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Ideal Gas Law and Pressure at 80°C
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[QUOTE="SakuRERE, post: 6105972, member: 651815"] [h2]Homework Statement [/h2] An ideal gas has a molar mass of 40 g and a density of 1.2 kg m-3 at 80°C. What is its pressure at that temperature? [h2]Homework Equations[/h2] PV=nRT R constant= 8.314 n= number of moles T= tempreture in kelvin density=Mass/ Volume [h2]The Attempt at a Solution[/h2] i simply solved it like this: i found first the volume: V=molar mass/ density V= 0.04kg/ 1.2kg/m^3 = 0.03 m^3 and then i just substituted in the ideal gas law P=nRT/V (where n is the moles and here we have 1 mole) P= (1)*(8.314)*(353K)/ (0.03) = 97828.06 Pa but my professor solved it like this: T = 273 + 80 = 353 K PV = nRT m = rV so V = 0.04 / 1.2 with n = 1 (since 1 mole of gas has a mass of 40 g, or 0.04 kg) P = RT/V = 8.3 x 353 x 1.2/0.04 = 8.79x104 Pa I noticed that he didn't find the volume first and then substituted but he substituted directly in the ideal gas law! why it should be like this!? [/QUOTE]
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Ideal Gas Law and Pressure at 80°C
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