Question

Given a barometric pressure of 737.0mmHg, calculate the pressure of gas sample (a) as indicated by the manometer (Figure 1). Part B Given a barometric pressure of 737.0mmHg. calculate the pressure of gas sample (b) as indicated by the manometer Given a barometric pressure of 737.0mmHg, calculate the pressure of gas sample (a) as indicated by the manometer (Figure 1). Part B Given a barometric pressure of 737.0mmHg, calculate the pressure of gas sample (b) as indicated by the manometer (Elgure 2) Given a barometric pressure of 737.0mmHg, calculate the pressure of gas sample (a) as indicated by the manometer (Figure 1). Given a barometric pressure of 737.0mmHg, calculate the pressure of gas sample (b) as indicated by the manometer (Figure 2).

Answer 1

To determine the pressure of a gas sample with a manometer at sea level, compare the mercury level difference with atmospheric pressure and convert the result to the desired units using conversion factors. So, the correct option is

(a) as indicated by the manometer (Figure 1). Part B Given a barometric pressure of 737.0mmHg.

Step-by-step explanation:

The question pertains to the use of a manometer to measure the pressure of a gas sample at sea level.

With the given barometric pressure of 737.0 mmHg, the pressure of the gas sample can be calculated using the difference in mercury levels in the two sides of the manometer.

The calculation would vary depending on whether the mercury level on the side open to the atmosphere is higher or lower than the side connected to the gas sample.

When the mercury level is higher on the atmospheric side, the pressure of the gas is equal to the atmospheric pressure plus the height difference in mm Hg.
When the mercury level is higher on the gas sample side, the pressure of the gas is the atmospheric pressure minus the height difference in mm Hg.

The pressure in mm Hg can then be easily converted to other units such as atmospheres (atm) or kilopascals (kPa) using their respective conversion factors: 1 atm = 760 mm Hg and 1 atm = 101.325 kPa.

So, the correct option is (a) as indicated by the manometer (Figure 1). Part B Given a barometric pressure of 737.0mmHg.

Answer 2

To determine the pressure of a gas sample with a manometer, subtract or add the height difference in the mercury levels to the atmospheric pressure, then convert to the desired units.

Step-by-step explanation:

To calculate the pressure of a gas sample using an open-end mercury manometer, you need to take into account the atmospheric pressure and the height difference in the mercury levels in the manometer.

When the atmospheric pressure is given (737.0mmHg in this case), and you have the manometer reading (the difference in mercury level), you can calculate the pressure of the gas using the following steps:

1. For gas sample (a), if the mercury level on the side open to the atmosphere is higher than the side connected to the gas sample, subtract the difference in height from the atmospheric pressure to find the gas pressure in mmHg.
2. To convert this pressure from mmHg to atmospheres (atm), divide the mmHg value by 760.0 (since 1 atm = 760 mmHg).
3. To convert to kilopascals (kPa), use the conversion factor that 1 atm is approximately equal to 101.325 kPa.

For sample (b), if the mercury level on the side connected to the gas sample is higher than the side open to the atmosphere, add the difference in height to the atmospheric pressure to find the gas pressure in mmHg, and then convert as needed.

Without the specific measurements from the manometer, the exact pressure of the gas sample cannot be provided.