Question

Determine the partial pressure of the hydrogen gas collected in the gas collection tube. (3 points)


Data Table
Mass of magnesium strip (grams) 0.034 g
Volume of gas collected (mL) 32.2 mL
Barometric pressure (atm) 1.10 atm
Room Temperature (°C) 24.0 °C
Vapor pressure of the water (torr) 22.4 torr

Answer 1

I need a walk-through, I don't understand.

Answer 2

@ganeshie8 Can you help?

Answer 3

Only three points?

Answer 4

use the ideal gas law to find the \(total\) pressure in the tube. That pressure has \(both\) water and hydrogen gas in it. Use the total pressure and the partial pressure of water (given) to find the partial pressure of the hydrogen

Answer 5

@JFraser, thanks so much this helped me alot! My teacher says the barometric pressure is the total pressure; so that's already given. The rest of this message isn't for you.


This is for anyone looking for the answer to a question like this: First, you'd need to convert from torr to atm (760 torr= 1atm) with your vapor pressure of the water.

You then set up an equation like this: PT = P1 + P2
This means that the total pressure equals each individual pressure added together.
So you'd set up the total pressure (the barometric pressure) and the water vapor pressure (which should now be converted to atm, which you should have already done.

This is the last and easiest step; no worries here. Just set up the equation according to what you have:

Barometric Pressure(atm) = P1(LEAVE THIS BLANK) + Water Vapor Pressure (atm)

Now, if you subtrace the Water Vapor Pressure from the Barometric Pressure, you'll have your answer!!!


My teacher hasn't checked this, but I was having so much trouble figuring this out and I really hope this helps someone!!!!!

Answer 6

GJ