Question

Suppose a 500.mL flask is filled with 1.9mol of Br2, 1.5mol of OCl2 and 0.40mol of BrOCl. The following reaction becomes possible: +Br2gOCl2g +BrOClgBrClg The equilibrium constant K for this reaction is 5.17 at the temperature of the flask. Calculate the equilibrium molarity of BrOCl. Round your answer to two decimal places.

Answer 1

Answer:-

This question is solved by using the simple concept of chemical equilibrium using the expression of equilibrium constant and its value, concentration is calculated.

The answer is given in the image,

Answer - Brocas + Olga Brodo + Brdig 1.90 1.50 0.40 0.00 1.90-8 1.50-2 8.40+2 x K = 5017 -K? (Brodl (Bra) [Br.] [oc] 5017 = (0,40+)2) (a (1.90-2) (1:50-X) 5-11 = 0.40 X +32 2.85-3.402 +22 14.7345 - 17.578x_+50/7*?=0A0x+22 401722_17.978X+14-7345=0 2217.978 - 111.97812_4x4.17% 14.2345 ex417 x= 17,978- 8.7998 274.17 x = 1-10 So, At equilibrium Moles o Broll = 0.40 + 7010 = 1.50 mola CBTOU] = 1.50 x 1000 500.00 = 3.00 M