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5.2 lab notes and coursework
Fundamentals of Chemistry Lab (CHM101L)
Southern New Hampshire University
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CHEM labPreview text
Factors Affecting Reaction Rates
Jacen Duplain
06/02/
Data
Activity 1
Data Table 1: Calibration
Trial Na 2 S 2 O 3 (drops) Reaction time (sec) 1 8 19. 2 8 18. 3 8 19.
Question 1: How many drops will be used in the remaining experiments?
I will be using 8 drops of Na2S2O
Activity 2
Data Table 2a. Effects of KI (I-) Concentration
Trial (drops)KI (drops)HCl (drops)Starch (drops)H 2 O Na(drops) 2 S 2 O 3 H(mL) 2 O 2 Time(sec) 1 Time(sec) 2
Average time (Tavg) ( )
Average Rate (1/Tavg)
1 8 2 4 0 8 0 20 (20 + 20)/ = 20.
1M/19.
s 2 8 2 4 0 8 0 20 = 0/s
3 6 2 4 2 8 0 26 (26 + 25)/ = 26.
1M/26.
s 4 6 2 4 2 8 0 25 = 0/s
5 4 2 4 4 8 0 33 (33 + 34)/ = 34.
1M/34.
s 6 4 2 4 4 8 0 34 = 0/s
7 2 2 4 6 8 0 80 (80 + 78)/ = 79.
1M/79.
s 8 2 2 4 6 8 0 78 = 0/s
Data Table 2b. Effects of H 2 O 2 Concentration
Data Table 3. Temperature Effects
Water bath trial
Temperature of the water bath (°C) Reaction time (sec) Cold water 4°C 52.
Room-temperature water 23°C 18.
Hot water 48°C 5.
Question 2: Explain how each of these treatments affected the reaction rate. Describe the effect at a molecular level.
a. Concentration An increase of concentration of the reactant results in a higher frequency of molecular collision which increases the rate of reaction.
b. Temperature
Increasing temperature causes molecules to collide more frequent with greater force in turn increasing the rate of reaction.
Activity 4
Data Table 4. Catalyst
Trial Water (drops) CuSO 4 (drops) Reaction time (sec) 1 4 0 19. 2 3 1 2. 3 2 2 2. 4 1 3 1. 5 0 4 1.
Question 3: How did the addition of copper(II) sulfate affect the reaction rate? Did the amount of catalyst affect the reaction rate?
Copper(II) sulfate increase the reaction time, the presence of CuSO4 provides an alternate where the reaction can take place with lower activation energy resulting in a more speedy reaction.
Activity 5:
Data Table 5. Orders of Reactants in the Rate Law
Determine the actual Rate Law: R = k[I–]m[H 2 O 2 ]n[H+]p
Calculated Reaction order (X) (e. (
concentration 1
concentration 2 )
X = rate 1 rate 2 )
You must show your full calculation work for credit.
Reactant Concentration
Average Rate (1/Tavg)
Calculated Reaction order (X) Show work!
Average Reaction order
Reaction Order (integer)
KI (I) 8 drops 0.
1 m = 1
(8/6)^x = 0/0. x = 0. KI (I) 6 drops 0. 6/4^x = 0/0. x = 1. KI (I) 4 drops 0. 4/2^x = 0/0. x = 1. KI (I) 2 drops 0.
H 2 O 2 0 mL 0.
0 n = 1
0.4/0^x = 0/0. x = -0. H 2 O 2 0 mL 0. 0.3/0^x = 0/0. x = 2. H 2 O 2 0 mL 0. 0.2/0^x = 0/0. x = 0. H 2 O 2 0 mL 0.
HCl (H+) 100% 0.
0 p = 1
1/0^x = 0/0. x = 0. HCl (H+) 75% 0. 0.75/0^x = 0/0. HCl (H+) 50% 0 x = 0. 0.50/0^x = 0/0. HCl (H+) 25% 0 x = 0.
5.2 lab notes and coursework
Course: Fundamentals of Chemistry Lab (CHM101L)
University: Southern New Hampshire University
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