Determine the partial pressure of the hydrogen gas collected in the gas collection tube.

Question

anonymous · Answer

Mass of magnesium strips (grams) 0.028g
Volume of gas collected (mL) 24mL
Barometric pressure (atm) 1atm
Room temperature (C) 24c
Vapor pressure of the water (torr) 22.4torr

anonymous · Answer

Balanced equation:
Mg(s) + 2HCl(aq) --> MgCl2(aq) + H2(g)

chmvijay · Answer

u know the equation to do that?

anonymous · Answer

no.

jfraser · Answer

when the gas is collected out of an aqueous solution, a tiny amount of water is picked up and exists with the gas molecules inside the collection tube.

the total pressure inside the tube will be equal to the total pressure of the outside atmosphere (1atm or 760 torr).

the water is responsible for a small portion of that pressure (22.4 torr)

what's the pressure of JUST the hydrogen gas, if the total pressure is 760 torr, and 22.4 torr is from the water

anonymous · Answer

i don't know, can you help me?

jfraser · Answer

the total pressure is 760 torr. most of that pressure is created by the hydrogen gas, and a small part is created by the water vapor. you have the pressure of the water, how much pressure does the hydrogen create so that the pressures ADD to 760 torr?

anonymous · Answer

not sure...do you subtract?

jfraser · Answer

yes