Answer:
the answer is 25.032g check pic for explanation
The molecular formula of the compound that we are required to find is the compound C4H8O8
<h3>What is empirical formula?</h3>
The empirical formula of a compound is a formula that shows the ratio of each atom present in the compound. We will start by dividing each mass with the relative atomic mass of the atom.
Carbon - 48.38 g/12 Hydrogen - 6.74 g/1 Oxygen - 53.5 g/16
Carbon - 4 Hydrogen - 6.74 Oxygen - 8.9
Dividing through by the lowest ratio;
Carbon - 4/4 Hydrogen - 6.74/4 Oxygen 8.9/4
Carbon 1 Hydrogen 2 Oxygen 2
The empirical formula is CH2O2.
To obtain the molecular formula; brainly.com/question/11588623
[12 + 2 + 32]n = 180
n = 180/[12 + 2 + 32]
n =4
The compound C4H8O8
Learn more about empirical formula:
Explanation:
Since mole ratio of O2 : NH3 = 7 : 4,
Volume of NH3 = 50dm³ * 4/7 = 28.57dm³.
Glucose can be converted into ethanol, carbon dioxide and energy (usually in the form of heat).
Using chemical formulas, this can be illustrated as follows:
Glucose = Ethanol + Carbon Dioxide + Energy
C6H12O6 = 2C2H5OH + 2CO2 + Energy
From the periodic table:
molecular mass of carbon = 12 grams
molecular mass of oxygen = 16 grams
molecular mass of hydrogen = 1 gram
Therefore:
molar mass of glucose = 6(12) + 12(1) + 6(16) = 180 grams
molar mass of ethanol = 2(12) + 5(1) + 16 + 1 = 46 grams
molar mass of carbon dioxide = 1(12) + 2(16) = 44 grams
Based on the conversion equation, each one mole of glucose converts into two moles of ethanol and two moles of carbon dioxide.
Therefore, each 180 grams of glucose converts into 46 x 2 = 92 grams of ethanol and 44 x 2 = 88 grams of carbon dioxide in addition to energy.
To calculate the mass of ethanol and carbon dioxide produced from 200 grams of glucose, we will simply use cross multiplication as follows:
mass of ethanol = (200 x 92) / 180 = 102.2 grams
mass of carbon dioxide = (200 x 88) / 180 = 97.7 grams
Total mass of ethanol and carbon dioxide = 102.2 + 97.7 = 199.9 grams
Answer: -
O 2 limiting reagent
53.83 g CO2 theoretical Yield
97.9% percentage yield
Explanation: -
Mas of CH4 = 23.2 g
Molar mass of CH4 = 12 x 1 + 1 x 4 = 16g
Mass of O2 = 78.3 g
Molar mass of O 2 – 16 x 2 = 32 g
The balanced chemical equation for the reaction is
CH4 + 2 O2 = CO2 + 2 H2O
From the balanced equation we see that
2 O 2 reacts with 1 CH4
2 x 32 g of O 2 react with 16 g of CH4
78.3 g of O 2 react with
= 19.575 g pf CH4
Thus CH4 is in excess.
The limiting reagent is thus O 2.
Molar mass of CO2 = 12 x 1 + 16 x 2= 12 +32 = 44g
From the balanced equation we see
2O 2 gives 1 CO2
2 x 32 g of O 2 gives 44g of CO2
78.3 g of O 2 gives =
=53.83 g of CO2
Theoritical Yield = 53.83 g of CO2
Actual yield = 52.7 g
Percentage yield =
=97.9 %
