The rate expression for reaction $A (g) + B (g) ⟶ C (g)$ is rate $= k {[A]}^{1 / 2} {[B]}^{2}$ . What change in rate if initial concentration of A and B increase by factor 4 and 2 respectively?

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Solution

The correct option is C 8
Given
A(g) + B(g) = C(g)
Let Rate of reaction be R
$R = k [A]^{\frac{1}{2}} [B]^{2}$
Let [A]=a [B]=b
$R = k * a^{\frac{1}{2}} * b^{2}$
Final Concentrations
[A]=4a [B]=2b
$R^{'} = k * (4 a)^{\frac{1}{2}} * (2 b)^{2}$
$R^{'} = k * 2 (a)^{\frac{1}{2}} * 4 (b)^{2}$
$R^{'} = 8 k * (a)^{\frac{1}{2}} * (b)^{2}$
$R^{'} = 8 * R$
The correct option is C

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The rate expression for reaction A(g)+B(g)⟶C(g) is rate =k[A]1/2[B]2. What change in rate if initial concentration of A and B increase by factor 4 and 2 respectively?

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The rate expression for reaction $A (g) + B (g) ⟶ C (g)$ is rate $= k {[A]}^{1 / 2} {[B]}^{2}$ . What change in rate if initial concentration of A and B increase by factor 4 and 2 respectively?