The table above gives the initial concentrations and rate for three experiments involving the decomposition of urea, $\ce{CN2H4O}$. The reaction is $\ce{H+}(aq)+\ce{2 H2O(l)}+\ce{CN2H4O}(aq)\rightarrow \ce{2 NH4+}(aq)+\ce{HCO3-}(aq)$. What is the rate law for this reaction?
A.
Rate = $k[\ce{CN2H4O}]$
B.
Rate = $k[\ce{CN2H4O}]^2[\ce{H+}]^2$
C.
Rate = $k[\ce{H+}]$
D.
Rate = $k[\ce{CN2H4O}]^2[\ce{H+}]$
Exam No：AP Chemistry Problem Set 6 Year：2024 Question No：APChemistry2024AP0291
Answer:
A
Knowledge points:
4.5 Stoichiometry
Solution:
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