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Physical Chemistry Question (work done during decomposition)
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[QUOTE="Paint, post: 2625140, member: 237729"] [h2]Homework Statement [/h2] A sample consisting of 1.0 mol of calcium carbonate CaCO3(s) was heated to 800°C, when it decomposed (CaCO3 → CaO + CO2). The heating was carried out in a container fitted with a piston which was initially resting on the solid. Calculate the work done during complete decomposition at 1.0 atm. What work would be done if instead of having a piston the container was open to the atmosphere? [h2]Homework Equations[/h2] Expansion work against constant external pressure: w=-[I]p[SUB]ex[/SUB][/I][tex]\Delta[/tex]V [h2]The Attempt at a Solution[/h2] Ok the textbook gives an example, so I tried following that. Because V[SUB]f[/SUB]>>V[SUB]i[/SUB], and V[SUB]f[/SUB]=nRT/p[SUB]ex[/SUB], then w=-p[SUB]ex[/SUB] x nRT/p[SUB]ex[/SUB]=-nRT (im assuming n is number of moles of CO[SUB]2[/SUB]?). 1 mole of CaCO3 makes 1 mole of CO2, so plugging in numbers, I get 8.9kJ, although I don't use the 1 atm pressure at all, so I'm thinking I'm doing the second part of the question first. Any help would be appreciated. [/QUOTE]
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Physical Chemistry Question (work done during decomposition)
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