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welcome to our first example video. Looking at the first law of thermodynamics. To begin with, we're going to look at this P V diagrams and evaluate the work done along the two different paths. One. And to that we have here just conceptually looking at this. You should remember that when we have work that is done at a constant volume, that work is zero. So work one is going to be equal to zero jewels, plus the work done along this path, which is going to be one Kill a pascal. That's the constant pressure multiplied by the change in volume, which is 500 minus 100 cubic centimeters. So that's 400 cubic centimeters for work. Along the second path, we see that we're going to have a constant pressure of three Killah Paschal's over the same over the same change in volume, which means we have three Killah Pascal's multiplied by 400 cubic centimeters, and then we have a constant volume. Step again means we will add zero jewels. So notice here that it took more work to do go along the second path than it took to go along the first path or Rather, it required more work from the system to follow the second bath than to follow the first path. So, uh, again, path dependence is important here with our work, we need to make sure we're keeping track of which path we're taking. And we can also begin to ask ourselves, Is there a most efficient path that we could take?

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