Problem

Explain why an egg cooks more slowly in boiling w…

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Problem 7 Medium Difficulty

Describe the effect of each of the following on the rate of the reaction of magnesium metal with a solution of hydrochloric acid: the molarity of the hydrochloric acid, the temperature of the solution, and the size of the pieces of magnesium.

Answer

The change in molarity of $H C l$ and reaction rate are proportional.
The change in temperature is proportional to reaction rate.
The size of the magnesium particles and reaction rate are reversely proportional.

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Chemistry 102

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Video Transcript

Okay, So our question is asking us, um the effect of different variables on the rate of the, um, reaction between HCL and magnesium, and, uh, I drew three different graphs here to show, um, the three variables that they're asking about the 1st 1 is ah, bee concentration of hydrochloric acid. Um, you can really see it, but it's down here. The concentration of hydrochloric acid, the 2nd 1 is rate versus temperature in the 3rd 1 they asked about is rate versus the particle size. And so to begin, this has to do with, um, the collision theory, which, um, has a couple of factors, the first being that molecules have to collide in order to react. The 2nd 1 is, um, they have to have they have to overcome the activation energy of the reaction, and then the third is that they have to have the right orientation in order to, um, have a successful reaction. And so, uh, mostly, we just have to think of the first to be overcoming the activation energy and that they must collide. And so, if we're thinking are about our first variable, which is a concentration of hydrochloric acid, If um you increase the, uh, concentration of hydrochloric acid. This is increasing. Going this way, you there's more particles in your solution, so there's more chance for particles to collide and make a reaction. So as your concentration of your reactant increases, also, your rate increases. So your graph would look something like this. Um, for the next one, let's see, we have rate versus temperature. And so this has to do with overcoming the, um, activation energy and also, um, more collisions. Because as you increase the temperature, which is increasing going this way, um, then, um, you have, uh, more energy in your solution. And also, your particles are moving, uh, more quickly, and so there's more of a chance for them to collide. So, as ah, your temperature increases, your rate will also increase. So your graph would look something like this. Sorry. It's a bit messy. And then finally, um, the third variable that they're asking about his particle size. And so for this one, I am two different pictures here. This one is very small particles, and this one is a one very large particle. And so, if you're thinking about it, um, knowing that particles have to, uh, collide in order to react. If a particle, um, let's see, you have a particle right here in its colliding with this large particle. The only point that it could Clyde with is right here. It couldn't glide with any point inside of this very large particle. And so, um, it limits it to only being able to collide with thesis surface. And with these ones, uh, like this particle could collide with that one. Or it could collide with this one, or it could quite this one. Um, so this, uh, these smaller particles have like a higher surface area to them. Um, so it's it's easier for them to collide with other particles, Um, because they have a higher surface area. So for this graph rate versus increasing particle size, so as you increase your particle size, your rate will actually decrease for this one. So your graph would look something like this. Um, so this one you're, um, particle size and rate, uh, are inversely proportional. This one year rate versus temperature are proportional to each other, and for this one rate versus your concentration of hydrochloric acid are proportional to each other.

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