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Factors Affecting Alpha

A reaction is...

Question

A reaction is catalysed by $H^{+}$ ion. In presence of HA, rate constant is $2 \times 10^{- 3} m i n^{- 1}$ and in presence of HB rate constant is $1 \times 10^{- 3} m i n^{- 1}$ , HA and HB both being strong acids, we may conclude that:

A

equilibrium constant is 2.

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B

HA is stronger acid than HB.

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C

relative acidic strength of HA and HB is 2.

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D

HA is weaker acid than HB and relative strength is 0.5.

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Solution

The correct options are
B HA is stronger acid than HB.
C relative acidic strength of HA and HB is 2.
Rate $=$ k [reactant] [HA or HB].
Rate is more with HA so it is stronger than HB.
Relative strength of HA and HB $= \frac{2 \times 10^{- 3}}{1 \times 10^{- 3}} = 2$ .
Therefore options B and C are correct.

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