A particular chemical reaction that produces hydrogen gas as a byproduct has an activation energy of 19.2 $\times$ 10^-20 J.If the reaction produces 0.15 $\times$ 10^-3 mol H₂/hr at room temperature (20$^{\circ}$C),what is the rate of production of H₂ at 52$^{\circ}$C by means of this reaction?

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The rate of a reaction increases with increasing temperature. The Arrhenius equation can be used to calculate the rate constant at a different temperature. The equation is:k = Ae^(-Ea/RT)where:k is the rate constantA is the pre-exponential factorEa is the activation energyR is the gas constantT is the temperature in KelvinIn this problem, we are given the activation energy (Ea), the rate constant at room temperature (k1), and the temperature at which we want to calculate the rate constant (T2). We can use the Arrhenius equation to solve for k2:k2 = k1 * e^(-Ea/R * (1/T2 - 1/T1))Plugging in the values we know:k2 = (0.15 x 10^-3 mol H2/hr) * e^(-19.2 x 10^-20 J/R * (1/(52 + 273 K) - 1/(20 + 273 K)))k2 = 0.16 x 10^-2 mol H2/hrTherefore, the rate of production of H2 at 52oC by means of this reaction is 0.16 x 10^-2 mol H2/hr.

A Particular Chemical Reaction That Produces Hydrogen Gas as a Byproduct