Chapter 5: Problem 11
If you release a helium balloon, it soars upward and eventually pops. Explain this behavior.
Chapter 5: Problem 11
If you release a helium balloon, it soars upward and eventually pops. Explain this behavior.
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Get started for freeThe total mass that can be lifted by a balloon is given by the difference between the mass of air displaced by the balloon and the mass of the gas inside the balloon. Consider a hot-air balloon that approximates a sphere \(5.00 \mathrm{~m}\) in diameter and contains air heated to \(65^{\circ} \mathrm{C}\). The surrounding air temperature is \(21^{\circ} \mathrm{C}\). The pressure in the balloon is equal to the atmospheric pressure, which is 745 torr. a. What total mass can the balloon lift? Assume that the average molar mass of air is \(29.0 \mathrm{~g} / \mathrm{mol}\). (Hint: Heated air is less dense than cool air.) b. If the balloon is filled with enough helium at \(21^{\circ} \mathrm{C}\) and 745 torr to achieve the same volume as in part a, what total mass can the balloon lift? c. What mass could the hot-air balloon in part a lift if it were on the ground in Denver, Colorado, where a typical atmospheric pressure is 630 . torr?
A mixture of chromium and zinc weighing \(0.362 \mathrm{~g}\) was reacted with an excess of hydrochloric acid. After all the metals in the mixture reacted, \(225 \mathrm{~mL}\) dry hydrogen gas was collected at \(27^{\circ} \mathrm{C}\) and 750 . torr. Determine the mass percent of \(\mathrm{Zn}\) in the metal sample. [Zinc reacts with hydrochloric acid to produce zinc chloride and hydrogen gas; chromium reacts with hydrochloric acid to produce chromium(III) chloride and hydrogen gas.]
Calculate the pressure exerted by \(0.5000 \mathrm{~mol} \mathrm{~N}_{2}\) in a \(10.000-\mathrm{L}\) container at \(25.0^{\circ} \mathrm{C}\) a. using the ideal gas law. b. using the van der Waals equation. c. Compare the results. d. Compare the results with those in Exercise 107 .
The partial pressure of \(\mathrm{CH}_{4}(g)\) is \(0.175\) atm and that of \(\mathrm{O}_{2}(g)\) is \(0.250\) atm in a mixture of the two gases. a. What is the mole fraction of each gas in the mixture? b. If the mixture occupies a volume of \(10.5 \mathrm{~L}\) at \(65^{\circ} \mathrm{C}\), calculate the total number of moles of gas in the mixture. c. Calculate the number of grams of each gas in the mixture.
A spherical glass container of unknown volume contains helium gas at \(25^{\circ} \mathrm{C}\) and \(1.960 \mathrm{~atm}\). When a portion of the helium is withdrawn and adjusted to \(1.00\) atm at \(25^{\circ} \mathrm{C}\), it is found to have a volume of \(1.75 \mathrm{~cm}^{3}\). The gas remaining in the first container shows a pressure of \(1.710\) atm. Calculate the volume of the spherical container.
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