<span>1.44x10^23 molecules of oxygen gas
The ideal gas law is
PV = nRT
where
P = pressure (800.0 Torr)
V = volume (5.60 L)
n = number of moles
R = Ideal gas constant (62.363577 L*Torr/(K*mol) )
T = absolute temperature (27C + 273.15 = 300.15 K)
Let's solve for n, the substitute the known values and solve.
PV = nRT
PV/RT = n
(800.0 Torr*5.60 L)/(62.363577 L*Torr/(K*mol)*300.15 K) = n
(4480 L*Torr)/(18718.42764 L*Torr/mol) = n
0.239336342 mol = n
So we have 0.239336342 moles of oxygen molecules. To get the number of atoms, we need to multiply by avogadro's number, so:
0.239336342 * 6.0221409x10^23 = 1.44x10^23</span>
Synonym: common fault
Antonym: un-normal fault
Homonym: geologic or hanging walls
Answer:
You can find the volume of an irregular object by immersing it in water in a beaker or other container with volume markings, and by seeing how much the level goes up. Or by multiplying all the sides of the container. #markasbrainliest
Answer: Molar mass of 
is 17.03 g
Explanation:
Molar mass is defined as the mass in grams of 1 mole of a substance.
S.I Unit of Molar mass is gram per mole and it is represented as g/mol.
It is found by adding the atomic masses of all the elements present.
Atomic Mass of Nitrogen (N) = 14.007 g
Atomic Mass of Hydrogen (H) = 1.008 g
Molar mass of = 1(14.007)+3(1.008) g = 17.03 g
Answer:
The most common example is the molar volume of a gas at STP (Standard Temperature and Pressure), which is equal to 22.4 L for 1 mole of any ideal gas at a temperature equal to 273.15 K and a pressure equal to 1.00 atm.If an ideal gas at a constant temperature is initially at a pressure of 3.8 atm and is then allowed to expand to a volume of 5.6 L and a pressure of 2.1 - 18914… ... of 5.6 L and a pressure of 2.1 atm, what is the initial volume of the gas? ... An ideal gas is at a pressure of 1.4 atm and has a volume of 3 L.
Explanation:
I hope I help :)
