Question: At a certain temperature this reaction follows second-order kinetics with a rate constant of 23.M1 ' s1 : 2H3PO4(aq)P2O5(aq)+3H2O(aq) Suppose a vessel contains H3PO4 at

At a certain temperature this reaction follows second-order kinetics with a rate constant of 23.M1 ' s1 : 2H3PO4(aq)P2O5(aq)+3H2O(aq) Suppose a vessel contains H3PO4 at a concentration of 1.00M. Calculate how long it takes for the concentration of H3PO4 to decrease to 6.0% of its initial value. You may assume no other reaction is important. Round your answer to 2 significant digits

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