A sample of liquid nitrogen trichloride in a 2.50 L closed reaction vessel is he

Question

A sample of liquid nitrogen trichloride in a 2.50 L closed reaction vessel is heated until it decomposes completely to gaseous elements. The resulting mixture exerts a pressure of 745 mm Hg at 95 degress C. What was the mass of the original sample? (Write a balanced equation.) A sample of liquid nitrogen trichloride in a 2.50 L closed reaction vessel is heated until it decomposes completely to gaseous elements. The resulting mixture exerts a pressure of 745 mm Hg at 95 degress C. What was the mass of the original sample? (Write a balanced equation.)

Explanation / Answer

Step1 Let w be mass of sample ; Molar mass of NCl3 =120.5

Step2 Moles of NCl3 =w/120.5


Step3 2NCl3 (g)---> N2(g)+3Cl2(g) ; Moles of products formed =2xMoles of NCl3=2w/120.5

Step4 P= 745/760 atm ; T= 368 K

Step5 PV = nRT ; 745x2.50/760 = (2w/120.5) x .0821 x368

Step6 w= 4.887 g

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