Some hydrogen gas is collected over water at 20.0 Cel. and the levels inside the container is the same. The partial pressure of hydrogen is 742.5 torr. What is the barometric pressure as the time the gas was collected.
My answer is 742.5 torr = 17.5 torr = 760 torr. Am I correct. thanks
No and yes.
Ptotal = pH2 + pH2O.
pH2 is given as 742.5
I assume you looked up the vapor pressure of H2O at 20 C and found 17.5 torr.
So 742.5 + 17.5 = 760.
I think you just made a typo and hit = instead of +.
Well, let's see if I can help you clown this one up a bit!
You're not quite correct, but don't worry, I'm here to make it all a bit more fun for you!
When hydrogen gas is collected over water, it can be affected by the vapor pressure of water. So, in order to find the barometric pressure, we need to consider the partial pressure of water vapor.
At 20.0°C, the vapor pressure of water is approximately 17.5 torr. Since the level of the water inside the container is the same, we can subtract this vapor pressure from the total pressure to find the barometric pressure.
So, the barometric pressure would be 742.5 torr - 17.5 torr, which gives us 725 torr.
So, the correct answer is 725 torr, not 760 torr.
I hope I could bring a smile to your face while explaining this!
To determine the barometric pressure at the time the gas was collected, we need to calculate the partial pressure of water vapor in the air and subtract it from the total pressure.
First, we need to find the vapor pressure of water at 20.0 °C. The vapor pressure of water at different temperatures can be found in a reference table or calculated using a vapor pressure chart or equation. At 20.0 °C, the vapor pressure of water is approximately 17.5 torr.
Next, we subtract the partial pressure of water vapor from the total pressure to find the barometric pressure:
Barometric pressure = Total pressure - Partial pressure of water vapor
Barometric pressure = 742.5 torr - 17.5 torr
Barometric pressure = 725 torr.
Therefore, the barometric pressure at the time the gas was collected is 725 torr, not 760 torr.
To find the barometric pressure at the time the gas was collected, you need to understand the concept of Dalton's Law of partial pressures. According to Dalton's Law, the total pressure of a mixture of gases is equal to the sum of the partial pressures of each gas.
In this case, the partial pressure of hydrogen is given as 742.5 torr. However, since the gas is collected over water, the water vapor also contributes to the total pressure.
Water vapor exerts a partial pressure known as the vapor pressure, which is dependent on the temperature. At 20.0°C, the vapor pressure of water is approximately 17.5 torr.
To find the barometric pressure, you need to add the partial pressure of hydrogen and the vapor pressure of water:
Barometric pressure = partial pressure of hydrogen + vapor pressure of water
Barometric pressure = 742.5 torr + 17.5 torr
Barometric pressure = 760 torr
Therefore, your answer of 742.5 torr = 17.5 torr = 760 torr is correct. The barometric pressure at the time the gas was collected is indeed 760 torr.