Hydrogen gas is collected by water displacement. If the barometric pressure is 752.0 torr and the water vapor pressure is 17.5 torr, what is the partial pressure of the hydrogen collected

734.5 torr

Explanation:

Let's find the difference between the barometric pressure and the water vapour pressure

Bp = 752 torr

Wp = 17.5 torr

Bp - wp

752- 17.5 = 734.5 torr

The partial pressure of the hydrogen collected is 734.5 torr

Explanation:The partial pressure of the hydrogen collected can be calculated using Dalton's law of partial pressure. Dalton's law of partial pressure states that  in a mixture of non-reacting gases, the total pressure exerted is equal to the sum of the partial pressures of the individual gases.

Mathematically,

P(total) = P1 + P2 + P3 + ... + Pn

From the question,

Parameters given:

Barometric pressure (Total pressure) = 752.0 torr

Water vapour pressure = 17.5 torr

Partial pressure of hydrogen = ??

Using,

P(total) = P(water vapour) + P(Hydrogen)

752.0 torr = 17.5torr + P(Hydrogen)

P(Hydrogen) = 752.0 torr - 17.5 torr

P(Hydrogen) = 734.5 torr

Therefore the partial pressure of the hydrogen collected is 734.5 torr

the increase of protons   hope this

a polar bond is formed when electrons are shared unevenly between atoms