Half-life of first order reaction X Y + Z is 3 minutes. What is the time required to reduce the concentration of ^ X ^ by 90 % of it's initial concentration?

Step-by-step solution

(A) array l t _ 1 / 2 =3 ~min k = 0.693 t _ 1 / 2 = 0.693 3 =0.231 ~min ⁻¹ array array l [ A ]₀= Original amount of reactant =100 [ ~A ]_ t = Reactant remaining unreacted =100-90=10 array For first order reaction, t= 2.303 k ₁₀ [A]₀ [A]_ t = 2.303 0.231 ~min ⁻¹ ₁₀ 100 10 =9.969 ~min