A balloon that is filled with gas was released at ground level. At ground level where the pressure was 790.0 mmHg and the temperature was 17.0 °C the balloon had a volume of 55.0 L. As the balloon floated higher in the atmosphere, it reached an altitude where the pressure and temperature were 170.0 mmHg and 1.00 °C, respectively. Determine the volume (in L) of the balloon at this new altitude. Volume: L

A balloon that is filled with gas was released at ground level. At ground level where the pressure was 790.0 mmHg and the temperature was 17.0 °C the balloon had a volume of 55.0 L. As the balloon floated higher in the atmosphere, it reached an altitude where the pressure and temperature were 170.0 mmHg and 1.00 °C, respectively. Determine the volume (in L) of the balloon at this new altitude. Volume: L

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

A balloon at sea level (1.0 atm) contains 15 L of air. If the balloon is taken to Denver, where the air pressure is 0.85 atm, what will the new volume (in L) of the new balloon be?
A 22.4 L sample of a gas is heated from 15 °C to 78 °C. What volume (mL) does the gas occupy at the higher temperature if the pressure remains constant? O 2.7 x 104 mL O 27 mL O 1.8 x 10 mL 1.2 x 105 mL
A 1.20 L weather balloon on the ground has a temperature of 25.0°C and is at atmospheric pressure (1.00 atm). When it rises to an elevation where the pressure is 0.710 atm, then the new volume is 1.80 L. What is the temperature (in °C) of the air at this elevation?
Boron trifluoride gas is collected at 6.0 °C in an evacuated flask with a measured volume of 15.0 L. When all the gas has been collected, the pressure in the flask is measured to be 0.140 atm . Calculate the mass and number of moles of boron trifluoride gas that were collected. Be sure your answer has the correct number of significant digits. mass: g x10 mole: | mol ?
A 1.20 L weather balloon on the ground has a temperature of 25.0°C and is at atmospheric pressure (1.00 atm). When it rises to an elevation where the pressure is 0.740 atm, then the new volume is 1.80 L. What is the temperature (in °C) of the air at this elevation?
An experimenter had a gas container that could change its volume. Several times, after setting the container to different volumes and letting the temperature reach room temperature, he measured the pressure at each different volume. Sketch what a graph of volume vs. pressure would look like.
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 an initial volume of 13.8 L at a pressure of 1.35 atm. If the sample is compressed to a volume of 10.3 L, what is its pressure? Express the pressure in atmospheres to three significant figures.
SF6 can be synthesized by the reaction: SO2(g) + 3 F2(g) → SF6(g) + O2(g)A 1.25-L reaction vessel, initially at 26°C, contains sulfur dioxide gas at a partial pressure of 184 mmHg and fluorine gas at a partial pressure of 511 mmHg. Identify the limiting reactant and determine the theoretical yield of SF6 in grams.
Hydrogen gas is produced when magnesium metal reacts with hydrochloric acid. In the lab, a student collects 0.002581 g of hydrogen gas over water in a eudiometer at 23°C. The atmospheric pressure is 794 mmHg. What volume (in mL) of dry hydrogen gas would be collected? Water Vapor Temperature °C Pressure (mmHg) 19 16.5 21 18.7 Volume of dry gas = mL 23 21.1 25 23.8 27 26.7 29 30.0
A 8.350 L sample of gas is cooled from 81.50°C to a temperature at which its volume is 6.950 L. What is this new temperature? Assume no change in pressure of the gas.