The density of mercury is 13.5 g/mL and the density of water is 1.00 g/mL.If a mercury barometer reads 761 mmHg, what is the barometric pressure in cmH₂O?Hint: From physics we find that the pressure is related to the height according to the equationP = dghwhere d = density, g=gravitational acceleration and h is the height.Now, if we have two devices at the same pressure we can say thatP = dighi= d₂gh2Use this equation, your algebra skills and your logic to see how tall a water barometer would be!

Let's start by using the equation P = dgh to find the height of the water barometer. We know the…

Answered: The density of mercury is 13.5 g/mL and…

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...

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For many purposes we can treat nitrogen (N₂) as an ideal gas at temperatures above its boiling point of −196. °C. Suppose the temperature of a sample of nitrogen gas is lowered from 14.0 °C to -10.0 °C, and at the same time the pressure is changed. If the initial pressure was 2.0 atm and the volume decreased by 55.0%, what is the final pressure? Round your answer to the correct number of significant digits. at atm x10 X ? 00. 18 Ar
Water can be decomposed by electrolysis to hydrogen gas and oxygen gas. If 2.33 g of water is decomposed to H2(g) and O2(g) and the gases are collected in a 1.00 L flask over water at 25°C (vapor pressure H2O(l) = 23.8 mm Hg), what is the pressure in the flask?
A scuba diver’s tank contains 0.30 kg oxygen (O2) compressed into a volume of 2.32 L.(a) Use the ideal gas law to estimate the gas pressure inside the tank at 5°C, and express it in atmospheres and in pounds per square inch.(b) What volume would this oxygen occupy at 30°C and a pressure of 0.98 atm?
For many purposes we can treat ammonia NH3 as an ideal gas at temperatures above its boiling point of −33.°C. Suppose the temperature of a sample of ammonia gas is raised from −12.0°C to 21.0°C, and at the same time the pressure is changed. If the initial pressure was 2.5atmand the volume decreased by 45.0%, what is the final pressure? Round your answer to the correct number of significant digits. atm
For many purposes we can treat ammonia (NH3) as an ideal gas at temperatures above its boiling point of – 33. °C. Suppose the pressure on a 830. mL sample of ammonia gas at 11.0°C is cut in half. Is it possible to change the temperature of the ammonia at the same time such that the volume of the gas doesn't change? If you answered yes, calculate the new temperature of the gas. Round your answer to the nearest °C. yes no °C x10 X 3
5.69 You want to store 165 g of CO2 gas in a 12.5-L tank at room temperature (25°C). Calculate the pressure the gas would have using (a) the ideal gas law and (b) the van der Waals equation. (For CO2, a = 3.59 atm L^2/mol^2 and b = 0.0427 L/mol.)
For many purposes we can treat ammonia NH3 as an ideal gas at temperatures above its boiling point of −33.°C. Suppose the temperature of a sample of ammonia gas is lowered from 23.0°C⁢ to −19.0°C, and at the same time the pressure is changed. If the initial pressure was 6.3atm and the volume increased by 55.0%, what is the final pressure? Round your answer to the correct number of significant digits.
11. (a) In a 20.0 L steel container, we have only 77.7 g of CO2(g), 66.6 g of N2(g), and O2(g). The temperature is 25.0 ◦C and the total pressure is 8.88 atm. What mass of O2(g) do we have, and what is its partial pressure? The molar masses of C, N, and O are 12.01, 14.01, and 16.00 g/mol. (b) The density of a sample of pure CH4(g) at a constant pressure of 1.00 atm is 0.666 g/L. What is the average speed, or root mean square speed, of the CH4(g) molecules in this sample? The molar masses of C and H are 12.01 and 1.01 g/mol.
For many purposes we can treat ammonia (NH,) as an ideal gas at temperatures above its boiling point of –33. °C. Suppose the temperature of a sample of ammonia gas is raised from – 25.0 °C to 17.0 °C, and at the same time the pressure is changed. If the initial pressure was 0.15 kPa and the volume decreased by 50.0%, what is the final pressure? Round your answer to 2 significant digits. kPa 1 Don't Know Submit etv DII esc %23 24 6 7 09 2 4 OP E T Y.
A balloon can be stretched to a maximum radius of 10.5 cm. The balloon is filled with 3.0 L of helium gas at a pressure of 755 torr and a temperature of 298 K. The balloon is then allowed to rise. If the balloon bursts at an atmospheric pressure of 431 mmHg, what must the temperaturehave been at that point? The formula for the volume of a sphere is V = 4/3πr3.
Hydrogen initially occupies 176 liters. If it changes to a volume of 84 liters at 0 degrees Celsius and 760 mm Hg. If the initial temperature of the hydrogen was 23 degrees celsius, what was its initial pressure of gas in mm Hg?
A sample of 328.1 mL of wet nitrogen gas was collected over water at a total pressure of 761 torr and a temperature of 21.0 °C. (The vapor pressure of water at 21.0 °C is 18.7 torr.) The nitrogen was produced by the reaction of sulfamic acid, HNH2SO3, with 404.3 mL of a solution of sodium nitrite according to the following equation. NANO2 + HNH2SO3¬ N2 + NaHSO4 + H2O Calculate what must have been the molar concentration of the sodium nitrite.

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