Question

In: Chemistry

Can someone verify for me that I'm doing this correctly? For data analysis, part b: All...

Can someone verify for me that I'm doing this correctly?

For data analysis, part b:

All S₂O₃^2- is consumed at the end of the reaction. Therefore, the moles of S₂O₃^2- consumed can be calculated using the equation below.
(moles S₂O₃^2-)_consumed = M_stock x (V_stock)

My instructor states "The stock sodium thiosulfate (S2O3) is 0.01M

0.01M x 0.010 L = 0.0001moles S2O3"

So I did the rest of this accordingly (below), and it differs a lot from what's on this website. Any explanations would be appreciated, thanks!

Chemical Kinetics

Lab Results

Record the following lab data in the table below for trial 4. (done)

(a) volume of potassium iodide solution added to Erlenmeyer flask A in mL	12.5 mL
(b) volume of potassium nitrate solution added to Erlenmeyer flask A in mL	12.5 mL
(c) volume of starch solution added to Erlenmeyer flask A in mL	5 mL
(d) volume of (NH₄)₂S₂O₈ solution added to Erlenmeyer flask B in mL	25 mL
(e) volume of (NH₄)₂SO₄ solution added to Erlenmeyer flask B in mL	0 mL
(f) volume of Na₂S₂O₃ solution added to Erlenmeyer flask B in mL	10 mL
(g) the initial color of the solution after adding flask B to flask A	grey/clear
(h) time for color change	41 s
(i) color of the final solution	black

Data Analysis

Fill in the following table. Look below the table for instructions on how to calculate the values for each row of the table.

a	total volume (L)	0.065 L
b	mol S₂O₃^2-_consumed	0.0001 moles
c	mol I₃^-_produced	0.00005 moles
d	[S₂O₃^2-] _consumed (M)	0.001538 mol/L
e	[I₃-] _produced (M)	0.000769 mol/L

a) Calculate the final volume of the reaction mixture after the contents of beaker B are added to beaker A. Report your answer in liters.

b) All S₂O₃^2- is consumed at the end of the reaction. Therefore, the moles of S₂O₃^2- consumed can be calculated using the equation below.
(moles S₂O₃^2-)_consumed = M_stock x (V_stock)

c) The I₃^- produced in reaction 1 reacts with S₂O₃^2- in reaction 2 as shown.
I₃^- (aq) 2S₂O₃^2- (aq) → 3I^- (aq) S₄O₆^2- (aq)

Therefore, for every mole of I₃^- produced, 2 moles of S₂O₃^2- have reacted.
(moles I₃^-)_produced = (moles S₂O₃^2-)_consumed / 2

d) [S₂O₃^2-]_consumed = (moles S₂O₃^2-)_consumed / (V_total)

e) Calculation is the same as d, but using I₃^- instead of S₂O₃^2-.

Expert Solution

queen_honey_blossom answered 2 years ago

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