**Measuring Gas Pressure Using an Open-End Mercury Manometer****Problem Statement:**The pressure of a sample of gas is measured at sea level with an open-end mercury manometer. Assuming atmospheric pressure is 684.73 mm Hg, determine the pressure of the gas if h = 18.24 cm. (Provide your answer in mmHg - but do not include units in your answer).**Diagram Description:**The diagram shows an open-end mercury manometer used to measure the pressure of a gas. The setup consists of the following parts:- A gas container connected to a manometer.- The manometer is a U-shaped tube partially filled with mercury.- One end of the manometer is exposed to the gas (labeled "Gas"), and the other end is open to the atmosphere (labeled "Open end").- The height difference of the mercury column between the two arms of the U-tube is marked as \( h \). In this case, \( h \) is given as 18.24 cm.**Calculation Explanation:**To determine the pressure of the gas, you can use the following steps:1. **Convert \( h \) to mm Hg**: Since \( h \) is given in centimeters (cm), convert it to millimeters (mm) because the pressure is asked to be in mm Hg. \[ h = 18.24 \, \text{cm} = 182.4 \, \text{mm} \]2. **Determine the type of manometer reading**: - If the mercury level in the arm open to the atmosphere is higher, the pressure of the gas is lower than atmospheric pressure. - If the mercury level in the gas-connected arm is higher, the pressure of the gas is higher than atmospheric pressure.3. **Calculate the Gas Pressure**: - In this diagram, it is assumed that the mercury level is higher on the open end side (which means the gas pressure is higher than the atmospheric pressure). \[ P_{\text{gas}} = P_{\text{atm}} + h = 684.73 \, \text{mmHg} + 182.4 \, \text{mmHg} \]4. **Result**: \[ P_{\text{gas}} = 867.13 \, \text{mmHg} \]Thus, the pressure of the gas

Answered: Image /qna-images/answer/97f47eb0-e1df-4eaf-a9a5-afba5d7c598c.jpg

The pressure of a sample of gas is measured at sea level with an open-end mercury manometer. Assuming atmospheric pressure is 684.73 mm Hg, determine the pressure of the gas if h = 18.24 cm. (answer in mmHg - but do not include units in your answer)

The pressure of a sample of gas is measured at sea level with an open-end mercury manometer. Assuming atmospheric pressure is 684.73 mm Hg, determine the pressure of the gas if h = 18.24 cm. (answer in mmHg - but do not include units in your answer)

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

7.) A glass bulb contains an unknown gas. The gas is either CO2, SO2, C2H6, or CH3F. Here is some data that was collected for this gas sample. Use the data to identify the unknown gas. Mass of glass bulb with the unknown gas: 14.402 g Volume of glass bulb: 670. mL Mass empty bulb 12.232 g Pressure 1751. torr Temperature 21.oC
A sample of a gas at room temperature occupies a volume of 16.0 L at a pressure of 442 torr . If the pressure changes to 2210 torr , with no change in the temperature or moles of gas, what is the new volume, V2? Express your answer with the appropriate units.
2. A gas sample collected at 35.0°C and a pressure of 710 torr has a volume of 200 mL. The temperature and pressure are changed, and the gas is compressed to 150 mL. The new temperature is 40.0°C; what is the new pressure? Use the combined gas law for this problem.
A helium-filled weather balloon has a volume of 683 L at 22.9°C and 755 mmHg. It is released and rises to an altitude of 5.47 km, where the pressure is 457 mmHg and the temperature is –13.1°C. The volume of the balloon at this altitude is _____ L.
A sample of gas has a mass of 38.8 mg. Its volume is 228 mL at a temperature of 56 ∘C and a pressure of 896 torr. Find the molar mass of the gas
A balloon is partly inflated with 4.50 liters of helium at sea level where the atmospheric pressure is 992 mbar. The balloon ascends to an altitude of 3.00× 103 meters, where the pressure is 853 mbar. What is the volume of the helium in the balloon at the higher altitude? Assume that the temperature of the gas in the balloon does not change in the ascent. L
ompleted 8 out of 18 stion 17 of 18 O Macmillan Learning > Introductory Chemistry Revell SECOND EDITION Resources amount of oxygen: Submit All presented by Macmillan Learning Imagine you are sitting in a room with a volume of 27000 liters and a temperature of 69 °F. The total air pressure is 784 mm Hg, and the partial pressure from oxygen is 21% of the total pressure. How many grams oxygen are in the room? grams
A sample of gas has a mass of 38.6 mg. Its volume is 226 mL at a temperature of 55 ∘C and a pressure of 896 torr. Find the molar mass of the gas.
A.) What is the temperature of 0.45 mol of gas at a pressure of 1.0 atm and a volume of 12.0 L ? Express the temperature in kelvins to two significant figures. B.) A weather balloon is inflated to a volume of 25.9 L at a pressure of 752 mmHg and a temperature of 27.5∘C. The balloon rises in the atmosphere to an altitude where the pressure is 400. mmHg and the temperature is -15.3∘C. Assuming the balloon can freely expand, calculate the volume of the balloon at this altitude.
The typical human lung has a volume when full of approximately 5.0 L. The partial pressure of oxygen in the atmosphere is 160 mm Hg (1 atm = 760 atm). How many moles of oxygen are in the typical human lung when full? (You can assume the air in the lungs is at a normal human body temperature of 37oC.)
A sample of gas has a mass of 0.565 g g . Its volume is 115 mL mL at a temperature of 86 ∘C ∘C and a pressure of 755 Torr Torr . Find the molar mass of the gas. Use the molar volume of a gas at STP to determine the volume (in LL) occupied by 19.8 g g of neon at STP.
A weather ballon is inflated to a volume of 67.0 L at a pressure of 748 mm Hg and a temperature of 28.0 celsius. The balloon rises where the pressure is 385 mm Hg and the temperature is 15.0 celsius. Assuming the balloon can freely expand, calculate the volume of the balloon in liters.