Given the following data for the reaction A + B → products:| [A] (mol/L) | [B] (mol/L) | Initial Rate (mol/L·s) ||-------------|-------------|------------------------|| 0.10 | 0.10 | 0.020 || 0.20 | 0.10 | 0.040 || 0.10 | 0.20 | 0.040 |Assuming the rate law is rate = k[A][B], what is the value of the rate constant k (in L/mol·s)?

• A. 2.0
• B. 0.10
• C. 0.20
• D. 4.0

Answer: (A)

Verified step by step guidance

1. Write down the given rate law: \(\text{rate} = k [A][B]\), where \(k\) is the rate constant, and \([A]\) and \([B]\) are the concentrations of reactants A and B respectively.
2. Choose one set of data from the table to substitute into the rate law. For example, use \([A] = 0.10\ \text{mol/L}\), \([B] = 0.10\ \text{mol/L}\), and the initial rate \(= 0.020\ \text{mol/L·s}\).
3. Substitute the values into the rate law equation: \$0.020 = k \times 0.10 \times 0.10$.
4. Rearrange the equation to solve for \(k\): \(k = \frac{0.020}{0.10 \times 0.10}\).
5. Calculate the value of \(k\) using the above expression to find the rate constant in units of L/mol·s.