Question

A chemist reacted 57.50 grams of sodium metal with an excess amount of chlorine gas. The chemical reaction that occurred is shown.

2Na + Cl2 - 2Naci

If the actual yield of the reaction is 125.7 g of NaCl, what is the percent yield? Show your work, including the use of stoichiometric calculations and conversion factors.

Answer 1

The percent yield of the reaction is 215%.

Step-by-step explanation:

To determine the percent yield, we compare the actual yield (125.7 g) to the theoretical yield. Theoretical yield can be calculated using stoichiometric calculations. From the balanced equation, we can see that 2 moles of Na react to form 2 moles of NaCl. Calculate the molar mass of NaCl: Na: 22.99 amu and Cl: 35.45 amu. The mass of 2 moles of NaCl is 58.44 g.

Now, calculate the percent yield:

Percent yield = (actual yield / theoretical yield) x 100

Plugging in the values, we get: (125.7 g / 58.44 g) x 100 = 215%.