AP EAMCET202317 May 2023Morning ShiftChemistryChemical KineticsActual
Consider the reaction carried out at T ( K ) A ( g )+ B ( g ) C ( g ) The rate law for this reaction is r=k[A]^1[B]^2 . The concentration of A in experiment 2 and rate in experiment 3 shown as x and z in the table, x and z are respectively array |l|l|l|l| array l Experi- ment array & [ A ] mol L ⁻¹ & [ B ] mol L ⁻¹ & array l Initial rate ( m o l ~ L ^ - 1 ~ s ^ - 1 ) array 1 & 0.05 & 0.05 & R 2 & x & 0.05 & 2 R 3 & 0
Options
- Ax=0.10 z=8 R
- Bx=0.05 z=4 R
- Cx=0.10 z=16 R
- D1) x=0.20 z =16 R
Correct answer
C. x=0.10 z=16 R
Step-by-step solution
According to the rate law:- When [ A ]₂=4[ ~A ]₁ and [ B ]₂=2[ ~B ]₁ aligned rate & = r = z = k [4 ~A ][2 ~B ]^2= k 4 4 [ A ]₁[ ~B ]₁ & =16 R . aligned And when [ B ] is kept constant, and [ A ]₂= x aligned rate & =r₂=2 R =2 k (0.05)(0.05)^2 & = k (0.10)(0.05)^2 & = k ( x )(0.05)^2 aligned Thus, x=0.10 .