1
Question
Observe the following reaction: A(g)+3B(g)→2C(g)
The rate of this reaction, −d[A]dt is 3×10−3 mol.lit−1.min−1. Then the value of −d[B]dt in mol.lit−1.min−1 is:
Observe the following reaction: A(g)+3B(g)→2C(g)
The rate of this reaction, −d[A]dt is 3×10−3 mol.lit−1.min−1. Then the value of −d[B]dt in mol.lit−1.min−1 is:
Open in App
Solution
The correct option is C 9×10−3
A+3B→2C
rate=−d[A]dt=−13d[B]dt
−d[B]dt=+3[−d[A]dt]
=3×3×10−3
=9×10−3mol. lit−1min−1
A+3B→2C
rate=−d[A]dt=−13d[B]dt
−d[B]dt=+3[−d[A]dt]
=3×3×10−3
=9×10−3mol. lit−1min−1
Suggest Corrections
0
Similar questions