The second order reaction A Products takes 13.5 s for the concentration of A to decrease from 0.740 M to 0.205 M. What is the value of k for this reaction?

The second order reaction A → Products takes 13.5 s for the concentration of A to decrease from 0.740 M to 0.213 M. What is the value of k for this reaction?

k=? k=?

What is the concentration of A after 37.5 minutes for the reaction A → Products when the initial concentration of A is 0.750 M? (k = 0.0451 M⁻¹min⁻¹)

How do I calculate k when [X]= .42 M and the rate of reaction is .0030 M/s. I can't remember exactly how to do this type of problem. Thank you for the help !

Consider the quilibrium reaction between X and Y, as shown below: X=Y AG The reaction is started with 10 mmol of X; no Y is initially present. After 48 hours, analysis reveals the presence of 10 mmol of X and 0 mmol of Y. Which is the most likely explanation? = −1 - 45 kJ mol X and Y have reached equilibrium concentrations. An enzyme has shifted the equilibrium toward X. Formation of Y is kinetically slow; equilibrium has not been reached by 48 hours. Formation of Y is thermodynamically unfavorable. Two of the above explanations are reasonable.

What is the concentration of A after 30.5 minutes for the reaction A → Products when the initial concentration of A is 0.750 M? (k = 0.0451 M⁻¹min⁻¹)

The second order reaction A → Products takes 13.5 s for the concentration of A to decrease from 0.740 M to 0.205 M. What is the value of k for this reaction?