<span>The ideal gas law.
PV=nRT
pressure x volume = moles x Faraday's constant x Temp Kelvin (C+273)
Original data
Pressure 1 atmosphere
Volume 1 liter
Temp 25C = 298K
New data
Volume 0.5 liter
pressure X
Temp 260C = 533K
P1v1T1 = P2v2T2
plug and chug.
(1)(1)(293) = (x)(0.5)(533)
Solve for X, which is the new pressure. </span>
The molecular formula for compound is
mass of compound is 0.670 g.
To calculate number of atoms first calculate number of moles in the compound as follows:

Molar mass of
is 283.886 g/mol, thus,

Thus, number of mole of
is 0.00236 mol.
From the molecular formula 1 mole of
has 2 mol of P (phosphorus) and 5 mol of O (oxygen).
Thus, number of moles of P and O in 0.00236 mol of
will be:

Similarly,

Now, in 1 mol of an element there are
atoms.
Number of atoms of P will be:

Similarly, number of atoms of O will be:

Total number of atoms will be sum of number of atoms of P and O:

Therefore, total number of atoms in
will be
.
Answer:
mm = 1043.33 g/mol
Explanation:
osmotic pressure (π):
∴ π = 17.8 torr = 0.0234 atm
∴ Cb: solute concentration
∴ T = 25°C = 298 K
∴ R = 0.082 atm.L/K.mol
⇒ Cb = π/RT
⇒ Cb = (0.0234 atm)/((0.082 atm.L/K.mol)(298 K))
⇒ Cb = 9.585 E-4 mol/L
molar mass (mm):
⇒ mm = (1.00 g/L)(L/9.585 E-4 mol)
⇒ mm = 1043.33 g/mol
So potassium is more reactive than lithium because the outer electron of a potassium atom is further from its nucleus than the outer electron of a lithium atom. Hope this answers the question. Have a nice day. Feel free to ask more questions.
The unhybridized pz orbitals on each carbon overlap to a π bond (pi).The sigma bond framework of the ethylene molecule is produced by the overlap of hybrid orbitals or by the interaction of a hybrid orbital and a 1s hydrogen orbital.
Each carbon still has its unhybridized pz orbital, though. Sigma bond are typically the only types of single bonding between atoms. One sigma bond and two pi bonds make up triple bonds. One sigma () bond makes up a single bond, one and one pi () bond makes up a double bond, and one and two bonds make up a triple bond.
To learn more about bond, click here.
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