Answer:
The answer is below
Explanation:
The density of an object is its mass per unit of volume. Dense objects feel very heavy for their size, while for objects with low density they are very light for their size.
Density is the ratio of mass to volume; it is given by:
Density (D) = mass (m) / volume (V)
An object sinks in water if the density of the object is greater than the density of water. While an objects floats on water if the density of the object is les than the density of water
The answer is B because glucose is an energy source and during photosynthesis, water combines with sunlight and carbon dioxide. You can observe by the chemical equation for photosynthesis : 6CO2 + 6H2O + light energy = C6H12O6 + 6O2
1.0 M, if you're just looking for an answer.
F<span>ormula </span>mass<span> of AgNO</span>3<span> is 107.9 + 14 + (3 X 16) = 169.9 g.</span><span>
</span><span>85.0 g 0.5 mole
------- = ------------ = 1.0 M
169.9 (g/mole) 0.5 liter</span>
1) Chemical equation
C2H5OH + 3 O2 ---> 2 CO2 + 3 H2O
2) Molar ratios
1 mol C2H5OH : 3 mol O2 : 2 mol CO2 : 3 mol H2O
3) Amount of ethanol burned
D = M / V => M = D * V = 0.789 g/ml * 4.61 ml = 3.637 g
Number of moles = mass in grams / molar mass
molar mass of C2H5OH = 2 *12 g/mol + 6*1.0 g/mol + 16.0 g/mol = 46.0 g/mol
=> number of moles of C2H5OH = 3.637 g / 46.0 g/mol = 0.079 mol
4) Amount of oxygen, O2
number of moles of O2 = mass in grams / molar mass
number of moles O2 = 15.70g / 32.0 g/mol = 0.49 mol
5) Limiting reactant
Theoretical ratio: 1 mol C2H5OH / 3 mol O2
Actual ratio: 0.079 mol / 0.49 mol = 0.16
=> there is more oxygen than needed to burn all the ethanol => ethanol burns completely and it is the limiting reactant.
6) Theoretical yield of H2O
1 mol C2H5OH / 3 mol H2O = 0.079 mol C2H5OH / x
=> x = 0.079 mol C2H5OH * 3 mol H2O / 1 mol C2H5OH
=> x = 0.237 mol H2O
Conversion to grams:
mass = molar mass * number of moles
mass H2O = 18.0 g/mol * 0.237 g/mol = 4.27 g <---- theoretical yield
7) grams of H2O collected (yield)
M = V * D = 3.27 ml * 1.00 g/ml = 3.27 g <----- actual yield
8) Percent yield
Percent yield = (actual yield / theoretical yield) * 100 = (3.27 g / 4.27) * 100 = 76.6%
Answer: 76.6%