Volume of 1 mol of gas at standard temperature and pressure is 22.4 L.
That is using ideal gas equation:
PV = nRT
P=pressure
V=volume
n=number of moles
R=gas constant
T=temperature
at STP,
P=1 atm
T=273K
n=1(given)
Putting all the values in the equation will give,
V= 22.4 L
So, the answer is :
The volume of 1 mol of gas at standard temperature and pressure is 22.4 L.
Answer:
1.Handpicking,winnowing and sieving 2. distillation 3.distillation 5. winnowing 6.magnet
Answer:
The final volume will be 5.80 L
Explanation:
Step 1: Data given
Number of moles gas = 0.140 moles
Volume of gas = 2.78 L
Number of moles added = 0.152 moles
Step 2: Calculate the final volume
V1/n1 = V2/n2
⇒ with V1 = the initial volume = 2.78 L
⇒ with n1 = the initial number of moles = 0.140 moles
⇒ with V2 = The new volume = TO BE DETERMINED
⇒ with n2 = the new number of moles = 0.140 + 0.152 = 0.292 moles
2.78/0.140 = V2 /0.292
V2 = 5.80 L
The final volume will be 5.80 L
Phosphorous has three lone electrons that need pairing. Similar to how carbon has 4 lone electrons, and forms CH4
The s orbitals are not symmetrical in shape is a FALSE statement.
An s orbital is so symmetric, more specifically spherically symmetric that it looks the same from all directions.
- The atomic orbitals in the atoms of elements differ in shape.
In essence, the electrons they describe have varying probability distributions around the nucleus. The spherical symmetry of s orbitals is evident in the fact that all orbitals of a given shell in the hydrogen atom have the same energy.
- All s orbitals are spherically symmetrical. Put simply, an electron that occupies an s orbital can be found with the same probability at any orientation (at a distance) from the nucleus.
The s orbitals are therefore represented by a spherical boundary surface which is a surface which captures a high proportion of the electron density.
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