The provided table is for an experiment that investigates the relationship between reaction rate and temperature. Complete the table by calculating the values for 1/t. The temperature column is intent

The reaction rate is often taken as inversely proportional to the time taken for the reaction to complete.

$$\text{Rate} = \frac{1}{\text{Time(t)}}$$

• Expt 1: $1/t = \frac{1}{70 \text{ s}} \approx 0.0143 \text{ s}^{-1}$
• Expt 2: $1/t = \frac{1}{74 \text{ s}} \approx 0.0135 \text{ s}^{-1}$
• Expt 3: $1/t = \frac{1}{78 \text{ s}} \approx 0.0128 \text{ s}^{-1}$
• Expt 4: $1/t = \frac{1}{82 \text{ s}} \approx 0.0122 \text{ s}^{-1}$
• Expt 5: $1/t = \frac{1}{86 \text{ s}} \approx 0.0116 \text{ s}^{-1}$
• Expt 6: $1/t = \frac{1}{90 \text{ s}} \approx 0.0111 \text{ s}^{-1}$

The temperature column is left blank as the values are not provided and cannot be determined from the image.

Here is the completed table:

Experiment	Volume of solution I / cm³	Volume of water / cm³	Volume of dilute H₂SO₄ / cm³	Volume of starch / cm³	Volume of solution J / cm³	Time, t / sec	Temperature / °C	1/t / s⁻¹
1	30.0	10.0	20	5.0	10.0	70		0.0143
2	26.0	10.0	20	5.0	10.0	74		0.0135
3	22.0	10.0	20	5.0	10.0	78		0.0128
4	18.0	10.0	20	5.0	10.0	82		0.0122
5	14.0	10.0	20	5.0	10.0	86		0.0116
6	10.0	10.0	20	5.0	10.0	90		0.0111

To plot the graph:

• Draw and label the horizontal axis (x-axis) as "Volume of solution I / cm³". Choose a suitable scale that covers the range from 10.0 to 30.0 cm³.
• Draw and label the vertical axis (y-axis) as "Reaction Rate, 1/t / s⁻¹". Choose a suitable scale that covers the range from approximately 0.011 to 0.015 s⁻¹.
• Plot the following points from the completed table:
  • (30.0, 0.0143)
  • (26.0, 0.0135)
  • (22.0, 0.0128)
  • (18.0, 0.0122)
  • (14.0, 0.0116)
  • (10.0, 0.0111)
• Draw a smooth curve or line of best fit through the plotted points.

The graph should show that as the volume of solution I (and thus the concentration of iodate ions) decreases, the reaction rate (1/t) also decreases.