M1V1 = M2V2
(2.50)(100.0) = (0.550)V2
V2 = 455mL
From 100.0 mL of 2.50 M KBr, you can prepare 455 mL of 0.550 M solution.
1) Calcium carbonate comprises 40.0% calcium by weight.
M(CaCO₃)=100.1 g/mol
M(Ca)=40.1 g/mol
w(Ca)=40.1/100.1=0.400 (which is 40.0%)!
2) The mass fraction mentioned is superfluous information.
3) The resulting solution is:
m(Ca)=1.2 g
m(CaCO₃)=M(CaCO₃)*m(Ca)/M(Ca)
m(CaCO₃)=100.1g/mol*1.2g/40.1g/mol=3.0 g
Solution:
The gas's new temperature is 604K
Justification:
Assuming standard temperature and pressure, we can determine the gas's temperature using the ideal gas law;
Step 1: Formulate the general gas law equation
P1V1/T1 = P2V2/T2
Step 2: Insert the values, converting as needed to standard units.
P1 = 0.800 atm
V1 = 0.180 L
T1 = 29°C = 273 + 29 = 302K
P2 = 3.20 atm
V2 = 90 mL = 90 * 10^-3 L = 0.09 L
Step 3: Solve for T2
The new gas temperature T2 is calculated as:
T2 = P2V2T1/(P1V1)
T2 = 3.20 * 0.09 * 302 / (0.800 * 0.180)
T2 = 86.976 / 0.144
T2 = 604K
The gas's new temperature is 604K.
The formula for a monoprotic acid can be represented as HA, and its reaction with a base is shown as follows: HA + NaOH ---> NaA + H₂O. The stoichiometry between the acid and the base is 1:1. At the point of neutralization, the moles of HA equals the moles of the base. The moles of NaOH that reacted can be calculated as 0.100M / 1000 mL/L x 30.0 mL = 0.003 mol. Consequently, the moles of HA that reacted equal 0.003 mol. The mass of the acid is 0.384 g, yielding a molar mass of 0.384 g / 0.003 mol = 128 g/mol.
For instance, what is the difference in electronegativity for Acetone(CH2O)? Are there two distinct values, namely 0.4 for C versus H and 1.0 for C versus O? How do you decide which one to adopt?
6 Comments
AlwaysReady1
•
Apr 3, 2016, 10:14 PM
I may not fully grasp the question, but if you’re seeking to determine a compound's electronegativity to assess its electron-attracting capability, there are various other influencing factors.
It varies depending on the compound. For example, CH2O, known as formaldehyde, has oxygen with two pairs of electrons that can be donated. Neither hydrogen nor carbon can bond further as they are already fulfilling their valence shell requirements.
Robo94
•
You're attempting to apply a concept from a binary system to a more complex one. I assume you're aiming to figure out a molecule's dipole moment. In the case of a diatomic molecule (where A is bonded to B), the potential difference can simply be determined as A minus B. For larger molecules, the calculations become much more involved.
If this inquiry is related to homework assistance, it’s a distinctly different method from what you might be accustomed to. I recommend starting with water and then expanding out from there.
Check this out: https://www.khanacademy.org/science/organic-chemistry/gen-chem-review/electronegativity-polarity/v/dipole-moment
Philosoaxolotl
•
Electronegativity pertains to single elements (or rather individual atoms) and lacks straightforward applicability to broader molecules.
What precisely are you aiming to do with this data? If you're delving into how electrons transition between molecules, the situation is more intricate—within a molecule, the more electronegative elements pull electrons from other atoms (which frequently happens in organic compounds, such as when oxygen bonds with carbon and pulls in some of its electrons). Nevertheless, this effect diminishes in lengthened molecules. The system is more complicated as molecules do not possess a single, constant electronegativity (which is more accurate for atoms); instead, they exhibit varied localized charge regions that will respond differently.
From what I gather, your question pertains to the electronegativity difference among the atoms within an acetone molecule. This indeed relies on which two atoms you are examining and won't remain constant throughout; however, the difference won't simply match the values listed in an electronegativity table due to the factors discussed earlier.
This explanation might seem a bit hazy, and I’m just an undergraduate, so please take my interpretation lightly, but I am open to clarifying further if needed.
cheeseborito
•
That statement is inaccurate.
Electronegativity represents the attraction an atom holds for the electrons in a covalent bond with another atom. Essentially, an element does not have a singular electronegativity; it fluctuates based on its bonding partners. We cannot discuss the electronegativity of an atom in isolation.
While average values are useful for practical discussions (though they may not capture the nuance), the effective electronegativity of an oxygen atom bonded to carbon will remain fairly consistent.
As far as my understanding goes, even though my definition of electronegativity may lack precision, the influence an oxygen atom has on the electrons of a carbon atom is affected by what the carbon is bonded to. For instance, the local charge around the oxygen in acetic acid will be more pronounced than that in decanoic acid.
I may have phrased the electronegativity issue poorly—what I meant was the interaction between pairs of atoms as related to one another. An oxygen will exert a consistent pull regarding a carbon atom, but the changes in local charge can differ due to the influence of surrounding atoms, making the topics we typically utilize electronegativity to clarify substantially more intricate.
