An apparatus consists of a 4.0 dm3 flask containing nitrogen gas at 25 oc and 803 kpa. it is joined by a valve to a 10.0 dm3 flask containing argon gas 25 oc and 47.2 kpa. the valve is opened and the gases mix. i. what is the partial pressure of each gas after mixing?

Partial pressure of nitrogen = 229.43 kpa

Partial pressure of argon = 33.7 Kpa

Explanation:

Given data:

Volume of flask one = 4.0 dm³

Temperature = 25°C

Pressure of nitrogen = 803 KPa

Final volume = 4.0 dm³ + 10.0 dm³ =  14.0 dm³

Initial volume of argon = 47.2 KPa

Final pressure of both gases when valve is open = ?

Solution:

For nitrogen:

P₁V₁ = P₂V₂

803 KPa × 4 dm³ = P₂ × 14.0 dm³

P₂ = 803 KPa × 4 dm³ /  14.0 dm³

P₂ = 3212 kpa / 14.0

P₂ = 229.43 kpa

For argon:

P₁V₁ = P₂V₂

47.2 KPa × 10.0 dm³  = P₂× 14.0 dm³

P₂ = 47.2 KPa × 10.0 dm³/14.0 dm³

P₂ = 472 kpa/ 14.0

P₂ = 33.7 Kpa

hope this

explanation:

covalent bonds

consist of pairs of electrons shared by two atoms, and bind the atoms to fixed orientation and requre high energies to break them

ionic bonds

when two atoms differ considerably in their electronegativity, then one of the atoms will lose its electron to the other atom. this results in a positively charged ion(cation) and a negatively charged ion (anion)

1 a

2 d

3 a

4 c

explanation: