Questions: Experiment 10 Reaction Orders (ML 10) Concentration Trial 1 Trial 2 Trial 3 ------------ Concentration of iodide solution (mM) 100.0 100.0 100.0 Concentration of thiosulfate solution (mM) 31.5 31.5 31.5 Concentration of hydrogen peroxide solution (mM) 176.5 176.5 176.5 Temperature of iodide solution (°C) 25.0 Volume of iodide solution (I-)used (mL) 10.0 Volume of thiosulfate solution (S2O32-) used (mL) 1.0 Volume of DI water used (mL) 2.5 Volume of hydrogen peroxide solution (H2O2) used (mL) 7.5 Time (s) 17.6 Observations solution turned blue Initial concentration of iodide in reaction (mM) Initial concentration of thiosulfate in reaction (mM) Concentration of hydrogen peroxide in reaction (mM) Initial Rate (mM/s) - Temperature Concentration of iodide solution (mM) Trial 1 Trial 2 Trial 3 ------------ Concentration of thiosulfate solution (mM) 100.0 100.0 100.0 Concentration of hydrogen peroxide solution (mM) 20.1 20.1 20.1 Temperature of iodide solution (°C) 176.0 176.0 176.0 PHASE 2: Observe reaction rate with 1) Complete the following steps. Place all used glassware in Wash/Waste bin. plate. Turn on stir plate Use 10-mL graduated pipet to transfer 7.5 mL of hydrogen peroxide solution (H2O2) to Trial 1 beaker. Stop timer when solution's color changes. Record exact volume and time in Lab Data Record your observations in Lab Data Calculate initial concentration of each reactant. Record in Lab Data Calculate initial rate of the reaction. Record in Lab Data Pour Trial 1 mixture into "Chemicals for Disposal" beaker and place used beaker into Wash/Waste bin GO TO PHASE 3

Experiment 10 Reaction Orders (ML 10) Concentration Trial 1 Trial 2 Trial 3 ------------ Concentration of iodide solution (mM) 100.0 100.0 100.0 Concentration of thiosulfate solution (mM) 31.5 31.5 31.5 Concentration of hydrogen peroxide solution (mM) 176.5 176.5 176.5 Temperature of iodide solution (°C) 25.0 Volume of iodide solution (I-)used (mL) 10.0 Volume of thiosulfate solution (S2O32-) used (mL) 1.0 Volume of DI water used (mL) 2.5 Volume of hydrogen peroxide solution (H2O2) used (mL) 7.5 Time (s) 17.6 Observations solution turned blue Initial concentration of iodide in reaction (mM) Initial concentration of thiosulfate in reaction (mM) Concentration of hydrogen peroxide in reaction (mM) Initial Rate (mM/s) - Temperature Concentration of iodide solution (mM) Trial 1 Trial 2 Trial 3 ------------ Concentration of thiosulfate solution (mM) 100.0 100.0 100.0 Concentration of hydrogen peroxide solution (mM) 20.1 20.1 20.1 Temperature of iodide solution (°C) 176.0 176.0 176.0 PHASE 2: Observe reaction rate with 1) Complete the following steps. Place all used glassware in Wash/Waste bin. plate. Turn on stir plate Use 10-mL graduated pipet to transfer 7.5 mL of hydrogen peroxide solution (H2O2) to Trial 1 beaker. Stop timer when solution's color changes. Record exact volume and time in Lab Data Record your observations in Lab Data Calculate initial concentration of each reactant. Record in Lab Data Calculate initial rate of the reaction. Record in Lab Data Pour Trial 1 mixture into "Chemicals for Disposal" beaker and place used beaker into Wash/Waste bin GO TO PHASE 3
Transcript text: Experiment 10 Reaction Orders (ML 10) Concentration \begin{tabular}{|c|c|c|c|} \hline & Trial 1 & Trial 2 & Trial 3 \\ \hline Concentration of iodide solution ( mM ) & 100.0 & 100.0 & 100.0 \\ \hline Concentration of thiosulfate solution ( mM ) & 31.5 & 31.5 & 31.5 \\ \hline Concentration of hydrogen peroxide solution ( $\mathrm{m} M$ ) & 176.5 & 176.5 & 176.5 \\ \hline Temperature of iodide solution ( ${ }^{\circ} \mathrm{C}$ ) & 25.0 & & \\ \hline Volume of iodide solution $\left(\mathrm{I}^{-}\right)$used ( mL ) & 10.0 & & \\ \hline Volume of thiosulfate solution $\left(\mathrm{S}_{2} \mathrm{O}_{3}{ }^{2-}\right)$ used ( mL ) & 1.0 & & \\ \hline Volume of DI water used ( mL ) & 2.5 & & \\ \hline Volume of hydrogen peroxide solution $\left(\mathrm{H}_{2} \mathrm{O}_{2}\right)$ used $(\mathrm{mL})$ & 7.5 & & \\ \hline Time (s) & 17.6 & & \\ \hline Observations & \begin{tabular}{l} solution turned \\ blue \end{tabular} & & \\ \hline Initial concentration of iodide in reaction ( mM ) & & & \\ \hline Initial concentration of thiosulfate in reaction ( mM ) & & & \\ \hline concentration of hydrogen peroxide in reaction ( $\mathrm{m} M$ ) & & & \\ \hline Initial Rate ( mM/s ) & - & & \\ \hline \end{tabular} emperature \begin{tabular}{|c|c|c|c|} \hline Concentration of iodide solution $(\mathbf{m} M)$ & Trial 1 & Trial 2 & Trial 3 \\ \hline Concentration of thiosulfate solution $(\mathbf{m} M)$ & 100.0 & 100.0 & 100.0 \\ \hline Concentration of hydrogen peroxide solution $(\mathbf{m} M)$ & 20.1 & 20.1 & 20.1 \\ \hline Temperature of iodide solution $\left({ }^{\circ} \mathbf{C}\right)$ & 176.0 & 176.0 & 176.0 \\ \hline \end{tabular} PHASE 2: Observe reaction rate with 1) Complete the following steps. Place all used glassware in Wash/Waste bin. plate. Turn on stir plate 7 Use $10-\mathrm{mL}$ graduated pipet to transfer 7.5 mL of hydrogen peroxide solution $\left(\mathrm{H}_{2} \mathrm{O}_{2}\right)$ to Trial 1 beaker. Stop timer when solution's color changes. Record exact volume and time in Lab Data 8 Record your observations in Lab Data 9 Calculate initial concentration of each reactant. Record in Lab Data 10 Calculate initial rate of the reaction. Record in Lab Data 11 Pour Trial 1 mixture into "Chemicals for Disposal" beaker and place used beaker into Wash/Waste bin GO TO PHASE 3
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Solution

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Solution Steps

Step 1: Calculate Initial Concentration of Iodide in Reaction

To find the initial concentration of iodide (\(\mathrm{I}^-\)) in the reaction, use the dilution formula: \[ C_{\text{initial}} = \frac{C_{\text{stock}} \times V_{\text{used}}}{V_{\text{total}}} \] Given:

  • \(C_{\text{stock}} = 100.0 \, \text{mM}\)
  • \(V_{\text{used}} = 10.0 \, \text{mL}\)
  • \(V_{\text{total}} = 10.0 \, \text{mL} + 1.0 \, \text{mL} + 2.5 \, \text{mL} + 7.5 \, \text{mL} = 21.0 \, \text{mL}\)

\[ C_{\text{initial}} = \frac{100.0 \, \text{mM} \times 10.0 \, \text{mL}}{21.0 \, \text{mL}} = 47.6190 \, \text{mM} \]

\(\boxed{47.6190 \, \text{mM}}\)

Step 2: Calculate Initial Concentration of Thiosulfate in Reaction

Using the same dilution formula for thiosulfate (\(\mathrm{S}_2\mathrm{O}_3^{2-}\)):

Given:

  • \(C_{\text{stock}} = 31.5 \, \text{mM}\)
  • \(V_{\text{used}} = 1.0 \, \text{mL}\)
  • \(V_{\text{total}} = 21.0 \, \text{mL}\)

\[ C_{\text{initial}} = \frac{31.5 \, \text{mM} \times 1.0 \, \text{mL}}{21.0 \, \text{mL}} = 1.5000 \, \text{mM} \]

\(\boxed{1.5000 \, \text{mM}}\)

Step 3: Calculate Initial Concentration of Hydrogen Peroxide in Reaction

Using the same dilution formula for hydrogen peroxide (\(\mathrm{H}_2\mathrm{O}_2\)):

Given:

  • \(C_{\text{stock}} = 176.5 \, \text{mM}\)
  • \(V_{\text{used}} = 7.5 \, \text{mL}\)
  • \(V_{\text{total}} = 21.0 \, \text{mL}\)

\[ C_{\text{initial}} = \frac{176.5 \, \text{mM} \times 7.5 \, \text{mL}}{21.0 \, \text{mL}} = 63.0357 \, \text{mM} \]

\(\boxed{63.0357 \, \text{mM}}\)

Final Answer

  • Initial concentration of iodide in reaction: \(\boxed{47.6190 \, \text{mM}}\)
  • Initial concentration of thiosulfate in reaction: \(\boxed{1.5000 \, \text{mM}}\)
  • Initial concentration of hydrogen peroxide in reaction: \(\boxed{63.0357 \, \text{mM}}\)
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