What is the mass of 2.15 liters of N2 gas at STP?
1 answer:
Answer:
2.68g
Explanation:
Given parameters:
Volume of gas at STP = 2.15L
Unkown:
Mass of Nitrogen N₂ gas at STP = ?
Solution
To find the mass of the gas at STP, we use the mole concept approach.
In using the mole approach we follow the following procedures:
1. Find the number of moles of gas at STP using the relationship below:
Number of moles =
Note: 1L = 1dm³
2. Then using the mole and mass relationship, we can find the mass of the gas using the equation below:
Mass = number of moles x molar mass
Workings
1. Number of moles of N₂ =
Number of moles of N₂ = 0.096mole
2. Given that the atomic mass of N = 14g
Molar mass of N₂ = 2 x 14 = 28gmol⁻¹
Mass = 0.096mol x 28gmol⁻¹ = 2.68g
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Answer:
The new equilibrium total pressure will be increased to one-half to initial total pressure.
Explanation:
From the information given :
The equation of the reaction can be represented as;
From above equation:
2 moles of sulphur dioxide reacts with 1 mole of oxygen (i.e 2 moles +1 mole =3 moles ) to give 2 moles of sulphur trioxide
So; suppose the volume of this system is compressed to one-half its initial volume and then equilibrium is reestablished.
So if this process takes place ; the equilibrium will definitely shift to the side with fewer moles , thus the equilibrium will shift to the right. As such; there is increase in pressure.
Let the total pressure at the initial equilibrium be
and the total pressure at the final equilibrium be
According to Boyle's Law; Boyle's Law states that the pressure of a fixed mass of gas is inversely proportional to the volume, provided the temperature remains constant.
Thus;
P ∝ 1/V
P = K/V
PV = K
where K = constant
So;
PV = constant
Hence;
From the foregoing; since the volume is decreased to one- half to initial Volume; then ,
also;
Thus ;
Dividing both sides by
From ;
Thus; The new equilibrium total pressure will be increased to one-half to initial total pressure.
The atomic mass of an element is the average relative mass of its atoms as compared with an atom of carbon-12 whose mass is taken as 12. In terms of percentages of different isotopes, the average atomic mass can be determined as follows: = ∑(
X
)/100. Where,
is the percentage abundance of isotope with atomic number
.
So, average atomic mass of neon = = 20.177 amu.