What would the partial pressure of hydrogen in the gas collection tube be if the water in the tube was 25.0 mm above the water level in the beaker, the room pressure was 655 mm Hg, and the temperature of the room was 22 degrees C?
I don't know from your description what the set up is.
630 mm Hg
I just had this same question in my class. The answer is 633 mm Hg.
NOT 630 mm Hg.
To find the partial pressure of hydrogen in the gas collection tube, we need to subtract the vapor pressure of water from the total pressure. Here's how we can do it step by step:
Step 1: Convert the water height from millimeters to atmospheres (atm):
Since pressure is typically reported in atmospheres, we need to convert the height of the water column from millimeters to atmospheres. We can use the conversion factor that 1 atm is approximately equal to 760 mm Hg.
25.0 mm / 760 mm Hg = 0.0329 atm
Step 2: Convert the room pressure from millimeters of mercury (mm Hg) to atmospheres (atm):
The room pressure is given as 655 mm Hg. We can use the same conversion factor as in step 1 to convert it to atm.
655 mm Hg / 760 mm Hg = 0.8618 atm
Step 3: Calculate the partial pressure of hydrogen:
The partial pressure of hydrogen is the difference between the total pressure and the vapor pressure of water.
Partial pressure of hydrogen = Room pressure - Vapor pressure of water
Given that the room pressure is 0.8618 atm and the vapor pressure of water at 22 degrees Celsius is 0.0329 atm (which we calculated in step 1), we can now calculate the partial pressure of hydrogen.
Partial pressure of hydrogen = 0.8618 atm - 0.0329 atm = 0.8289 atm
Therefore, the partial pressure of hydrogen in the gas collection tube would be 0.8289 atm.