1. molarity = (moles)/vol in litres
0.5=[(weight/40)*1000]/4
0.5 = weight/16
weight of NaOH = 8 grams
2. weight = 0.45*850*84/100 gms
molecular weight = 85m (not sure abt this)
Answer:
0.58 atm
Explanation:
Step 1: Given data
- Total pressure of the gaseous mixture (P): 1.05 atm
- Partial pressure of N₂ (pN₂): 0.35 atm
- Partial pressure of H₂ (pH₂): 0.12 atm
- Partial pressure of CO₂ (pCO₂): ?
Step 2: Calculate the partial pressure of CO₂
The total pressure of the gaseous mixture is equal to the sum of the partial pressures of the individual gases.
P = pN₂ + pO₂ + pCO₂
pCO₂ = P - pN₂ - pO₂
pCO₂ = 1.05 atm - 0.35 atm - 0.12 atm = 0.58 atm
A mole of CO2 = 2 moles of O2
8 CO moles x 2 =
16 moles
The molecules are continually colliding with each other and with the walls of the container. When a molecule collides with the wall, they exert small force on the wall The pressure exerted by the gas is due to the sum of all these collision forces. The more particles that hit the walls, the higher the pressure.
