The temperature affects the rate of a gas phase reaction between hydrogen gas and iodine gas through the collision theory and the Arrhenius equation. According to the collision theory, the rate of a reaction depends on the number of effective collisions between reactant molecules per unit time. As the temperature increases, the kinetic energy of the molecules also increases, leading to more frequent and energetic collisions. This results in a higher probability of successful collisions with enough energy to overcome the activation energy barrier, thus increasing the reaction rate.The relationship between temperature and the rate constant of a reaction can be described by the Arrhenius equation:k = Ae^-Ea/RT where:- k is the rate constant- A is the pre-exponential factor also called the frequency factor , which represents the rate constant when there is no activation energy barrier- Ea is the activation energy of the reaction- R is the gas constant 8.314 J/molK - T is the temperature in KelvinThe Arrhenius equation shows that the rate constant k increases exponentially with temperature. To develop a kinetic model for the reaction between hydrogen gas and iodine gas, we can use the Arrhenius equation to relate the rate constant to temperature.For the forward reaction H2 g + I2 g 2HI g , we can write the rate law as:Rate = k[H2][I2]For the reverse reaction 2HI g H2 g + I2 g , we can write the rate law as:Rate = k[HI]^2At equilibrium, the forward and reverse reaction rates are equal:Rate = Ratek[H2][I2] = k[HI]^2To find the relationship between temperature and the rate constants k and k, we can use the Arrhenius equation for each rate constant:k = Ae^-Ea/RT k = Ae^-Ea/RT By substituting these expressions into the equilibrium rate equation, we can develop a kinetic model that explains the relationship between temperature and the rate constant of the reaction between hydrogen gas and iodine gas.