CHEMISTRY COMMUNITY

How does the instantaneous rate react as the reaction proceeds?

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.

If you look at the curve graph for the concentration v. time, you can tell that the rate is very quick at first when the concentration is high and decreases as time increases.

The rate is high as the reaction begins because there are more reactants, as the concentration of reactants decreases, the rate decreases.

Instantaneous rate decreases as time increases

I believe instantaneous rate becomes 0 when the reaction reaches equilibrium

Instantaneous rate decreases as time increases and becomes 0 when equilibrium is reached

The instantaneous rate of change decreases as the reaction proceeds. The reaction gets closer to equilibrium and so the rate decreases.

The rate is very high when the reaction starts and decreases as the reaction continues. This can be determined by the slope of the tangent line at that point of the curve

Instantaneously was rate decreases with time. If you think about it, it makes sense that the reaction would slow as more of the reactants have been used up;.

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

Is there a case where the instantaneous rate increases with time?

The instantaneous rate should decrease with time.

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).

The instantaneous rate will decrease over time, as there becomes less reactants to be used up.

The instantaneous rate is equal to 0 when the reaction is at equilibrium at constant K. It is negative on the left side of K and it is positive on the right side of K, forming a U-shaped graph.

The rate is high as the reaction initially proceeds but as time goes on and the curve becomes flatter the rate decreases.

When considering that a reaction is beginning with a high concentration of reactants, the initial instantaneous rate will be very high as there are lots of reactants available; however, as the reaction continues as this high rate, the concentration of reactants will quickly decrease. With fewer reactants, the instantaneous rate will continually decrease with time until equilibrium is reached. At this point, the instantaneous rate will equal zero.

The instantaneous rate of reaction will decrease as the reaction proceeds given no reactant is added to the reaction

As time proceeds, the instantaneous rate will decrease. It approaches 0 as equilibrium is approached

The instantaneous rate is high at the beginning of a reaction because there are many reactants available. As the reaction proceeds, reactants are gradually depleted, so the instantaneous rate decreases. When the reaction ends/reaches equilibrium, the instantaneous rate will become 0.

I think it decreases as the reaction goes on and then approaches 0 at equilibrium.

As the reaction proceeds, the instantaneous rate will decrease. This is due to reactants being used up as the reaction proceeds, so the rate becomes slower as there are less reactants able to form products. Furthermore, if you look at a graph of concentration versus time, the slope of the tangent line at each instantaneous point will get less steep/closer to zero as time progresses.

As time goes on, the instantaneous rate decreases, until it approaches zero near equilibrium.

As time increases the instantaneous rate decreases.

The instantaneous rate decreases as the reaction proceeds since the more reactants are used up, the less is available to form products.

Instantaneous rate decreases as time goes and will approach 0 at equilibrium.

The instantaneous rate of the reactant eventually decreases to 0 as the time progresses for a reaction.

As the reaction tends towards equilibrium where the net rate of the reaction is 0, the instantaneous rate for the reactant will eventually decrease to 0.

Since there are more reactants when the reaction first begins, the reaction rate will be higher then but as the concentration of the reactants decreases as the reaction proceeds, the instantaneous rate will decrease as well.

As the reaction proceeds, the instantaneous rate decreases over time.

It starts off high as the concentration is the highest, then will decrease eventually to o.

It decreases as the reaction proceeds, because there will be fewer and fewer reactants that can bump into each other and react.

Instantaneous rate decreases as time increases and becomes 0 when equilibrium is reached.

As time increases, the instantaneous rate decreases

It will decrease as the reaction proceeds.

Average rate is simply an approximation of the change in concentration over a time interval. The instantaneous rate on the other hand is the slope of the tangent line at a specific time interval. It is like reading the speedometer of a car at a specific time.

Instantaenous rates will only be the rates for specific times. However for 0th order reactions, ALL instantaneous rates will be the same since the slope is a straight line.

The instantaneous rate decreases as the reaction proceeds--you can see this as the tangent line gets less steep as the time passes. hope this helps:)

The instantaneous rate decreases over time.

The instantaneous rate of the reactants decreases over time, no matter the order of the reaction, because reactants get used up over time and products are formed.

Instantaneous rate depends on what stage the reaction is in, but generally as time goes on, it ends up leveling out to zero once it reaches equilibrium.