8. Since pressure and temperature are directly proportional, their ratio gives a constant number (provided that volume and number of molecules are kept the same). So P1T1=a constant = P2/T2. It doesn't really matter what the constant is. As long as volume and the number of molecules remains constant: P1/T1 = P2/T2. This is only true when a Kelvin temperature scale is used. This is not true in the Celsius scale (or any other temperature scale). %3D If a sample of gas occupying some volume has a pressure of 1.53 atm at 298 K, what is the pressure at 310. K? 9. If a sample of gas occupying some volume has a pressure of 1.5 atm at 25 °C, what is the pressure at 50. °C?

8. Since pressure and temperature are directly proportional, their ratio gives a constant number (provided that volume and number of molecules are kept the same). So P1T1=a constant = P2/T2. It doesn't really matter what the constant is. As long as volume and the number of molecules remains constant: P1/T1 = P2/T2. This is only true when a Kelvin temperature scale is used. This is not true in the Celsius scale (or any other temperature scale). %3D If a sample of gas occupying some volume has a pressure of 1.53 atm at 298 K, what is the pressure at 310. K? 9. If a sample of gas occupying some volume has a pressure of 1.5 atm at 25 °C, what is the pressure at 50. °C?

Introductory Chemistry: A Foundation

8th Edition

ISBN:9781285199030

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter13: Gases

Section: Chapter Questions

Problem 114AP

See similar textbooks

Similar questions

You have a gas, one of the three known phosphorus-fluorine compounds (PF3, PF3, and P2F4). To find out which, you have decided to measure its molar mass. (a) First, yon determine that the density of the gas is 5.60 g/L at a pressure of 0.971 atm and a temperature of 18.2 C. Calculate the molar mass and identify the compound. (b) To check the results from part (a), you decide to measure the molar mass based on the relative rales of effusion of the unknown gas and CO2. You find that CO2 effuses at a rate of 0.050 mol/min, whereas the unknown phosphorus fluoride effuses at a rate of 0.028 mol/min. Calculate the molar mass of the unknown gas based on these results.
A balloon filled with helium gas is found to take 6 hours to deflate to 50% of its original volume. How long will it take for an identical balloon filled with the same volume of hydrogen gas (instead of helium) to decrease its volume by 50%?
Helium-filled balloons rise in the air because the density of helium is less than the density of air. (a) If air has an average molar mass of 29.0 g/mol, what is the density of air at 25C and 770 mm Hg? (b) What is the density of helium at the same temperature and pressure? (c) Would a balloon filled with carbon dioxide at the same temperature and pressure rise?
Explain why the numbers of molecules are not identical in the left- and tight-hand bulbs shown in the center illustration of Figure 9.27.
109 An ore sample with a mass of 670 kg contains 27.7% magnesium carbonate, MgCO3. If all of the magnesium carbonate in this ore sample is decomposed to form carbon dioxide, describe how to determine what volume of CO2 is evolved during the process. What would have to be measured to predict the needed volume in advance?