If the reaction of 5.75 moles of sodium with excess hydrofluoric acid produced an 86.5% yield of hydrogen gas, what was the actual yield of hydrogen gas?

The actual yield of hydrogen gas in the following reaction is 4.974 grams.

Explanation:

The chemical equation for the reaction of sodium and hydrofluoric acid follows:

As, hydrofluoric acid is present in excess. So, it is considered as an excess reagent and sodium is considered as a limiting reagent because it limits the formation of products.

By Stoichiometry of the reaction:

2 moles of sodium is producing 1 mole of hydrogen gas.

So, 5.75 moles of sodium will produce = of hydrogen gas.

To calculate the actual yield of hydrogen gas, we use the equation:

% yield of reaction = 86.5 %

Theoretical yield of hydrogen gas = 2.875 moles

Putting values in above equation, we get:

Now, to calculate the mass of hydrogen gas, we use the equation:

Moles of hydrogen gas = 2.487 mol

Molar mass of hydrogen gas = 2g

Putting values in above equation, we get:

Hence, the actual yield of hydrogen gas in the following reaction is 4.974 grams.

b. atoms in metallic solids are not arranged in a regular pattern

explanation: