A reaction is catalysed by H+ ion. In presence of HA, rate constant is 2×10−3min−1 and in presence of HB rate constant is 1×10−3min−1, HA and HB both being strong acids, we may conclude that:

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A reaction is catalysed by H^+ ion. In presence of HA, rate co

Question

A reaction is catalysed by $H^{+}$ ion. In presence of HA, rate constant is $2 \times 1 0^{- 3} mi n^{- 1}$ and in presence of HB rate constant is $1 \times 1 0^{- 3} mi n^{- 1}$ , HA and HB both being strong acids, we may conclude that:

equilibrium constant is 2.

HA is stronger acid than HB.

relative acidic strength of HA and HB is 2.

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

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Mateo Discussed

A reaction is catalysed by

H^{+}

ion. In presence of HA, rate constant is

2 \times 1 0^{- 3} mi n^{- 1}

and in presence of HB rate constant is

1 \times 1 0^{- 3} mi n^{- 1}

, HA and HB both being strong acids, we may conclude that:

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15 mins ago

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 1 0 ^{- 3}}{1 \times 1 0 ^{- 3}} = 2

Therefore options B and C are correct.

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Question Text	A reaction is catalysed by $H^{+}$ ion. In presence of HA, rate constant is $2 \times 1 0^{- 3} mi n^{- 1}$ and in presence of HB rate constant is $1 \times 1 0^{- 3} mi n^{- 1}$ , HA and HB both being strong acids, we may conclude that:
Answer Type	Text solution:1
Upvotes	150