1.

Consider the following two first order reactions occurring at 298 K with same initial concentration of A:(1) A rarr B, rate constant, k = 0.693 min^(-1)(2) A rarr C, half-life, t_(1//2) = 0.693 minChoose the correct option.

Answer»

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 cannot be compared.

Solution : For reaction (1) : `ARARRB`,
rate constant `(k_1) = 0.693 min^(-1)`
For reaction (2), `ArarrC,`
rate constant `(K_2)=(0.693)/(t_(1//2)) implies (0.693)/(0.693)=1MIN^(-1)`
So,`k_1 LT k_2`
Hence,reaction (1) is slower than reaction (2).


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