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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P1A.12* Balloons are still used to deploy sensors that monitor meteorological phenomena and the chemistry of the atmosphere. It is possible to investigate some of the technicalities of ballooning by using the perfect gas law. Suppose your balloon has a radius of 3.0 m and that it is spherical. (a) What amount of H₂ (in moles) is needed to inflate it to 1.0 atm in an ambient temperature of 25 °C at sea level? (b) What mass can the balloon lift (the payload) at sea level, where the mass density of air is 1.22 kg m? (c) What would be the payload if He were used instead of H₂?
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?
ASK YOUR TEACHER A gas of unknown molar mass was allowed to effuse through a small opening under constant pressure conditions. It required 3650 s for 1.00 L of this gas to effuse. Under identical experimental conditions it required 471 s for 1.00 L of hydrogen (H2) gas to effuse. Calculate the molar mass of the unknown gas . (Remember that the faster the rate of effusion, the shorter the time required for effusion; that is, rate and time are inversely proportional.) a) The molar mass is 0.3 g/mol.b) The molar mass is 15.6 g/mol.c) The molar mass is 0.7 g/mol.d) The molar mass is 121.1 g/mol.e) The molar mass is 5.6 g/mol.
12
11) The temperature of a 9382 mL sample of Ne is changed, causing a change in pressure from 121.94 kPa to 175.82 kPa. If its new temperature is 849.71K and its new volume is 310.1 mL, what was the initial temperature in Kelvin? 12) A sample of O; at -38.62 °C experiences a change in volume from 3846.8 mL to 5820.5 mL. If its new pressure is 73634.12 torr at -164.3°C, what was the initial pressure in torr?
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(a) A piston at 1.5 atm contains a gas that occupies a volume of 3.5 L. What pressure would have to be placed on the piston to force the volume to adjust to 0.51 L? (b) A piston at 9.0°C contains a gas that occupies a volume of 2.5 L. To what temperature would the gas have to be heated to increase the volume to 7.5 L at constant pressure? (c) A piston at 4095 torr contains a gas that occupies a volume of 4.7 L. What pressure would have to be placed on the piston to force the volume to adjust to 1.34 L?
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.)
give the explanation of formula and calculations.
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.
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.

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