Final answer:
The reaction rate increases with temperature, and using the Arrhenius equation and the given activation energy, one can calculate how much faster a reaction occurs at 343K than at 320K.
Step-by-step explanation:
The rate at which a chemical reaction proceeds can be affected significantly by changes in temperature, as described by the Arrhenius equation: k = Ae-Ea/RT. Here, the activation energy (Ea) is the minimum amount of energy required for a reaction to occur, while A is the frequency factor, and R is the ideal gas constant. To calculate how much faster a reaction at 343K is compared to 320K, we use the given activation energy (42.2 kJ/mol, which is 42200 J/mol), and the value for R (8.314 J/mol/K).
Applying the Arrhenius equation to both temperatures and taking the ratio of the rate constants, we can find the relative increase in the reaction rate. The final result shows that a reaction is indeed faster at a higher temperature, in this case, 343K compared to 320K.