For a reaction: AB arrow A+B, rate=k[AB]^2and k=0.2L/mol.s
a)how long it will take for [AB] to reach its initial concentration of 1.5M
To find out how long it will take for [AB] to reach its initial concentration of 1.5 M, we need to use the given rate equation and the value of the rate constant (k).
The rate equation is given as: rate = k[AB]^2
First, we need to rearrange the rate equation to solve for time (t), since we are trying to find the time it takes for [AB] to reach 1.5 M. Rearranging the equation gives:
t = 1 / (k[AB]^2)
Now, substitute the given values into the equation:
k = 0.2 L/mol.s
[AB] = 1.5 M
t = 1 / (0.2 L/mol.s * (1.5 M)^2)
Next, calculate the value inside the parenthesis:
(1.5 M)^2 = 2.25 M^2
Now, substitute the calculated value back into the equation:
t = 1 / (0.2 L/mol.s * 2.25 M^2)
Finally, solve for time (t) using the appropriate units:
t = 1 / (0.2 L/mol.s * 2.25 M^2)
t = 1 / (0.9 L/mol.s.M^2)
t ≈ 1.11 seconds
Therefore, it will take approximately 1.11 seconds for [AB] to reach its initial concentration of 1.5 M.