H 2 g - Cl 2 g - 2 HCl g - rate - r 1 - D 2 g - Cl 2 g - 2 DCl g - rate - r 2 - r 1- r 2- Then the correct statement among the following isA- H - H and D - D bond length are sameB- H - H has greater bond energy than D - DC- The activation energy for the first reaction is greater than that of second reactionD- The activation energy for the first reaction is less than that of second reaction

The rate constant is numerically the same for three reaction of first, second and third order respectively. Which one is true for rate of three reaction, if concentration of reactant is greater than 1M?

(1) r₁= r₂ = r₃

(2) r₁> r₂> r₃

(3) r₁< r₂< r₃

(4) All of these

Q. At a certain temperature, the first order rate constant

k_{1}

is found to be smaller than the second order rate constant

k_{2}

. If the energy of activation

E_{1}

of the first order reaction is greater than energy of activation

E_{2}

of the second order reaction, then with increase in temperature:

Q. For an endothermic reaction, where

Δ H

represents the enthalpy of the reaction in

kJ/mol

, the minimum value for the energy of activation will be:

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H2(g) +Cl2(g) → 2HCl(g) ... rate = r1 ; D2(g) +Cl2(g) → 2DCl(g)... rate = r2 ; r1 = r2. Then the correct statement among the following is

The correct option is C The activation energy for the first reaction is less than that of second reaction D2 is less reactive than H2

$H_{2}$ $_{(g)}$ + ${C l}_{2}$ $_{(g)}$ $\to$ 2HCl $_{(g)}$ ... rate = $r_{1}$ ; $D_{2}$ $_{(g)}$ + ${C l}_{2}$ $_{(g)}$ $\to$ 2DCl $_{(g)}$ ... rate = $r_{2}$ ; $r_{1}$ = $r_{2}$ . Then the correct statement among the following is

The correct option is C
The activation energy for the first reaction is less than that of second reaction

$D_{2}$ is less reactive than $H_{2}$