For a zero-order reaction, the plot of concentration vs time...

For a zero-order reaction, the plot of concentration vs time is linear with
(a) +ve slope and zero intercept
(b) -ve slope and zero intercept
(c) tve slope and non-zero intercept
(d) -ve slope and non-zero intercept

Key Concepts

Zero-Order Reaction

A zero-order reaction is one in which the rate of reaction is independent of the concentration of the reactant. This implies that the reaction proceeds at a constant rate over time until the reactant is exhausted.

Integrated Rate Law

For a zero-order reaction, the integrated rate law is expressed as [A] = [A]? - kt. In this equation, [A] is the reactant concentration at time t, [A]? is the initial concentration, and k is the rate constant. This relation shows that the concentration decreases linearly with time.

Graphical Analysis of Reaction Kinetics

Plotting the concentration versus time for a zero-order reaction results in a straight line with a negative slope, which is indicative of the constant rate of consumption of the reactant. The y-intercept of this line is the initial concentration ([A]?), confirming that the curve starts at the initial concentration and decreases uniformly over time.

Transcript

00:01 In this question we need to comment on the zero order reaction right so for zero order reaction or a reaction with zero order it has been given that the plot of concentration versus time is linear right the concentration obviously concentration of reactant right so concentration of reactant versus time plot is going to be linear right but we need to know whether it is having a positive slope or negative slope and also whether it has a non -zero intercept or a zero intercept right so in case of zero of reaction we can say that the rate is going to be equal to k multiplied by the concentration of reactant concentration of reactant right because the order is zero now again this becomes rate equals to k now when we take rate as the change in concentration with respect to change in time we can take d x equals to d t which is again going to be equal to k now this assumption has been made for a reaction for a reaction let us say from a reactant we are getting b product right so initially or we can say at time equals to zero the concentration of a was the concentration of this a reactant was small a while the concentration of product b was zero while after some time in double t2 which is of t seconds we can say that out of this a concentration of we can say x has been converted into product b right now the remaining concentration of the reactant a would be a minus x so this is our assumption here now we are taking the fact that the change in concentration of product is also a rate right so now we can say that we can just transfer d t to the right hand side like this and then we can integrate this expression on both sides now this leaves us with the integral equation for the zero order reaction which is x equals to k t right now let us just name it as equation number one so this is the integral equation for the zero order reaction now what we need to do is we just need to simply find out what is going to be but now since we have this expression…

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