Data Table 1. Varying Concentrations of 1.0 M HCl. Concentrations # of drops # o
ID: 878030 • 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
27.44
27.40
27.42
C2, D2
6
6
8
1M
0.3M
31.66
31.68
31.67
C3, D3
4
8
8
1M
0.3M
46.90
46.98
46.94
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
19.96
19.64
19.8
C5, D5
8
6
6
1M
0.3M
48.69
48.63
48.66
C6, D6
8
8
4
1M
0.3M
134.62
134.65
134.64
Reaction Order and Rate Laws ^ ^ ^
Need help with finding the reaction after mixing well for Hcl and Na2S2O4 and the reaction rate (sec). How do you find??
and
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.
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
27.44
27.40
27.42
C2, D2
6
6
8
1M
0.3M
31.66
31.68
31.67
C3, D3
4
8
8
1M
0.3M
46.90
46.98
46.94
Explanation / Answer
calculate moles of both reactants.
calculate the one in excess
convert to Molar concentration of each
Na2S2O3 + 2 HCl = H2O + 2 NaCl + S + SO2
1 mole of Na2S2O3 reacts with 2 moles of HCl
Its not specified how many ml is 1 drop.
It is thus difficult to calculate the concentration of each in the final solution and hence the rate.
The unit of rate suggests it is a first order reaction,
thus,
Rate = k[A]
ln[A]t = -kt + ln[A]o
Find k
substitute in the rate equation to find the rate
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