Data Table 1. Varying Concentrations of 1.0 M HCl. Concentrations # of drops # o
ID: 890980 • Letter: D
Question
Data Table 1. Varying Concentrations of 1.0 M HCl.
Concentrations
# of drops
# of drops
# of drops
Stock Solution
Stock Solution
Reaction (after mixing in well)
Reaction (after mixing in well)
Reaction Time
(seconds)
Reaction
Rate
(sec-1)
Well #
HCl
H2O
Na2S2O3
HCl
Na2S2O3
HCl
Na2S2O3
Trial 1
Trial 2
Average
C1, D1
12
0
8
1M
0.3M
34.58
34.55
34.57
C2, D2
6
6
8
1M
0.3M
43.37
47.25
45.31
C3, D3
4
8
8
1M
0.3M
54.59
53.65
54.12
Data Table 2. Varying Concentrations of 0.3 M Na2S2O3.
Concentrations
# of drops
# of drops
# of drops
Stock Solution
Stock Solution
Reaction (after mixing in well)
Reaction (after mixing in well)
Reaction Time
(seconds)
Reaction
Rate
(sec-1)
Well #
HCl
H2O
Na2S2O3
HCl
Na2S2O3
HCl
Na2S2O3
Trial 1
Trial 2
Average
C4, D4
8
0
12
1M
0.3M
26.66
27.69
27.18
C5, D5
8
6
6
1M
0.3M
65.04
59.89
62.47
C6, D6
8
8
4
1M
0.3M
115.59
122.38
118.99
Questions
Determine the Reaction Order for HCl using calculations described in the Background section. Show your work. Note that your answer will probably not be an even whole number as it is in the examples, so round to the nearest whole number.
Determine the Reaction Order for Na2S2O3 using calculations described in the Background section. Show your work. Note that your answer will probably not be an even whole number as it is in the examples.
Write the rate law for the reaction between HCl and Na2S2O3.
Using the following rate law, and the experimental values given, calculate k:
Experiment
[F2] (M)
[ClO2] (M)
Initial rate (M/s)
1
0.5
0.5
0.3 M/s
2
0.8
0.8
0.768 M/s
3
0.5
0.8
0.48 M/s
Concentrations
# of drops
# of drops
# of drops
Stock Solution
Stock Solution
Reaction (after mixing in well)
Reaction (after mixing in well)
Reaction Time
(seconds)
Reaction
Rate
(sec-1)
Well #
HCl
H2O
Na2S2O3
HCl
Na2S2O3
HCl
Na2S2O3
Trial 1
Trial 2
Average
C1, D1
12
0
8
1M
0.3M
34.58
34.55
34.57
C2, D2
6
6
8
1M
0.3M
43.37
47.25
45.31
C3, D3
4
8
8
1M
0.3M
54.59
53.65
54.12
Explanation / Answer
problem number 2 ) :
rate= k [F2]x [ClO2]y
we need to find out x and y
from data
0.5 =k [0.5]x [0.5]y ------------->(1)
0.768 =k [0.8]x [0.8]y ------------->(2)
0.48 =k [0.5]x [0.8]y ------------->(3)
by solving (2) and (3)
x = 1
by solving 1 and 2
y = 0
rate law = k [F2]0[ClO2]1
from (1) data
0.5 =k [0.5]x [0.5]y ------------->(1)
substitute x , y value
0.5 = k (0.5)^0 (0.5)^1
k = 1 sec-1
note : the above problem is very lengthy problem. first we need to solve concentration all trails . and at respective trails we need to calculate rate . from that we need to draw another table then we can find out order.
i am doing final step for problem 2. it is also another lengthy problem
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