I was given this problem: Liquid nitrogen trichloride is heated in a 2.50-L clos

Question

I was given this problem: Liquid nitrogen trichloride is heated in a 2.50-L closed reaction vessel until it decomposes completely to gaseous elements. The resulting mixture exerts a pressure of 754 mmHg at 95 0C. What is the mass of the original sample.

and this was the explained 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= 754/760 atm ; T= 368 K

Step5 PV = nRT ; 754x2.50/760 = (2w/120.5) x .0821 x368

Step6 w= 4.946 g


But how do you determine step 3 without any other given information?

Explanation / Answer

Can someone explain to me how you found that w? I have no idea how to calculate steps 2 and 3

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