Record and calculate the following masses:
(a)mass of empty beaker: 47.420g
(b)mass of beaker plus Na₂CO₃:47.920g
(c)Mass of Na₂CO₃:0.5g
(d)mass of beaker plus NaCl:47.438g
(e) Mass of NaCl (g):0.018g
**I need help with these questions below**
2. Convert the masses of Na₂CO₃ and NaCl to moles, given their molecular weights (MW) of Na₂CO₃ = 105.989 g/mole, MW of NaCl = 58.443 g/mole.
3. Calculate the experimentally determined ratio of moles of NaCl produced to moles of Na₂CO₃ reacted, according to:
mole-ratio = (moles NaCl)/(moles Na₂CO₃)
5. Use the mole ratio to write a balanced chemical equation for the reaction.
6. What is the theoretical mole ratio according to this balanced equation?
7. Use the theoretical mole ratio to calculate the theoretical yield of NaCl in grams from .5g of Na₂CO₃?
8. The "percent yield" is the ratio of the actual amount of a product to the theoretical amount. Calculate the percent yield of NaCl as:
% yield = (experimental grams NaCl) / (theoretical grams NaCl) * 100%
9. What sources of error may have reduced your yield?
2. Convert the masses of Na₂CO₃ and NaCl to moles, given their molecular weights (MW) of Na₂CO₃ = 105.989 g/mole, MW of NaCl = 58.443 g/mole.
mols = grams/molar mass
3. Calculate the experimentally determined ratio of moles of NaCl produced to moles of Na₂CO₃ reacted, according to:
mole-ratio = (moles NaCl)/(moles Na₂CO₃)
Use the moles from the previous question for these ratios as the procedure tells you.
5. Use the mole ratio to write a balanced chemical equation for the reaction.
I don't know what equation you had so you're on your own here
6. What is the theoretical mole ratio according to this balanced equation?
Use the coefficients in the balanced equation for the ratios
7. Use the theoretical mole ratio to calculate the theoretical yield of NaCl in grams from .5g of Na₂CO₃?
This is a regular stoichiometry problem.
8. The "percent yield" is the ratio of the actual amount of a product to the theoretical amount. Calculate the percent yield of NaCl as:
% yield = (experimental grams NaCl) / (theoretical grams NaCl) * 100%
Just follow the directions.
9. What sources of error may have reduced your yield?
You must do this from your observations
To answer the questions, follow these steps:
2. Convert the masses of Na₂CO₃ and NaCl to moles using their molecular weights:
- Moles Na₂CO₃ = Mass Na₂CO₃ / MW Na₂CO₃
- Moles NaCl = Mass NaCl / MW NaCl
For example, to calculate moles of Na₂CO₃:
- Moles Na₂CO₃ = 0.5g / 105.989 g/mole
3. Calculate the experimentally determined mole ratio of NaCl to Na₂CO₃:
- Mole ratio = Moles NaCl / Moles Na₂CO₃
For example, if you calculated 0.018 moles of NaCl and 0.0047 moles of Na₂CO₃:
- Mole ratio = 0.018 moles NaCl / 0.0047 moles Na₂CO₃
5. Use the mole ratio to write a balanced chemical equation for the reaction:
For example, if the mole ratio is 2:1 (2 moles of NaCl produced for every 1 mole of Na₂CO₃ reacted), the balanced chemical equation would be:
2 Na₂CO₃ + X → 2 NaCl + Y
6. The theoretical mole ratio according to the balanced equation is determined from the coefficients of the balanced equation:
For example, in the balanced equation above, the theoretical mole ratio is 2:1.
7. Use the theoretical mole ratio to calculate the theoretical yield of NaCl in grams from 0.5g of Na₂CO₃:
- Theoretical yield of NaCl = Moles Na₂CO₃ * (Theoretical mole ratio) * MW NaCl
For example:
- Theoretical yield of NaCl = 0.0047 moles Na₂CO₃ * 2 moles NaCl / 1 mole Na₂CO₃ * 58.443 g/mole NaCl
8. Calculate the percent yield of NaCl as the ratio of the experimental grams of NaCl to the theoretical grams of NaCl:
- Percent yield = (Experimental grams NaCl / Theoretical grams NaCl) * 100%
For example, if you obtained 0.015g of NaCl experimentally and calculated the theoretical yield as 0.153g:
- Percent yield = (0.015g / 0.153g) * 100%
9. Possible sources of error that could have reduced the yield include impurities in reagents, incomplete reaction, loss during transfer or handling, measurement errors, and experimental limitations of the apparatus.