For a given reaction the concentration of the reactant plotted against time gave a straight line with negative slope. The order of the reaction is-
A
3
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B
0
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C
1
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D
2
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Solution
The correct option is B0 Rate law for zero order is: [A]−[A0]=−kt
i.e. [A]=[A0]−kt...(i)
On comparing eq (i) with straight line equation i.e. y = mx + c,
we get, slope = -k and intercept = [A0]
Hence, for zero order, graph is straight line with negative slope.