If k = 0.3 1/Mxs and the concentration [A] = 0.035 M, what is the calculated rate for the reaction?

To calculate the rate of the reaction, we use the rate law formula. The rate of a reaction is often expressed in terms of the rate constant ( k ) and the concentration of the reactant ( [A] ). In this case, the relationship given by the rate law can be expressed as follows:

[

\text{Rate} = k \cdot [A]

]

Given that ( k = 0.3 , \text{1/Mxs} ) and ( [A] = 0.035 , \text{M} ), we can substitute these values into the equation:

[

\text{Rate} = 0.3 , \text{1/Mxs} \times 0.035 , \text{M}

]

Carrying out the multiplication:

[

\text{Rate} = 0.3 \times 0.035 = 0.0105 , \text{M/s}

]

However, we must account for the units of the rate constant and the concentration to find the rate in M/s correctly. Given that the rate law typically involves negative signs when the concentration of a reactant decreases (assuming a decrease in