Empirical formula is the simplest ratio of whole numbers of components in a compound
calculating for 100 g of compound
C H O
mass 64.27 g 7.19 g 28.54 g
number of moles 64.27 g / 12 g/mol 7.19 g/1 g/mol 28.54 g / 16 g/mol
= 5.356 mol = 7.19 mol = 1.784 mol
divide by least number of moles
5.356 / 1.784 7.19 / 1.784 1.784 / 1.784
= 3.002 4.03 = 1.000
rounded off to nearest whole number
C - 3
H - 4
O - 1
empirical formula - C₃H₄O
mass of empirical formula = 12 g/mol x 3 + 1 g/mol x 4 + 16 g/mol x 1 = 56 g
molecular mass = 168.19 g/mol
molecular formula is the actual ratio of elements making up the compound
number of empirical units = molar mass of molecule / empirical mass
empirical units = 168.19 g/mol / 56 g = 3.00
there are 3 empirical units making up the molecular formula
molecular formula = 3 x C₃H₄O
molecular formula = C₉H₁₂O₃
Answer: Yes
The antibonding orbital is empty. Thus, H2 is a stable molecule.
Answer:
There are two possible answers to the question
I) decreasing the pressure of the system
II) decreasing the temperature of the system
Explanation:
Looking at the equation of the reaction, it can be seen that the reaction is endothermic. This implies that decreasing the temperature favours the reverse reaction and more NO2 is produced.
Secondly, decreasing the pressure drives the equilibrium position towards the side having the higher total volume hence decreasing the pressure favours the reverse reaction and more NO2 is produced.
The density of the patient's hemoglobin in their blood in units of g/ml = 0.2g/mL
<h3>Calculation of hemoglobin density</h3>
Hemoglobin is the red blood cell pigment that transports oxygen to the body cells.
1 gram of hemoglobin = 2.15mg
Blood volume of the patient is = 4.9ml
Density= mass/volume
Therefore the density of patients hemoglobin= 1/4.9 = 0.2g/mL
Learn more about hemoglobin here:
brainly.com/question/8197071
Answer: The correct option is, They are different units of concentration.
Explanation: Molarity : It is defined as the number of moles of solute present in one liter of solution.
