Equivalent mass of a bivalent metal is 32.7. Molecular mass of its chloride is
(a) 68.2
(b) 103.7
(c) 136.4
(d) 4166.3

To determine the molecular mass of the chloride of the bivalent metal, we need to use the concept of equivalent mass and molecular mass.

Here's how you can solve the problem:

1. **Understand Equivalent Mass:**
The equivalent mass of a substance is the mass of the substance that reacts with or is equivalent to 1 gram of hydrogen or 8 grams of oxygen or 35.5 grams of chlorine. For a bivalent metal (a metal that forms ions with a charge of +2), the equivalent mass is the mass of the metal that combines with or displaces 1 mole of hydrogen.

For a bivalent metal (let’s call it M), its equivalent mass is given by:
\[
\text{Equivalent Mass of M} = \frac{\text{Molecular Mass of M}}{2}
\]

2. **Given Data:**
- Equivalent mass of the bivalent metal, M = 32.7

3. **Calculate Molecular Mass of the Metal:**
\[
\text{Molecular Mass of M} = 2 \times \text{Equivalent Mass of M}
\]
\[
\text{Molecular Mass of M} = 2 \times 32.7 = 65.4
\]

4. **Determine the Molecular Mass of the Chloride:**
The molecular formula of the chloride of a bivalent metal M would be \(MCl_2\). To find the molecular mass of \(MCl_2\), we add the molecular mass of the metal and twice the atomic mass of chlorine.

The atomic mass of chlorine (Cl) is approximately 35.5.

Molecular mass of \(MCl_2\):
\[
\text{Molecular Mass of } MCl_2 = \text{Molecular Mass of M} + 2 \times \text{Atomic Mass of Cl}
\]
\[
\text{Molecular Mass of } MCl_2 = 65.4 + 2 \times 35.5
\]
\[
\text{Molecular Mass of } MCl_2 = 65.4 + 71.0 = 136.4
\]

So, the molecular mass of the chloride of the bivalent metal is **136.4**.

**Answer: (c) 136.4**