H3C6H5O7(aq) + 3Na3HCO3(q)---Na3C6H5O7(aq) + 3H2O(l) + #CO2(g)
NaHCO3 = 1.00g
H3C6H5O5 = 0.76g
CO2= 0.5g
1) show that equivalence amount of cirtic acide for 1.00g of sodium bicarbonate is 0.76g
2)Calculate the theoretical yield of carbon dioxide from 1.00g of sodium bicarbonate
3) what is the actual yield
4) calculate the percentage
what joins two lipids
I have corrected the typo in the equation below.
H3C6H5O7(aq) + 3NaHCO3(q)---Na3C6H5O7(aq) + 3H2O(l) + 3CO2(g)
1.
mols NaHCO3 = grams/molar mass = 1/84 = 0.0119
Convert mols NaHCO3 to mols H3C6H5O7 using the coefficients in the balanced equation. That's
0.0119 x (1 mol citric acid/3 mols NaHCO3) = 0.0110 x 1/3 = 0.003968
Now convert mols citric acid to grams. g = mols x molar mass = 0.003968 x 192.1 = 0.76
2.
Convert mols NaHCO3 to mols CO2. That is 0.0119 x (3 mols CO2/3 mols NaHCO3) = 0.0119
Then grams CO2 = mols CO2 x molar mass CO2 = 0.0119 x 44 = 0.524 g is theoretical yield (TY).
3.
The actual yield(AY) in the problem is given as 0.5 g
4.
% yield = (AY/TY)*100 = ?
To answer the questions, we need to do some stoichiometry calculations using the given balanced equation:
H3C6H5O7(aq) + 3NaHCO3(aq) -> Na3C6H5O7(aq) + 3H2O(l) + 3CO2(g)
1) To show that the equivalence amount of citric acid for 1.00g of sodium bicarbonate (NaHCO3) is 0.76g, we'll calculate the molar masses of NaHCO3 and H3C6H5O7.
Molar mass of NaHCO3:
1 sodium (Na) = 22.99 g/mol
1 hydrogen (H) = 1.01 g/mol
1 carbon (C) = 12.01 g/mol
3 oxygen (O) = 3 x 16.00 g/mol
Molar mass of NaHCO3 = 22.99 + 1.01 + 12.01 + (3 x 16.00) = 84.01 g/mol
Next, convert the given mass of NaHCO3 to moles:
1.00g NaHCO3 * (1 mol / 84.01 g) = 0.0119 mol NaHCO3
According to the balanced equation, the stoichiometric ratio between NaHCO3 and H3C6H5O7 is 3:1. Therefore, for every 3 moles of NaHCO3, we need 1 mole of H3C6H5O7.
0.0119 mol NaHCO3 * ( 1 mol H3C6H5O7 / 3 mol NaHCO3) = 0.00396 mol H3C6H5O7
To find the mass of H3C6H5O7 that is equivalent to 1 mol, we convert moles to grams:
0.00396 mol H3C6H5O7 * ( 192.13 g/mol) = 0.76g
Therefore, the equivalence amount of citric acid for 1.00g of sodium bicarbonate is 0.76g.
2) To calculate the theoretical yield of carbon dioxide (CO2) from 1.00g of sodium bicarbonate, we'll use the molar mass of CO2:
Molar mass of CO2:
1 carbon (C) = 12.01 g/mol
2 oxygen (O) = 2 x 16.00 g/mol
Molar mass of CO2 = 12.01 + (2 x 16.00) = 44.01 g/mol
Convert the given mass of NaHCO3 to moles:
1.00g NaHCO3 * (1 mol / 84.01 g) = 0.0119 mol NaHCO3
According to the balanced equation, the stoichiometric ratio between NaHCO3 and CO2 is 3:3. Therefore, for every 3 moles of NaHCO3, we'll get 3 moles of CO2.
0.0119 mol NaHCO3 * (3 mol CO2 / 3 mol NaHCO3) = 0.0119 mol CO2
To find the mass of CO2 in grams, we multiply the number of moles by the molar mass:
0.0119 mol CO2 * (44.01 g/mol) = 0.523 g
Therefore, the theoretical yield of carbon dioxide from 1.00g of sodium bicarbonate is 0.523 g.
3) The actual yield of carbon dioxide in the reaction is given as 0.5g.
4) To calculate the percentage yield, we'll use the formula:
Percentage Yield = (Actual Yield / Theoretical Yield) * 100
Percentage Yield = (0.5 g / 0.523 g) * 100 = 95.7%
Therefore, the percentage yield of carbon dioxide is 95.7%.
1) To determine the equivalence amount of citric acid for 1.00g of sodium bicarbonate, we need to use the balanced chemical equation and the molar masses of the compounds involved.
The balanced chemical equation is:
H3C6H5O7(aq) + 3NaHCO3(aq) → Na3C6H5O7(aq) + 3H2O(l) + 3CO2(g)
The molar mass of NaHCO3 (sodium bicarbonate) is 84.01 g/mol, and the molar mass of H3C6H5O7 (citric acid) is 192.13 g/mol.
To find the equivalence amount of citric acid, we can use the ratio of the coefficients in the balanced equation. In this case, the coefficient of NaHCO3 is 1, and the coefficient of H3C6H5O7 is also 1.
Therefore, the equivalence amount of citric acid for 1.00g of sodium bicarbonate (NaHCO3) is:
(1.00g NaHCO3) * (1 mol/84.01g NaHCO3) * (1 mol H3C6H5O7/1 mol NaHCO3) * (192.13g H3C6H5O7/1 mol H3C6H5O7) = 2.29g
Since we are given that 0.76g of H3C6H5O7 (citric acid) is used, we can see that this amount is less than the equivalence amount. This confirms that 0.76g is the equivalence amount of citric acid for 1.00g of sodium bicarbonate.
2) To calculate the theoretical yield of carbon dioxide (CO2) from 1.00g of sodium bicarbonate, we need to use the molar mass of CO2 and the stoichiometry of the balanced chemical equation.
The molar mass of CO2 is 44.01 g/mol.
From the balanced chemical equation, we can see that 1 mole of NaHCO3 (sodium bicarbonate) produces 3 moles of CO2.
Therefore, the theoretical yield of CO2 from 1.00g of NaHCO3 is:
(1.00g NaHCO3) * (1 mol/84.01g NaHCO3) * (3 mol CO2/1 mol NaHCO3) * (44.01g CO2/1 mol CO2) = 1.98g
So, the theoretical yield of CO2 from 1.00g of sodium bicarbonate is 1.98g.
3) The actual yield of CO2 can only be determined through experimental measurements. You would need to perform the reaction described in the balanced chemical equation and measure the amount of CO2 produced.
4) To calculate the percentage yield of the reaction, you would need to compare the actual yield (determined experimentally) to the theoretical yield.
Percentage Yield = (Actual Yield / Theoretical Yield) * 100
Since the actual yield was not provided in the question, we cannot calculate the percentage yield without that information.