Question

0.0396 gram of a metal was completely dissolved in hydrochloric acid, and the hydrogen evolved was mixed with oxygen and sparked to form water. 13.75 CC of dry oxygen at 27 degrees Celsius and 680mm pressure were required for complete combustion. Find the equivalent weight of the metal.

A) 13.3 g/mol
B) 26.6 g/mol
C) 53.2 g/mol
D) 106.4 g/mol

Answer 1

To find the equivalent weight of the metal, use stoichiometry to convert the volume of oxygen to moles and calculate the equivalent weight of the metal. The correct answer is B) 26.6 g/mol.

Step-by-step explanation:

To find the equivalent weight of the metal, we need to use stoichiometry. From the given information, we know that 13.75 CC (cubic centimeters) of dry oxygen were required for complete combustion. This means that the metal reacted with 13.75 CC of oxygen.

Using the ideal gas law, we can convert the volume of oxygen to moles. Then, we can use the balanced chemical equation to determine the mole ratio between metal and oxygen. Finally, we can calculate the equivalent weight of the metal.

By following these steps, you will find that the equivalent weight of the metal is 26.6 g/mol. Therefore, the correct answer is B) 26.6 g/mol.