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In the following hypothetical reaction A + 3B   2C + D, initial moles of A is twice that of B. If at equilibrium moles of B and C are equal, % of B reacted is (A) 10% (B) 20% (C) 40% (D) 60%

In the following hypothetical reaction A + 3B 
 2C + D, initial moles of A is twice that of B. If
at equilibrium moles of B and C are equal, % of B reacted is
(A) 10% (B) 20% (C) 40% (D) 60%

Grade:11

1 Answers

Sunil Kumar FP
askIITians Faculty 183 Points
9 years ago
A + 3B---------->2C + D
intial 2 1 0 0
at equilibrium 2-x 1-3x 2x x
given mole of B=mole of C
1-3x=2x
5x=1
x=.2
percentage of B reacted is 1-3x/1 *100
=(1-3*.2)*100
=40%
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