 1 E3 Fullscreen If we focus on the first line of the above equations, we can begin to solve for k, the rate dt eq. 1 If we focus on the first line of the above equations, we can begin to solve for k, the rate constant, with respect to time. During hydrolysis or solvolysis of t-BuCl, the concentration of t- BuCI changes over time according to the following differential equation: dt_ [t-BuCl] =k [t-BuCl] rate eq. 2 During hydrolysis or solvolysis of t-BuCl, the concentration of t-BuCI changes over time In this experiment the rate of appearance of the product HCllaq) is equal to the rate of reaction of t-BuCl. The rate of HCl (aq) production will be observed by adding known amount"r. Fullscreen NaOH(aq) to the starting solution along with a pH indicator, bromophenol blue. While tne The rate constant of the reaction, k, is measured in inverse seconds (s1). The value of k for a given reaction is a function of temperature and solvent. Integrating, we get: kt= In [t-BuCI eq. 3 The value of k for a given reaction is a function of temperature and solvent This equation can be rearranged to the following: In[t-Bucllt--kt+In[t-Bucllo A plot of In[t-BuClt vs t (in seconds) gives a slop of-k where k is the rate constant. This equation is based on the reaction being 1st order in [t-BuCI]. This is true if the rate Fullscreen

Answer 1

trial | t-Bucl | | water | % reaction | % t-Buci | Time (s) (mL)completion remaining Remaining 1 attemps 2 attemps NaOH [t-BuCl] | Time (s) | solnsoln (mL) (mL) 3.00 3.00 3.00 3.00 6.40 6.55 6.70 6.85 0.60 0.45 0.30 0.15 20 15 10 80 85 90 95 0.0240 0.0255 0.0270 0.0285 87 72 35 7 4 The initial concentration of t-BuCI can be calculated as follows 0.024 M 80 % 100 0.03 M t-BuCl remaining is: 0.03 M 100 0.03 M 100 0.03 M 85% t-BuCl remaining-85* 90% t-BuCl r em aining 90% -0.0270 M 95% t-BuCl remaining = 95 * 0 .0285 M