Question

HEY!!! I NEED SOME HELP<3A chemist reacted 57.50 grams of sodium metal with an excess amount of chlorine gas. The chemical reaction that occurred is shown.Na + Cl2 → NaClIf the percentage yield of the reaction is 86%, what is the actual yield? Show your work, including the use of stoichiometric calculations and conversion factors.

Answer 1

The actual yield is 125.646 grams

Explanation

Given information

The mass of sodium in grams = 57.50 grams

The percentage yield = 86%

The next step is to write the balanced equation of the reaction

`2Na_((s))+Cl_(2(g))\text{ }\rightarrow2NaCl_((aq))`

From the above reaction, we can see that 2 moles of sodium react with 1 mole of chloride too give moles of sodium chloride

The next step is to find the number of moles sodium using the below formula

`\text{mole = }\frac{\text{ mass}}{\text{ molar mass}}`

According to the periodic table, the molar mass of sodium is 23 g/mol

`\begin{gathered} \text{mole = }(57.50)/(23) \\ \text{mole = }2.5\text{ moles} \end{gathered}`

The next step is to find the number of moles of sodium chloride using a stoichiometry ratio

From the above reaction, you can see that 2 moles of sodium react to give 2 moles of sodium chloride

Let x represents the number of moles of sodium chloride

`\begin{gathered} 2\text{ moles }\rightarrow\text{ 2 moles} \\ 2.5\text{ moles }\rightarrow\text{ x moles} \\ \text{cross multiply} \\ 2\text{ }*\text{ x = 2 }*\text{ 2.5} \\ 2x\text{ = 5} \\ \text{Divide both sides by 2} \\ \frac{\cancel{2}x}{\cancel{2}}\text{ = }(5)/(2) \\ x\text{ = 2.5 moles} \end{gathered}`

Therefore, the number of moles of NaCl is 2.5 moles

The next step is to find the theoretical yield using the below formula

`\text{mole = }\frac{\text{ mass}}{\text{ molar mass}}`

According to the periodic table, the molar mass of NaCl is 58.44 g/mol

`\begin{gathered} 2.5\text{ = }(mass)/(58.44) \\ \text{cross multiply} \\ \text{mass = 2.5 }*\text{ 58.44} \\ \text{mass = 146.1 grams} \end{gathered}`

Since the theoretical yield is 146.1 grams, then we can now find the actual yield using the below formula

`\begin{gathered} \text{Percentage yield =}\frac{actual\text{ yield}}{\text{theoretical yield}} \\ \end{gathered}`

Recall that, the percentage yield is86%

`\begin{gathered} (86)/(100)\text{ = }\frac{actual\text{ yield}}{146.1} \\ 0.86\text{ = }\frac{actual\text{ yield}}{146.1} \\ \text{cross multiply} \\ \text{actual yield = 0.86 }*\text{ 146.1} \\ \text{actual yield = 125.646 grams} \end{gathered}`

Therefore, the actual yield is 125.646 grams