The ionization constant of  NH4+   in water is    5.6 × 10−10  at  25oC  . The rate constant for the reaction of  NH4+  and  OH−   to form   NH3 and  H2O   at  3.4 × 1010Lmol−1s−1  . The rate constant for proton transfer from water to  NH3   is

A chemistry graduate student is studying the rate of this reaction:→NH4OHaq+NH3aqH2OaqShe fills a reaction vessel with NH4OH and measures its concentration as the reaction proceeds:time(seconds) NH4OH0 0.400M1.0 0.277M2.0 0.191M3.0 0.132M4.0 0.0915MUse this data to answer the following questions.Write the rate law for this reaction. rate=k  Calculate the value of the rate constant k.Round your answer to 2 significant digits. Also be sure your answer has the correct unit symbol.

At a certain temperature this reaction follows second-order kinetics with a rate constant of ·0.0577M−1s−1:→NH4OHaq+NH3aqH2OaqSuppose a vessel contains NH4OH at a concentration of 1.16M. Calculate the concentration of NH4OH in the vessel 53.0 seconds later. You may assume no other reaction is important.Round your answer to 2 significant digits.M

Ammonia is commonly produced via the Haber-Bosch process, which proceeds via the following equilibrium:𝑁2+3𝐻2⇌2𝑁𝐻3The reaction has reached equilibrium. The concentration of nitrogen is 1.41 M, The concentration of hydrogen is 2.43 M and the concentration of ammonia is 4.67 M. What is the value of the equilibrium constant, Kc to 2 decimal places?

Using the equilibrium constant expression given below,=KeqNH32N2H23and the equilibrium constant, =Keq0.575, determine the equilibrium concentration of NH3 if the concentration of N2 is ×4.310−2M, and the concentration of H2 is ×6.810−3M. Round your answer to 2 significant figures.

NH3    +    H2O    -->    OH-    +    NH4+