The effect of temperature on the rate of a catalytic reaction between hydrogen gas and iodine gas in the presence of a solid catalyst can be explained using the collision theory and the Arrhenius equation. The reaction between hydrogen and iodine gas is as follows:H2 g + I2 g 2HI g In the presence of a solid catalyst, the reaction rate is increased due to the catalyst providing an alternative reaction pathway with a lower activation energy. The catalyst does not get consumed in the reaction and remains unchanged after the reaction is complete.According to the collision theory, the rate of a reaction depends on the frequency of effective collisions between reactant molecules. When the temperature is increased, the kinetic energy of the molecules also increases, leading to a higher frequency of collisions between the reactant molecules. This results in an increased reaction rate.The Arrhenius equation further explains the relationship between temperature and reaction rate:k = Ae^-Ea/RT where k is the rate constant, A is the pre-exponential factor, Ea is the activation energy, R is the gas constant, and T is the temperature in Kelvin.As the temperature T increases, the exponential term e^-Ea/RT becomes larger, leading to an increase in the rate constant k . This means that the reaction rate will increase with increasing temperature.In summary, increasing the temperature will increase the rate of a catalytic reaction between hydrogen gas and iodine gas in the presence of a solid catalyst. This is due to the increased frequency of effective collisions between reactant molecules and the lower activation energy provided by the catalyst.