This chemistry question involves key chemical concepts and calculations. The detailed solution below walks through each step, from identifying the reaction type to computing the final answer.
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3: 6.3.1 Between t_0 and t_1, the concentrations of the reactants decrease as they are consumed to form products. A decrease in reactant concentration leads to fewer effective collisions between reactant particles, thus decreasing the rate of the forward reaction. The concentration of reactants decreases. 6.3.2 At t_3, both the forward and reverse reaction rates increase instantaneously and equally, and the system immediately re-establishes equilibrium at a higher rate. This is characteristic of the addition of a catalyst. A catalyst was added. 6.3.3 At time t_2, the temperature of the system is increased. The graph shows that both forward and reverse reaction rates increase, but the reverse reaction rate increases more significantly than the forward reaction rate, causing the equilibrium to shift towards the reactants (left). According to Le Chatelier's principle, an increase in temperature favors the endothermic reaction. Since the reverse reaction is favored, the reverse reaction is endothermic. Therefore, the forward reaction must be exothermic. EXOTHERMIC 6.3.4 According to Le Chatelier's principle, when the temperature of a system at equilibrium is increased, the system will shift in the direction that absorbs heat (the endothermic direction) to counteract the change. At t_2, increasing the temperature caused the reverse reaction rate to increase more than the forward reaction rate, indicating a shift in equilibrium towards the reactants (left). This means the reverse reaction is endothermic, and consequently, the forward reaction is exothermic. Drop the next question.