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The half-life of the chemical reaction, A → Product, for initial reactant concentrations of 0.1 and 0.4 mol L–1 are 200 and 50 s, respectively. The order of the reaction is
  • a)
    0
  • b)
    1
  • c)
    2
  • d)
    3
Correct answer is option 'C'. Can you explain this answer?
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For 2nd order  T1/2=1/Ao.k 
                      k=1/T1/2.Ao=const
               put all values and check
k1=1/ 0.1*200=1/20
k2=1/0.4*50=1/20
                   both values are const in 2nd order reaction so correct option is c
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The half-life of the chemical reaction, A →Product, for initial reactant concentrations of 0.1 and 0.4 mol L–1 are 200 and 50 s, respectively. The order of the reaction isa)0b)1c)2d)3Correct answer is option 'C'. Can you explain this answer?
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