The second-order reaction 2 Mn(CO)₅ → Mn₂(CO)₁₀,has a rate constant equal to 3.0 × 10⁹ M^-1 s^-1 at 25°C.If the initial concentration of Mn(CO)₅ is 2.0 × 10^-5 M,how long will it take for 90.% of the reactant to disappear?

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The Answer of The second-order reaction 2 Mn(CO)₅ → Mn₂(CO)₁₀,has a rate constant equal to 3.0 × 10⁹ M^-1 s^-1 at 25°C.If the initial concentration of Mn(CO)₅ is 2.0 × 10^-5 M,how long will it take for 90.% of the reactant to disappear?

The Second-Order Reaction 2 Mn(CO)5 → Mn2(CO)10,has a Rate Constant

The Second-Order Reaction 2 Mn(CO)₅ → Mn₂(CO)₁₀,has a Rate Constant