For the reaction A arrow Products, it is found that the rate of reaction increases by a factor of 6.25 when concentration of A increases by a factor of 2.5. Calculate the order of reaction with respect to A

Question

For the reaction A arrow Products, it is found that the rate of reaction increases by a factor of 6.25 when concentration of A increases by a factor of 2.5. Calculate the order of reaction with respect to A (A)  (B)  (C)  (D)

Tardigrade Admin · Accepted Answer

Rate (r)=k[ A ]n=k( X )n ldots( i ) 6.25 × r=k(2.5 X )n ldots( ii ) Or 6.25 × k ×( X )n=k(2.5 × X )n ⇒((2.5 X/X))n=6.25 ⇒(2.5)n=(2.5)2 ∴ n=2

Q. For the reaction $A \to$ Products, it is found that the rate of reaction increases by a factor of $6.25$ when concentration of A increases by a factor of $2.5$ . Calculate the order of reaction with respect to A

Rate $(r) = k [A]^{n} = k (X)^{n} \dots (i)$
$6.25 \times r = k (2.5 X)^{n} \dots (ii)$
Or $6.25 \times k \times (X)^{n} = k (2.5 \times X)^{n}$
$\Rightarrow (\frac{2.5 X}{X})^{n} = 6.25 \Rightarrow (2.5)^{n} = (2.5)^{2}$
$∴ n = 2$

Q. For the reaction A→ Products, it is found that the rate of reaction increases by a factor of 6.25 when concentration of A increases by a factor of 2.5. Calculate the order of reaction with respect to A

Rate (r)=k[A]n=k(X)n…(i) 6.25×r=k(2.5X)n…(ii) Or 6.25×k×(X)n=k(2.5×X)n ⇒(X2.5X​)n=6.25⇒(2.5)n=(2.5)2 ∴n=2

Q. For the reaction $A \to$ Products, it is found that the rate of reaction increases by a factor of $6.25$ when concentration of A increases by a factor of $2.5$ . Calculate the order of reaction with respect to A

Rate $(r) = k [A]^{n} = k (X)^{n} \dots (i)$
$6.25 \times r = k (2.5 X)^{n} \dots (ii)$
Or $6.25 \times k \times (X)^{n} = k (2.5 \times X)^{n}$
$\Rightarrow (\frac{2.5 X}{X})^{n} = 6.25 \Rightarrow (2.5)^{n} = (2.5)^{2}$
$∴ n = 2$