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  • Calculate the pressure (in atm) exerted by 8.5g of ammonia contained in a 0.5L vessel at 300K. For ammonia, <img alt="\small a=4.0atmL^2mol^{-2}" src="http://entrancecorner.oncodecogs.com/gif.latex

Calculate the pressure (in atm) exerted by 8.5g of ammonia contained in a 0.5L vessel at 300K. For ammonia, \small a=4.0atmL^2mol^{-2} , \small b=0.036Lmol^{-1}

Option: 1

20.23


Option: 2

21.51


Option: 3

19.34


Option: 4

24.23


Answers (1)

best_answer

We have
Number of moles of ammonia, n = 8.5/17 = 0.5 moles
Now, according to Van der Waals equation, we have

\\\mathrm{\left ( P\: +\: \frac{an^{2}}{V^{2}} \right )\left ( V\: -\: nb \right )\: =\: nRT}\\\\\mathrm{P\: =\: \frac{nRT}{(V\: -\: nb)}\: -\: \frac{an^{2}}{V^{2}}\: =\: \frac{0.5\: x\: 0.082\: x\: 300}{0.5\: -\: 0.5\: x\: 0.036}\: -\: \frac{4(0.5)^{2}}{(0.5)^{2}}}\\\\\mathrm{\: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: =\: 21.51\: atm}

 

Posted by

sudhir kumar

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