Question

Determine the value of the rate constant for the elementary reaction: I₂ (g)+H₂ (g)→2HI (aq)Given that when [I₂] is 0.15 M and [H₂] is 0.2M, the rate of reaction is 0.005 M s⁻¹ at 298 K. *
(a) 1.06 M⁻¹s⁻¹
(b) 2.16 M⁻¹s⁻¹
(c) 3.16 M⁻¹s⁻¹
(d) 0.166 M⁻¹s⁻¹​

Answer 1

Answer:

The value of the rate constant for the elementary reaction: I₂ (g)+H₂ (g)→2HI (aq) is Option (d) 0.166 M⁻¹s⁻¹​

Explanation:

Given elementary reaction : I₂ (g)+H₂ (g)→2HI (aq)

Formula for rate of the reaction is Rate= K $[A]^{a} [B]^{b}$ , Where K is the Rate constant.

Therefore,

                       Rate= K $[A]^{a} [B]^{b}$

Substituting the values of A and B,

                      Rate= K $[I_{2}] ^{1} [H_{2}] ^{1}$

                      K = Rate / $[I_{2}] ^{1} [H_{2}] ^{1}$ ,

Where $[I_{2}] ^{1}$= 0.15M

           $[H_{2}] ^{1}$= 0.2M

    Rate of the reaction = 0.005 M s⁻¹

Substituting the above values in rate constant expression, we get,

Hence , K =    0.005 / (0.15)(0.2)

            K =    0.005 / 0.03

            K =    0.166 M⁻¹s⁻¹​        

Therefore, The value of the rate constant for the elementary reaction: I₂ (g)+H₂ (g)→2HI (aq) is Option (d) 0.166 M⁻¹s⁻¹​

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