Experiments carried out by French chemists Jacques Alexandre César Charles and Joseph-Louis Gay-Lussac and British physicist Lord Kelvin determined a quantitative relationship between the volume and temperature of a gas. Their data showed that for a container of gas held at constant pressure, the volume and temperature are directly proportional. For example, if you inflate a balloon outdoors with cold air on a cold day and then take it inside, it will expand, and it might even burst. This happens because as the temperature of the air inside the balloon increases, the volume of the balloon increases as well. What is less obvious is the quantitative relation: If the pressure is held constant, then when the temperature is doubled, the volume is doubled as well. Part A According to Charles's law, for a fixed quantity of gas at constant pressure, which the given quantities is constant? ▸ View Available Hint(s) O O VxT O V +T Submit Part B A balloon was filled to a volume of 2.50 L when the temperature was 30.0°C. What would the volume become if the temperature dropped to 11.0°C. Express your answer with the appropriate units. ▸ View Available Hint(s) Value Submit μÀ Part C → C Units ? Refrigerators are usually kept at about 5°C, while room temperature is about 20°C. If you were to take an "empty" sealed 2-liter soda bottle room temperature and place it in the fridge, would you expect it to contract to one-fourth its original volume? O Yes, because 5 is one-fourth of 20. O No, because there is no gas inside the bottle. O No, because Celsius is not an absolute temperature scale.

A helium-filled weather balloon has a volume of 687 L at 21.9°C and 757 mmHg. It is released and rises to an altitude of 2.61 km, where the pressure is 614 mmHg and the temperature is 4.9°C. The volume of the balloon at this altitude is    ?      L.

A sample of gas contains 0.1700 mol of CH4(g) and 0.1700 mol of H2O(g) and occupies a volume of 19.2 L. The following reaction takes place:CH4(g) + H2O(g)3H2(g) + CO(g)Calculate the volume of the sample after the reaction takes place, assuming that the temperature and the pressure remain constant.

2.00 liter of nitrogen at 26.35 torr is mixed with 2.00 liter of helium at 42.45 torr and a third gas, oxygen. Together, the three gases exert a pressure of 1,245.32 torr in a 2.00 liter container. What is the pressure of the oxygen gas in torr? (Answer to two decimal places and no units in your answer please.)

In an air-conditioned room at 21.0 ∘C, a spherical bubble had the diameter of 60.0 cm. When taken outside on a hot summer day, the bubble expanded to 61.0 cm in diameter. What was the temperature outside in degrees Celsius? Assume that the bubble is a perfect sphere and that the pressure and number of moles of air molecules remains the same.

Two students perfomed an experiment on the decomposition of hydrogen peroxide. One student was in Wisconsin where the atmospheric pressure was 0.996 atm. The other was in Colorado, where the atmospheric pressure was 0.832 atm. Both reactions were performed at the same temperature and produced the same number of moles of oxygen gas. How do the volumes of gases collected compare? Are they the same or not? Explain.

The total energy of two colliding gas molecules is conserved because the Group of answer choices collision is inelastic. collision is elastic. collision intensity varies as temperature changes. collision occurs too rapidly for energy to be lost.

Match the characteristic of gases described below to the postulates of the kinetic molecular theory that best explain that characteristic. (Note: You may need to list more than one postulate.) The pressure of a gas in a fixed volume increases when its temperature increases. Select one or more: The average kinetic energies of gas particles increase with an increase in temperature. Gas particles are widely spaced. A gas consists of many small particles in rapid, random motion. The total volume of the molecules themselves is very small compared to the volume of the container. There are virtually no attractive forces between gas particles.

What happens to the average kinetic energy of gas when the particles of the gas collide against each other at a constant temperature and volume? Explain

The average kinetic energy of the molecules in a gas sample depends only on the temperature T. R=8.314. What is the rms speed 02 molecules at 443 K? What is the rms speed of He atoms at 443 K?