Answer:
Ethanol = 102.29 g
Carbon Dioxide = 97.71 g
Solution:
The Balance Chemical Equation for the fermentation of Glucose is as follow,
C₆H₁₂O₆ → 2 C₂H₅OH + 2 CO₂
Mass of Ethanol produced:
According to equation;
180.156 g (1 mole) C₆H₁₂O₆ produces = 92.14 g (2 moles) of C₂H₅OH
So,
200 g of C₆H₁₂O₆ will produces = X g of C₂H₅OH
Solving for X,
X = (200 g × 92.14 g) ÷ 180.156 g
X = 102.29 g of C₂H₅OH
Mass of Carbon Dioxide produced:
According to equation;
180.156 g (1 mole) C₆H₁₂O₆ produces = 88.02 g (2 moles) of CO₂
So,
200 g of C₆H₁₂O₆ will produces = X g of CO₂
Solving for X,
X = (200 g × 88.02 g) ÷ 180.156 g
X = 97.71 g of CO₂
The more electronegative an atom is, the more strength it has to pull electrons closer to itself. If one atom is highly electronegative and the other is barely electronegative then an ionic bond will form. If one is highly electronegative and the other is slightly electronegative, then a polar covalent bond will form. If they are both the same electronegativity then a nonpolar covalent bond will form.
Sodium- Na
most active element- Fluorine
lightest element- Hydrogen
Answer:
Some examples of homoatomic molecules are hydrogen gas, and oxygen gas and some examples of heteroatomic molecules are water, methane
Explanation:
Answer: a. 7.31 g
b. 20.4 %
Explanation:
To calculate the moles :
According to stoichiometry :
3 moles of require = 1 mole of
Thus 0.645 moles of will require= of
Thus is the limiting reagent as it limits the formation of product and is the excess reagent.
As 3 moles of give = 2 moles of
Thus 0.645 moles of give = of
Mass of
Thus theoretical yield for this reaction under the given conditions is 7.31 g.
b)
The percent yield for this reaction under the given conditions is 20.4 %