A reaction is first order in A. If the rate constant of the reaction is 8.33 x10–3 s–1, what is the half-life (t1/2) of the reaction?

1. Reaction Kinetics and Dimensional Analysis (a) Consider an example first-order reaction of the nuclear decay of element A: A+B+C where B and C are the products of the decay. The reaction is said to be first-order because, at a given time, the rate at which the molar concentration of A, denoted as [A] (mol/L), decreases is proportional to the molar concentration of A at that time: d[A] dt = -k[A] Here, k, the proportionality constant, is known as the rate constant. Let time be measured in seconds. Determine the units for the rate constant k. b) The dissociation of hydrogen iodide (a.k.a., HI) is a second-order process, which means d[HI] dt = -k[HI]² Let time be measured in seconds. Determine the units for the rate constant k for this particul reaction.

0.1 M of a material has a decomposition rate constant (k) of 2.46×105 M-1 s-1. What equation would you use to calculate the half-life of decomposition?

She fills a reaction vessel with H2CO3 and measures its concentration as the reaction proceeds. Here's a graph of her data: (W) [200³H] 2 1.5- 0.5 0 0 t(s) Use this graph to answer the following questions: What is the half life of the reaction? Round your answer to 2 significant digits. Suppose the rate of the reaction is known to be first order in 11/2 = ☐ s S ☐ x10 H2CO3. Calculate the value of the rate constant k. k = ☐ Round your answer to 2 significant digits. Also be sure you include the correct unit symbol. Predict the concentration of H2CO3 in the engineer's reaction vessel after 5.0 seconds have passed. Assume no other reaction is important, and continue to assume the rate is first order in H2CO3. Round your answer to 2 significant digits. [H₂CO,] = M