The change in reactant orientation can affect the rate of the chemical reaction between magnesium and hydrochloric acid by influencing the frequency and effectiveness of collisions between the reactant particles. This is based on the collision theory, which states that for a reaction to occur, the reactant particles must collide with the appropriate orientation and sufficient energy.To investigate the effect of reactant orientation on the rate of the reaction between magnesium and hydrochloric acid, you can perform a series of experiments with varying orientations of the magnesium ribbon. Here's a suggested procedure:1. Prepare a series of hydrochloric acid solutions with the same concentration in separate beakers or conical flasks.2. Cut magnesium ribbons into equal lengths and modify their orientations as follows: a. Straight ribbon no change in orientation b. Ribbon coiled into a loose spiral c. Ribbon coiled into a tight spiral3. Measure and record the initial temperature of the hydrochloric acid solutions.4. Add the magnesium ribbons with different orientations to the separate hydrochloric acid solutions simultaneously, and start a timer for each reaction.5. Observe the reactions and measure the time taken for each magnesium ribbon to completely dissolve in the hydrochloric acid. This is the reaction time.6. Calculate the rate of each reaction by dividing the amount of magnesium in moles by the reaction time. The rate can be expressed in moles per second mol/s .7. Compare the rates of the reactions with different magnesium orientations. A faster rate indicates a higher frequency of effective collisions between the magnesium and hydrochloric acid particles.8. Analyze the results and draw conclusions about the effect of reactant orientation on the rate of the chemical reaction between magnesium and hydrochloric acid.By comparing the reaction rates, you can determine how the orientation of the magnesium ribbon affects the rate of the reaction. A possible explanation for any observed differences in reaction rates could be that a change in orientation alters the surface area of the magnesium ribbon exposed to the hydrochloric acid, thus affecting the frequency and effectiveness of collisions between the reactant particles.