The rate expression for the reaction, A(g)+B(g) longrightarrow C(g), is rate =k[A]2[B]1 / 2 What changes in the initial concentrations of A and B will cause the rate of reaction to increase by a factor of eight?

Question

The rate expression for the reaction, A(g)+B(g) longrightarrow C(g), is rate =k[A]2[B]1 / 2 What changes in the initial concentrations of A and B will cause the rate of reaction to increase by a factor of eight? (A) [A] × 2 ;[B] × 2 (B) [A] × 2 ;[B] × 4 (C) [A] × 1 ;[B] × 4 (D) [A] × 4 ;[B] × 1

Tardigrade Admin · Accepted Answer

If [A prime]=2[A], [B prime]=4[B] Rate =k[A prime]2[B prime]1 / 2=k[2 A]2[4 B]1 / 2=k[A]2[B]1 / 2 × 8

Q. The rate expression for the reaction,
$A_{(g)} + B_{(g)} ⟶ C_{(g)}$ , is rate $= k [A]^{2} [B]^{1/2}$
What changes in the initial concentrations of $A$ and $B$ will cause the rate of reaction to increase by a factor of eight?

$[A] \times 2; [B] \times 2$

$[A] \times 2; [B] \times 4$

$[A] \times 1; [B] \times 4$

$[A] \times 4; [B] \times 1$

If $[A^{'}] = 2 [A], [B^{'}] = 4 [B]$

Rate $= k [A^{'}]^{2} [B^{'}]^{1/2} = k [2 A]^{2} [4 B]^{1/2} = k [A]^{2} [B]^{1/2} \times 8$

Q. The rate expression for the reaction, A(g)​+B(g)​⟶C(g)​, is rate =k[A]2[B]1/2 What changes in the initial concentrations of A and B will cause the rate of reaction to increase by a factor of eight?

[A]×2;[B]×2

[A]×2;[B]×4

[A]×1;[B]×4

[A]×4;[B]×1