Two elements `A` and `B` form compounds having molecular formula `AB_(2)` and `AB_(4)`. When dissolved in `20 g` of benzene, `1 g`of `AB_(2)` lowers the freezing point by `2.3 K`, whereas `1.0 g` of `AB_(4)` lowers it by `1.3 K`. The molar depression constant for benzene is `5.1 K kg mol^(-1)`. Calculate the atomic mass of `A` and `B`.

Explanation

To solve the problem, we need to calculate the atomic masses of elements A and B based on the information provided about their compounds AB₂ and AB₄. We will use the freezing point depression formula and the data given in the question.

### Step-by-Step Solution:

1. **Understand the Freezing Point Depression Formula**:
The freezing point depression (\( \Delta T_f \)) is given by the formula:
\[
\Delta T_f = K_f \cdot m
...