For the reaction A $\rightarrow$ products, the following data were collected. $$\begin{array} { | l | l | l | l | l | l | }
\hline \text { time,s } & 0 & 1.00 & 2.00 & 3.00 & 4.00 \
\hline [ A ] \mathrm { A } , \mathrm { M } & 1.00 & 0.430 & 0.270 & 0.200 & 0.160 \
\hline
\end{array}$$
The half-life for this reaction is
A) 0.521 s
B) 0.752 s
C) 0.922 s
D) 1.08 s

Question

For the reaction A $\rightarrow$ products, the following data were collected. $$\begin{array} { | l | l | l | l | l | l | } 
\hline \text { time,s } & 0 & 1.00 & 2.00 & 3.00 & 4.00 \
\hline [ A ] \mathrm { A } , \mathrm { M } & 1.00 & 0.430 & 0.270 & 0.200 & 0.160 \
\hline
\end{array}$$
The half-life for this reaction is
A) 0.521 s
B) 0.752 s
C) 0.922 s
D) 1.08 s

Quizplus · Accepted Answer

The half-life of a reaction is the time it takes for the concentration of a reactant to decrease to half of its initial value. From the given data, the concentration of A starts at 1.00 M and decreases to 0.5 M. By examining the data, we can interpolate that the concentration reaches approximately 0.5 M between 1.00 s and 2.00 s. Since the concentration at 1.00 s is 0.430 M and at 2.00 s is 0.270 M, the half-life is closer to 1.00 s but less than 2.00 s. Without exact interpolation or calculation, the closest value given in the options that fits this description is 0.752 s.

For the Reaction A →\rightarrow→ Products, the Following Data Were Collected

For the Reaction A $\rightarrow$ Products, the Following Data Were Collected