the plot of concentration of the reactant versus time for a reaction is a straight line with a negative slope.The reaction follows a zero order or first order rate reaction? and why.please explain.
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Suppose we have to plot a graph of the reactant concentration versus time graph then we will use some simple formula already learnt in chemical kinetics that is
Rate = Reaction constant * [ Concentration ] ^ Order
Now,
If we put 0 as the order then the value of concentration will become 1 due to concentration^0 = 1
So, the rate will Become the constant value of reaction constant and hence the graph will be a straight line parallel to the x-axis
Suppose if we put order as 1
Then, the rate = constant * Concentration
which again is a constant value however changes proportionally to the value of concentration of the reactant and hence, this line when drawn on the graph will be x=y passing through the origin at time t=0
And thus having a slope of -1.
Hope this helps you and you've understood the concept
Rate = Reaction constant * [ Concentration ] ^ Order
Now,
If we put 0 as the order then the value of concentration will become 1 due to concentration^0 = 1
So, the rate will Become the constant value of reaction constant and hence the graph will be a straight line parallel to the x-axis
Suppose if we put order as 1
Then, the rate = constant * Concentration
which again is a constant value however changes proportionally to the value of concentration of the reactant and hence, this line when drawn on the graph will be x=y passing through the origin at time t=0
And thus having a slope of -1.
Hope this helps you and you've understood the concept
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