How much expansion work is done on the system when exactly 1mol of solid ammonium chloride, NH4C1, decomposes completelyto yield gaseous ammonia, NH3, and hydrogen chloride, HCl, at atemperature of 1280 K. Treat the expansion as irreversible and thegases formed as perfect.
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How much expansion work is done on the system when exactly 1 mol of solid ammonium chloride, NH4Cl, decomposes completely to yield gaseous ammonia, NH3, and hydrogen chloride, HCl, at a temperature of 1280 K. Treat the expansion as irreversible and the gases formed as perfect.
I'm not sure how to compute the two volumes required to use the formula:
W=nRT∫ViVfdVV
Do I assume 1 atm=101.325 kPa. I did that and was able to use the ideal gas law: V=nRTP to get the final volume of the 1 mole of gas, but I'm unsure how to choose the initial volume (0 won't work here as it leads to −∞).
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