Consider the following two first order reactions occuring at 298 K with same initial concentration of A: (1) Aarrow B; rate constant, k = 0.693 min-1 (2)AarrowC;half - life, t½ = 0.693 min Choose the correct option :

Question

Consider the following two first order reactions occuring at 298 K with same initial concentration of A: (1) Aarrow B; rate constant, k = 0.693 min-1 (2)AarrowC;half - life, t½ = 0.693 min Choose the correct option : (A) Reaction (1) is faster than Reaction (2). (B) Reaction (1) is slower than Reaction (2). (C) Both reactions proceed at the same rate. (D) Since two different products are formed, rates can not be compared.

Tardigrade Admin · Accepted Answer

For reaction (1); k1= 0.693 min-1 For reaction (2); k2 =(0.693/0.693) =1min-1 Rate of reaction propto k

Q. Consider the following two first order reactions occuring at 298 K with same initial concentration of A:
(1) A $\to$ B; rate constant, k = 0.693 min $^{-} 1$
(2)A $\to$ C;half - life, t $_{½}$ = 0.693 min
Choose the correct option :

Reaction (1) is faster than Reaction (2).

Reaction (1) is slower than Reaction (2).

Both reactions proceed at the same rate.

Since two different products are formed, rates can not be compared.

$F orre a c t i o n (1); k_{1} = 0.693 mi n^{- 1}$
$F orre a c t i o n (2); k_{2} = \frac{0.693}{0.693} = 1 mi n^{- 1}$
$R a t eo f re a c t i o n \propto k$

Q. Consider the following two first order reactions occuring at 298 K with same initial concentration of A: (1) A→ B; rate constant, k = 0.693 min−1 (2)A→C;half - life, t½​ = 0.693 min Choose the correct option :