This chemistry question involves key chemical concepts and calculations. The detailed solution below walks through each step, from identifying the reaction type to computing the final answer.
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Step 1: Complete Table 1. The reaction rate is inversely proportional to the time taken for the cross mark to disappear, so Rate = (1)/(Time(t)). We will calculate the rate for each experiment using the given Time(t) values. Expt 1: Rate = (1)/(83 s) ≈ 0.0120 s^-1 Expt 2: Rate = (1)/(111 s) ≈ 0.00901 s^-1 Expt 3: Rate = (1)/(128 s) ≈ 0.00781 s^-1 Expt 4: Rate = (1)/(285 s) ≈ 0.00351 s^-1 Expt 5: Rate = (1)/(884 s) ≈ 0.00113 s^-1 Here is the completed Table 1: | Expt No | Vol of sol A (cm³) | Vol of sol B (cm³) | Vol of Distilled water/cm³ | B/moldm⁻³ | Time(t)/sec | Rate, 1/t (s⁻¹) | | :------ | :----------------- | :----------------- | :-------------------------- | :---------------------- | :---------- | :-------------- | | 1 | 25.0 | 25.0 | 0 | 0.5 | 83 | 0.0120 | | 2 | 25.0 | 20.0 | 5 | 0.4 | 111 | 0.00901 | | 3 | 25.0 | 15.0 | 10 | 0.3 | 128 | 0.00781 | | 4 | 25.0 | 10.0 | 15 | 0.2 | 285 | 0.00351 | | 5 | 25.0 | 5.0 | 20 | 0.1 | 884 | 0.00113 | Step 2: Plot a graph of reaction rate (vertical axis) against concentration of B ([S₂O₃²⁻]) (horizontal axis). To plot the graph: Draw and label the horizontal axis (x-axis) as "Concentration of [S₂O₃²⁻] / moldm⁻³". Choose a suitable scale that covers the range from 0.1 to 0.5 moldm⁻³. Draw and label the vertical axis (y-axis) as "Reaction Rate / s⁻¹". Choose a suitable scale that covers the range from approximately 0.001 to 0.012 s⁻¹. Plot the following points from the completed Table 1: (0.5, 0.0120) (0.4, 0.00901) (0.3, 0.00781) (0.2, 0.00351) (0.1, 0.00113) Draw a smooth curve or line of best fit through the plotted points. The graph should show that as the concentration of [S₂O₃²⁻] decreases, the reaction rate also decreases. The relationship appears to be non-linear, suggesting the reaction order with respect to [S₂O₃²⁻] is not simply first order. Send me the next one 📸