Can someone add more details to this to make it better and explain the changes when my character goes through thermal energy.
there was an ice cube made by the water from the freezer in an ice shop.
the ice cube, with a bunch of other ice cubes, were taken to be packed and sold to a restaurant. the ice cube was excited to where he was going while the other ice cubes are just meh. now that the ice cubes arrived, a restaurant worker stores the ice cubes in a cooler and later used to put ice in a lemonade. while the lemonade in a glass cup was carried outside the porch of the restaurant by the waiter, the ice cube was fascinated by the environment of the restaurant. the waiter finally serves the thirsty customer and the customer drank almost half of the lemonade but the ice cube did not get in the man's mouth. instead the other ice cubes went. the ice cube feared the person. shortly after checking his phone, the customer was about to reach on to the glass until the hands accidentally pushes the glass over and falls. the ice cube and the remaining ice cubes spread away with the wasted lemonade liquid. no one bothered cleaning up the ice cubes, only the glass shards because the floor is a smooth concrete. outside was really hot from the sun anyways so it would melt the ice cube and sooner evaporate. as it was in liquid form, the "ice cube" was feeling relaxed because it was just chilling on the floor. and when it evaporates, the ice cubes becomes more fascinated since it goes up to the sky while having a sky-view from above.

Experiment: effect of solution concentration on reaction rate you have learned that as the concentration of reactants increases, there will most likely be a greater number of collisions, and hence increase the rate of a reaction. in this experiment, you will see a demonstration of this, with a twist. there will be three reactions going on in this experiment. objectives determine how solution concentration can affect the rate of a reaction. the first reaction will be a reaction of the iodide ion (i-1) with hydrogen peroxide (h2o2) in an acidic solution. this reaction produces a slightly orange solution. in our experiment, we will add some orange food coloring to make this solution more orange. 2 h+ (aq) + 2 i- (aq) + h2o2 (aq) ⟶ i2 (aq) + 2 h2o (l) the next reaction will be between the iodine and starch i2 + starch ⟶ i2-starch complex (blue-black) so, when starch is added to the iodine solution made from the first reaction, the solution will turn black immediately, so it is difficult to find the rate of reaction. in order to be able to time this reaction, you will slow it down with another reaction. adding ascorbic acid will react with the iodine, reducing the concentration of the iodine available to react with the starch. c6h8o6 (aq) + i2 (aq) ⟶ 2i- (aq) + c6h6o6 (aq) + 2 h+ (aq) when the ascorbic acid is used up, the remaining iodine molecules can react with the starch and form the black color. the more ascorbic acid you add, the slower the reaction to form the iodine-starch complex will be. use your data and observations to complete the assignment. analysis and conclusions submit your data and the answers to these questions in the essay box below. what was your hypothesis? plot your data as drops of ascorbic acid vs. time. as the concentration of ascorbic acid was increased, did the rate of the formation of the iodine-starch complex increase or decrease? explain your answer in terms of the chemical reactions involved. was your hypothesis correct? make a general rule about the effects of concentration of reactants on reaction rates. for practice, the molecular formula for ascorbic acid is c6h8o6, and you used 6 g in this experiment, calculate the molarity of the ascorbic acid. now calculate the concentration in moles per drop (assume 1 ml = 20 drops).