Grossmont-Cuyamaca Community College District Lab Report

For K-323 here are the 2 parts needed. Notice that you do not need to submit purpose, procedures or data and observations or conclusions!1. Title page (just your name and the expt number – will help me identify what I am looking at when I download the submissions and view them).2. Answers to analysis Q – with the following modifications. You can write answers to Q by hand or in MS-Word or some combination of those. Please rewrite the Q before answering.For Q 1 and Q 2 show all working so I can see what data numbers you are using.For Q3 a) and Q 3b):For each temperature calculate 1/T and ln(rate). Show these calculated values in a table. Create a plot of ln(rate) vs 1/T. This should be an x-y scatter plot with ln(rate) on the y-axis and 1/T on the x-axis. Remember to have a title, and axis labels on the graph. Use landscape format for any kind of printing that you do with this graph.Add a best fit straight line and make sure the equation of the line is shown on the graph.You can make this graph in MS-Excel, or Logger pro or other graphing software you may have. Remember you can download Logger pro from Canvas – you will find it in the modules section under Expt S-201 with instructions on how to install it.For Q3c) Use the slope of the line from the graph to calculate the activation energy in kilojoules per mol (kJ/mol).

Data

1 room temperature

T i = 21.0 c

Ti = 2:30 min to sec?

Tf = 2:40 min to sec?

Mean?

2) in high temperature

Ti = 40.0 c Tf =28.0 c

ti =2:10 min to sec?

Tf= 2:16 min to sec¿

Mean?

3) In low temperature

Ti= 5.30 c Tf= 10.6 c

Ti= 3:40 min to sec?

Tf= 3:51 min to sec?

Mean?

X10′
Ans
EXPERIMENT K-32
Experimental Procedure
1 Max a 400 mL leaker containing 200 mL of water on a hot plate at a setting of LO. Cover the beaker with a
watch glass to minimize evaporation. The hot water will be used later in the experiment for the high tempera-
ture run.
2 Room Temperature Run:
a NaHSO, and KIO, solutions will be available. Take 25 mL (no more) of each in small beakers. Record the
information on the labels of these solutions. Piper 5.0 mL of NaHSO, solution into a small test tube. Pipet
5.0 mL of KIO, solution into another small test tube.
b Place the rest tubes in a large styrofoam cup filled about 2-3 inches high with room temperature water. The
water level in the cup should be higher than the solutions in the test tubes. Place a digital thermometer in
the cup. Cover the cup with clear plastic wrap to minimize temperature
drift. Wait 5 minutes (or longer if necessary) in order to allow everything
in the cup to reach the same temperature. Record the temperature.
c After temperature equilibrium has been achieved, pour the contents of one
test tube into the other. Stopper the test tube and invert it several times to
mix the solutions. Return the rest tube to the cup. Record the time (to the
nearest second) at which you first mixed the reactants.
d The reaction mixture should be colorless initially. Wait for the blue color
of the iodine starch complex to appear. (See Figure 1). Record the time of
appearance of the blue color to the nearest second.
Figure 1
3 High Temperature Run:
Repeat the procedure for the room temperature run except that the styrofoam cup should contain water in
the range of 30-35°C after the test tubes have been placed in the cup. Add hot or room temperature water, as
necessary to adjust the temperature to this range. After temperature equilibrium has been reached, record the
temperature and proceed as in the room temperature run.
4 Low Temperature Run:
Repeat the procedure for the room temperature run except that the styrofoam cup should contain water in
the range of 5-10°C after the test tubes have been placed in the cup. Add ice or room temperature water, as
necessary, to adjust the temperature to this range. After temperature equilibrium has been reached, record the
temperature and proceed as in the room temperature run.
4 Chemistry 142: General Chemistry Il Laboratory Manual
Cuyamaca College
nach
1.0.3 m
H3
Initired ohne
33.81 ml
Titration
foromt
M
20.85 L
33.81 L
Titration
6.91
20.85
Titation
3
Post-Lab
Questions
Experiment K-323
Temperature Dependence of Rate
of lodine Clock Reaction
(To be answered in the “Analysis” section of your lab report)
1 Calculate the initial molarity of HSO; – in the reaction mixture.
2 Calculate the rate of disappearance of HSO; – in mol/L sec at
a) the low temperature
b) room temperature
c) the high temperature
3 a) For each temperature calculate 1/T and In(rate). Show all work and carry three decimal places in the
logarithm. Determine the best straight line through the points in the computer-generated graph.
b) Determine the slope of the line. (Use two points on the line that are far apart. Determine the coordinates
of each point and write their values on the graph.]
c) Calculate the activation energy in Joules.
EXPERIMENT K-323
Temperature Dependence of Rate of lodine Clock Reaction
rach
1.0.3 m
NH3
Iriiled ohne
33.81 ml
The train
soromt
20.85 L
33.81
Titration
6.91
20.85
Titeltion
3
Post-Lab
Questions
Experiment K-323
Temperature Dependence of Rate
of lodine Clock Reaction
(To be answered in the “Analysis” section of your lab report)
1 Calculate the initial molarity of HSO; – in the reaction mixture.
2 Calculate the rate of disappearance of HSO; – in mol/L-sec at
a) the low temperature
b) room temperature
c) the high temperature
3 a) For each temperature calculate 1/T and In(rate). Show all work and carry three decimal places in the
logarithm. Determine the best straight line through the points in the computer-generated graph.
b) Determine the slope of the line. (Use two points on the line that are far apart. Determine the coordinates
of each point and write their values on the graph.)
c) Calculate the activation energy in Joules.
EXPERIMENT K-323
Temperature Dependence of Rate of lodine Clock Reaction