Determine the value of the rate constant for the elementary reaction: \(I_{2}(g)+H_{2}(g)\rightarrow2HI(aq)\) Given that when \(I_{2}\) is "0.15M" and \(H_{2}\) is "0.2M",the rate of reaction is 0.005M\(s^{-1}\) at 298K.

Determine the value of the rate constant for the elementary reaction: I_(2)(g)+H_(2) (g) rarr 2 Hl (aq) Given that when [ I_(2) ] is 0.15 M and [ H_(2) ] is 0.2M ,the rate of reaction is 0.005M s^(-1) at 298K . (a) 1.06 M^(-1)s^(-1) (b) 2.16 M^(-1)s^(-1) (c) 3.16 M^(-1)s^(-1) (d) 0.166M^(-1)s^(-1)

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) 1.06M^(-1)s^(-1) (b) 2.16M^(-1)s^(-1) (c) 3.16M^(-1)s^(-1) (d) 0.166M^(-1)s^(-1)

The equilibrium constant K_(p) for the reaction H_(2)(g)+I_(2)(g) hArr 2HI(g) changes if:

Rate constant for a reaction H_(2) + I_(2) rarr 2HI is 49 , then rate constant for reaction 2HI rarr H_(2) + I_(2) is

Which of the following will not affect the value of equilibrium constant of the reaction H_(2)(g) +I_(2) hArr 2HI(g)

Suppose the value of the equilibrium constant for the given reaction H_2(g) + I_(2)(g) hArr 2HI(g) at 717 K is 64, then calculate the same (eq. const.) for the reaction HI hArr 1/2 H_2 + 1/2 I_2 .