lab234

What are the effects of H2SO4 on the Starch and KIO3’s reaction when we change its proportion?
Abstract:
This lab will manipulate the reaction that occurs between Starch and Potassium iodide by changing the proportion of water to acid. The manipulation’s effects in this report will be shown in discussion II and a bit less precisely in the method section.
Introduction:
In this lab, the effects of an acid on a reaction will be shown. First, the gathering of materials, then the method, the results, the explanation of said results, and finally the general overview of what happened and why in conclusion. The hypothesis of what will happen before this experiment takes place: the acid will increase the reaction time as its concentration increases while water’s proportion lowers. The acid would be considered a catalyst in this scenario.
Materials:
•	Test tube
•	H2SO4
•	Starch
•	KIO3
•	Graduated cylinders
•	Small beaker
•	Timer
•	Safety glasses

Method:
1.	Gather materials
2.	Measure 2 ml of starch and KIO3 in the graduated cylinder
3.	Pour the compounds together in test tube and time the reaction. Record data.
4.	Do the same reaction just add 1 ml H2SO4 and subtract each time and record.
5.	Repeat step 4 three times adding 1 ml of H2SO4 each time.
6.	Clean up area and materials
Quantitative:
#	starch	KIO3	H2SO4	H2O	RXN time[sec]	color
1	2ml	2ml	0ml	4ml	NONE	clear
2	2ml	2ml	1ml	3ml	0.9	orange/slight dark
3	2ml	2ml	2ml	2ml	0.7	light orange/dark yellow
4	2ml	2ml	3ml	1ml	0.6	orange/slight dark
5	2ml	2ml	4ml	0ml	0.5	light orange



Qualitative:
The results of the experiments show that the acid, H2SO4, did in fact increase the reaction time, while water seemed to inhibit less of a reaction. On the first test, the 2ml of starch and KIO3 did not react at all with each other when there was 4 ml of water and no acid. On the second experiment, the reactants did react with the proportion of 1ml of acid to 3ml water, which yielded a reaction time of .9 seconds. From this point on, all reactions react. With a proportion of 2ml acid to 2ml water, the reaction time was .7 seconds. When the proportion of 3ml acid to 1ml water occurred, the reaction time was .6 seconds. On the final try, with 4ml of acid to 0ml of water, the reaction happened in .5 seconds. You can see a trend that as acids amount increases and waters amount decreases, the reaction time speeds up.
Discussion II:
The fruit of this lab shows that the acid did in fact create a faster reaction as you increased its part in the reaction; because of this knowledge, the hypothesis is proven correct. It is noted that because of h2so4 acting as a catalyst, the reaction could happen like it was just between KIO3 and starch. Because the catalyst reduced the amount of energy needed to produce the color change. The color change is an effect of the reaction. When the reaction time was faster and faster every time the acid increased in amount, it is also possible that water can limit the reaction.
Conclusion:
This lab showed a perfect example of catalyst’s effect. The hypothesis was proven and was correct as thought originally.