Answer:
0.184 atm
Explanation:
The ideal gas equation is:
PV = nRT
Where<em> P</em> is the pressure, <em>V</em> is the volume, <em>n</em> is the number of moles, <em>R</em> the constant of the gases, and <em>T</em> the temperature.
So, the sample of N₂O₃ will only have its temperature doubled, with the same volume and the same number of moles. Temperature and pressure are directly related, so if one increases the other also increases, then the pressure must double to 0.092 atm.
The decomposition occurs:
N₂O₃(g) ⇄ NO₂(g) + NO(g)
So, 1 mol of N₂O₃ will produce 2 moles of the products (1 of each), the <em>n </em>will double. The volume and the temperature are now constants, and the pressure is directly proportional to the number of moles, so the pressure will double to 0.184 atm.
Answer: The system will try and offset the change.
Explanation: Any change in the equilibrium is studied on the basis of Le-Chatelier's principle.
This principle states that if there is any change in the variables of the reaction, the equilibrium will shift in a direction to minimize the effect.
Thus if temperature is increased, the reaction will shift in a direction where temperature is decreasing and vice versa. Similarly if pressure is increased, the reaction will shift in a direction where pressure is decreasing and vice versa.
Atomic number is less than 11
Answer:
The answer to your question is 2.1
Explanation:
Data
Molarity = 1 l
mass = 120 g of NaCl
moles = ?
Formula
Process
1.- Calculate the number of moles of NaCl
Molecular weight NaCl = 23 + 35.5 = 58.5 g
2.- Calculate the number of moles using proportions
58.5 g of NaCl --------------- 1 mol
120.0 g of NaCl --------------- x
x = ( 120 x 1) / 58.5
x = 2.1 moles
3.- Calculate Molarity
Substitution
Simplification and result
Molarity = 2.1
