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The instantaneous rate decreases as the reaction proceeds because the reactants are consumed and less amount of reactant is left in the reaction which causes the rate of the reaction to decrease since the number of collisions between the reactants decreases and the change in the reactant concentration becomes less which causes the tangent to the plot of its concentration against time to become less steep as the reaction proceeds since the rate has decreased and the plot started to approach a straight vertical line as the reactant concentrations remain unchanged at equilibrium.
looking at it graphically, the curve downwards will make the line tangent to the curve less and less steep. since the instantaneous rate is dependent on the slope of the tangent line, it will decrease over time. hope this helps
As the reaction proceeds, think of it as a curved graph (seen with the equilibrium reaction graph, with E), the initial rate is very high as there is a readily amount of reactant available to react, and as its used up less reactant is available, so the reaction rate goes down (as reaction rate depends on concentration of reactants), eventually it will level out when all the products are formed (curved graph situation).
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