sl showpage 307c6abssase presented the in material the 1-5: mirror reference ans

Question

sl showpage 307c6abssase presented the in material the 1-5: mirror reference answer questions always mee lab notebook feel conduet was of cRchandbook wrote to that violated. of carbonless the ased You for low You jot a yield. points of were the front of your standard watch to quickly see philosophy the Academic Code. N time your lose prepare you Given points the Honor save to totally 1. violate while you didn't to transferring CHM molar product Your The looking the some your displayed you experiment. following up was of balance outline 2. accidentally end studying general pobicy. You cited higher night the safety data. a you lab than work work. possible. safety sig At b in was up the a that and collects regarding whenever record (ua down mass the sentences raised used Mo. for your following are be each Fisher acid required containers and points these down completes directly is chemicals resource. of chloride. sashes 3. the that aocessed as yield sodium isolated Write of word be for organic ofthe on your must the height to a working and solubility use were to percent solvent. the The cal The data added the b To health suggest isolated. as c the calculations water the d. Approved following g were acid. The Naci using 4. To the experiment by benzole to of answer o 5 a the an the recovery the of lea) end Hoi percent (to the syllabus of Calculate course g g. 3.22 314L was

Explanation / Answer

NaHCO3 + HCl --> NaCl + H2CO3

Next, you have to figure out the limiting reagent. Since the problem tells you HCl is in excess, sodium bicarb is the limiting reagent. They tell you that you have 1.34 g of NaHCO3. You have to calculate the molar mass of NaHCO3 which is 84g/mol. You also have to calculate the molar mass of NaCl which is 58.44 g/mol. With this information, you can calculate the theoretical yield:

1.34g NaHCO3 x (1 mol NaHCO3/ 84g NaHCO3) x (mol NaCl/ mol NaHCO3) x (58.44 g NaCl / mol NaCl) = 0.34 g NaCl

As you can see, this is the theoretical yield. It's the ideal yield you would get if the reaction ran perfectly. But rarely do you get the full yield. You usually lose stuff from the reaction. The yield you get from the actual reaction is called the actual yield. Note that in this problem, they tell you that the actual yield is 0.434 g. To get the percent yield, you divide the actual yield by the theoretical yield and multiply by 100%, so in this case, the percent yield is:

(0.434 g / 2.14 g) x 100% =20.28%

Related Questions

Navigate

• Browse (All)
• Browse S
• Subjects

---

---

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.