Rate constant k - 2 - 103 mol-1 L s-1 and Ea - 2-0 - 102 kJ mol-1- When T - -

The correct option is C A = 2.0 × 10^3 kJ mol^ 1 L s^ 1 Now here we are going to use #160;Arrhenius equation for the temperature dependence of a ...

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Standard XII

Chemistry

Arrhenius Equation

Rate constant...

Question

Rate constant $k = 2 \times 10^{3} m o l^{- 1} L s^{- 1} a n d E_{a} = 2.0 \times 10^{2} k J m o l^{- 1} . W h e n T \to \infty$

A = 2.0 \times 10^{2} k J m o l^{- 1}

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A = 2.0 \times 10^{3} k J m o l^{- 1} L s^{- 1}

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A = 2.0 \times 10^{3} k J m o l L^{- 1} s^{- 1}

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A = 2.0 \times 10^{3} k J m o l^{- 1} s^{- 1}

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Solution

The correct option is C $A = 2.0 \times 10^{3} k J m o l^{- 1} L s^{- 1}$
Now here we are going to use Arrhenius equation for the temperature dependence of a rate constant.
That is $K = A e^{- \frac{E q}{R T}}$
Now as $T$ will tend to infinity then $e^{- \frac{E q}{R T}}$ will tend to zero
so, we can say that $K$ will be almost equal to $A$ .
now matching the units of A accordingly and making $K \approx A$
we get,
$A = 2.0 \times 10^{3} k J m o l^{- 1} L s^{- 1}$

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Similar questions

Q. Rate constant

k = 2 \times 10^{3} m o l^{- 1} L s^{- 1} a n d E_{a} = 2.0 \times 10^{2} k J m o l^{- 1}

. What is the value of A when

T \to \infty

Q. For the reaction

2 A + B \to A_{2} B

rate

= k [A] [B]^{2}

with

k = 2.0 \times 10^{- 6} m o l^{- 2} L^{2} s^{- 1}

, what is the rate of the reaction when [A] is reduced to 0.060 molL^{-1} . the initial rate of reaction when

[A] = 0.1 m o l L^{- 1} a n d [B] = 0.2 m o l L^{- 1} i s 8 \times 10^{- 9} m o l L^{- 1} s^{- 1}

A hypothetical reaction : $A_{(g)} + B_{(g)} ⇌ C_{(g)} + D_{(g)}$ occurs in a single step, the specific rate constant of forward reaction at TK is $2.0 \times 10^{- 3} m o l^{- 1} L s^{- 1}$ . When start is made with equimolar amounts of A and B, it is found that the concentration of A is twice that of C at equilibrium. The specific rate constant of the backward reaction is ?

For the reaction:

$[C r (H_{2} O)_{6}]^{3 +} + [S C N^{⊖}] \to [C r 9 H_{2} O)_{5} N C S]^{2 +} H_{2} O$

The rate law is : $r = k [C r (H_{2} O)_{6}^{3 +} [S C N^{⊖}] .$

The value of k is $2.0 \times 10^{- 6} L m o l^{- 1} s^{- 1}$ at $14^{0}$ C and $2.2 \times 10^{- 5} L m o l^{- 1} s^{- 1}$ , at $30^{0}$ C

What is the value of $E_{a}$ ?

The following data pertains to reaction between A and B :
$\begin{matrix} S . N O . & [A] m o l L^{- 1} & m o l L^{- 1} & R a t e (m o l L^{- 1} t i m e^{- 1}) 1 & 1.0 \times 10^{- 2} & 2.0 \times 10^{- 2} & 2.0 \times 10^{4} 2 & 2.0 \times 10^{- 2} & 2.0 \times 10^{- 2} & 4.0 \times 10^{- 4} 3 & 2.0 \times 10^{- 2} & 4.0 \times 10^{- 2} & 8.0 \times 10^{- 4} \end{matrix}$
Which of the following inference(s) can be drawn from the above data ?

1. Rate constant of the reaction is $1.0 \times 10^{- 4}$

2. Rate law of the reaction is: rate $= k [A] [B]$

3. Rate of reaction increases four times on doubting the concentration of both the reactants.

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Rate constant k=2×103mol−1Ls−1andEa=2.0×102kJmol−1.WhenT→∞

Rate constant $k = 2 \times 10^{3} m o l^{- 1} L s^{- 1} a n d E_{a} = 2.0 \times 10^{2} k J m o l^{- 1} . W h e n T \to \infty$