The concentration for a zero-order reaction is given by the equation: [A]=-kt+[A]_(0) Where: [A]=concentration of reactantA [A]_(0)=initial concentration of reactantA k=rate constant t=time In order to solve for the rate constant,k, in two steps you must: Step One Add the same expression to each side of the equation to leave the term that includes the variable by itself on the right-hand side of the expression: (Be sure that the answer field changes from light yellow to dark yellow before releasing your answer.) underline ( )+[A]=underline ( )-kt+[A]_(0) Drag and drop your selection from the following list to complete the answer: -[A_(0)] [A_(0)] (1)/([A_(0)]) -(1)/([A_(0)])

To solve for the rate constant \( k \) in two steps, we need to isolate \( k \) on one side of the equation. Let's start with the given equation:<br /><br />\[ [A] = -kt + [A]_0 \]<br /><br />Step One:<br />Add \([A]_0\) to both sides of the equation to move the term that includes the variable \( [A] \) to the right-hand side:<br /><br />\[ [A] + [A]_0 = -kt + [A]_0 + [A]_0 \]<br /><br />Simplify the right-hand side:<br /><br />\[ [A] + [A]_0 = -kt + 2[A]_0 \]<br /><br />So the completed equation is:<br /><br />\[ [A] + [A]_0 = -kt + 2[A]_0 \]<br /><br />Now, we need to isolate \( k \). To do this, we will move the term \( 2[A]_0 \) to the left-hand side:<br /><br />\[ [A] + [A]_0 - 2[A]_0 = -kt \]<br /><br />Simplify the left-hand side:<br /><br />\[ [A] - [A]_0 = -kt \]<br /><br />Now, divide both sides by \(-t\) to solve for \( k \):<br /><br />\[ k = \frac{[A] - [A]_0}{-t} \]<br /><br />So, the correct selections to complete the answer are:<br /><br />\[ [A] + [A]_0 = -kt + 2[A]_0 \]<br /><br />And the final expression for \( k \) is:<br /><br />\[ k = \frac{[A] - [A]_0}{-t} \]