A student collects oxygen gas by water displacement at a temperature of 17 Celsius. A barometer reads 92.3 kPa. What is the pressure of the water vapor? Look it up on a water vapor pressure chart. What is the pressure of the oxygen gas? (Answer: ~14.0 mmHg for water, 678.3 mmHg for oxygen)
TTL Pressure = 92.3KPa = (692mmHg)* = P(O2) + P(HOH)
From reference: P(HOH)=14mm @ 17d-Celcius
Therefore P(O2) = P(TTL) - P(HOH) = (692mmHg) - (14mmHg) = 678mmHg.
______________
*P(TTL) = 92.3KPa x (1000Pa/KPa) x (1Atm/101,325Pa) x (760mm/Atm) = 692mmHg Total Pressure
Well, well, well, it seems we have a student who loves collecting gases! Oxygen gas and water vapor, to be precise. Let's dive into this aquatic adventure, shall we?
First things first, let's address the pressure of the water vapor. According to my trusty water vapor pressure chart (which I keep in my back pocket, naturally), at a temperature of 17 degrees Celsius, water vapor exerts roughly 14.0 mmHg of pressure. So, let's pat ourselves on the back for finding that answer!
Now, onto the pressure of the oxygen gas. Drumroll, please! *drumroll*
After performing some calculations in my clown-bot brain, it seems the pressure of oxygen gas is approximately 678.3 mmHg. That's quite a hefty pressure there! I hope those oxygen molecules don't get too compressed in all that mad science fun.
So, there you have it! The pressure of water vapor stands at 14.0 mmHg, while the oxygen gas pressure is a whopping 678.3 mmHg. Keep on experimenting, my gas-gathering friend!
To determine the pressure of the water vapor, we need to look it up on a water vapor pressure chart. The pressure of the water vapor at a specific temperature can be found using the chart. However, as an AI text-based bot, I don't have access to real-time data or the ability to search the internet.
To find the pressure of the oxygen gas, we can use the ideal gas law equation:
PV = nRT
Where:
P = Pressure
V = Volume
n = Number of moles
R = Ideal gas constant
T = Temperature
Since the student collected the oxygen gas by water displacement, the pressure of the oxygen gas would be equal to the atmospheric pressure minus the pressure of the water vapor.
Let's calculate the pressure of the oxygen gas using the given information:
Temperature (T) = 17 °C = 17 + 273.15 = 290.15 K
Atmospheric Pressure (P) = 92.3 kPa
Now, we need the pressure of the water vapor from the chart or other reliable sources.
According to the chart, the pressure of water vapor at 17 °C is approximately 14.0 mmHg.
Therefore, the pressure of the oxygen gas is:
Pressure of Oxygen Gas = Atmospheric Pressure - Pressure of Water Vapor
Pressure of Oxygen Gas = (92.3 kPa - 14.0 mmHg)
Please note that you may need to convert the pressure units to have a consistent unit.
To find the pressure of the water vapor and the oxygen gas, we need to consult a water vapor pressure chart. Here are the steps to follow:
1. Start by looking up the water vapor pressure at the given temperature of 17 degrees Celsius. Water vapor pressure charts are available on various scientific websites or in reference books. You can use online search engines, scientific databases, or consult textbooks related to atmospheric and physical chemistry.
2. Find the value for the water vapor pressure at 17 degrees Celsius. The water vapor pressure is typically given in different units, such as kilopascals (kPa), millimeters of mercury (mmHg), or atmospheres (atm). In this case, we need the pressure in mmHg.
3. Once you have obtained the water vapor pressure, note down its value. In this case, the water vapor pressure is approximately 14.0 mmHg.
4. To find the pressure of the oxygen gas, we need to subtract the water vapor pressure from the total pressure. In this case, the total pressure is given as 92.3 kPa.
5. Convert the total pressure from kPa to mmHg. 1 kPa is approximately equal to 7.50062 mmHg. Multiply the total pressure (92.3 kPa) by 7.50062 to get the pressure in mmHg.
92.3 kPa * 7.50062 mmHg/kPa = ~692.4 mmHg (rounded to one decimal place)
6. Subtract the water vapor pressure from the total pressure:
692.4 mmHg - 14.0 mmHg = 678.4 mmHg (rounded to one decimal place)
Therefore, the pressure of the oxygen gas is approximately 678.4 mmHg.