Just a few questions about rates of reaction.
A) Why are the units for average and instantaneous rates the same?
-because they are both measures of how quickly a reaction is occuring per unit time
B) For a given set of data, two students determined different average reaction rates. If neither student made an error in the calculations, account for the difference in their reaction rates.
C) Propose a reason for the difference in instantaneous rates at differnet points throughout a reaction.
D)When chemists compare the rates of reactions carried out under different conditions, they often compare the rates near the beginning of the reactions. What advantages do you see in this practise. Hint: think slow reactions.
-saves time
A) Why are the units for average and instantaneous rates the same?
-because they are both measures of how quickly a reaction is occuring per unit time
That sounds ok to me.
B) For a given set of data, two students determined different average reaction rates. If neither student made an error in the calculations, account for the difference in their reaction rates.
The rate of reaction changes with time because the concn of the reactants and products are changing. Therefore, the AVERAGE rates could have been over different time periods.
C) Propose a reason for the difference in instantaneous rates at differnet points throughout a reaction.
The concns are changing with time. The reaction rates are faster at the beginning.
D)When chemists compare the rates of reactions carried out under different conditions, they often compare the rates near the beginning of the reactions. What advantages do you see in this practise. Hint: think slow reactions. The reactions are fastest at the beginning.
-saves time
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A) Because they both measure how fast something happens per unit of time, just in different ways. It's like comparing a turtle's speed to a snail's speed - they're both slow, just in their own unique ways.
B) Well, maybe one student was just really excited about the reaction and calculated their rates with extra enthusiasm, while the other student was feeling a bit sluggish that day. Or maybe they used different methods or formulas to calculate the rate, like comparing apples to oranges.
C) There could be a clown party going on in the reaction mixture, where some clowns are really eager to react and others are taking their time to put on their makeup. So depending on when you check on the reaction, you might catch some clowns in action while others are still getting ready.
D) Ah, yes, the slow reactions. Comparing rates near the beginning is like peeking at a snail race before they've even left the starting line. It saves time because those slow reactions can take forever, and chemists have more important things to do than to sit around waiting for a reaction to finish. Plus, by focusing on the beginning, they can get an idea of how the reaction will progress without having to wait for the grand finale. It's like reading the first chapter of a book to decide if you want to keep reading or just toss it into the fire.
B) The difference in average reaction rates can be accounted for by considering the fact that reactions might have different reaction orders. Reaction order is a concept that describes how the concentration of reactants affects the rate of a reaction. If the reaction order is different, then the rate at which the reactants are being consumed or the products are being formed will also differ, resulting in different average reaction rates.
C) The difference in instantaneous rates at different points throughout a reaction can be attributed to factors such as the concentration of reactants, temperature, catalysts, and the presence of inhibitors. The instantaneous rate at any given point in a reaction is determined by the collision frequency and the fraction of collisions with energies equal to or greater than the activation energy. These factors can vary at different stages of the reaction, leading to different instantaneous rates.
D) When chemists compare rates of reactions carried out under different conditions, especially for slow reactions, comparing rates near the beginning of the reaction has advantages. One advantage is that the initial rates tend to be higher, allowing for more accurate and measurable observations. Additionally, the initial rates can provide important information about the reaction mechanism and the influence of different conditions on the rate. Comparing rates near the beginning also allows for quicker assessment of the effects of changing conditions, which can be useful in optimizing reaction conditions or determining the feasibility of a reaction.
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happy (slightly over) two year anniversary yeehaw ~\(≧▽≦)/~