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)`

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: \(I_{2}(g)+H_{2}(g)\rightarrow2HI(aq)\) 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.

A to B is a first order reaction with rate 6.6 xx 10^(-5) m-s^(-1) . When [A] is 0.6 m, rate constant of the reaction is……..

The emf of a cell corresponding to the reaction. Zn(s)+ 2H^(+)(aq)rightarrow Zn^(2+)(0.1M)+H_(2) (g,1atm) is 0.28 V at 25^(@) C . Calculate pH of the solution.

The rate constants of a reaction at 700 K and 760 K are 0.011" M"^(-1)s^(-1) and 0.105" M"^(-1)s^(-1) respectively. Calculate the values of Arrhenius parameters.

The potential of the cell for the reaction, M(s)+2H^(+) (1M)rightarrow H_(2) (g) (1atm)+M^(2+) (0.1m) ' is 1.500 V. The standard reduction potential for M^(2+) / M(s) couple is :

Define elementary reaction. For the reaction,\(A \rightarrow Products\), rate is \(1.25\times10^{-2}M/s\) when [A]=0.45M.Determine the rate constant if the reaction is.second order in A