Baseball reporters say that long fly balls that would havecarried for home runs in July “die” in the cool air of October and are caught. The idea behind this observation isthat a baseball carries better when the air is less dense. Dryair is a mixture of gases with an effective molar mass of29.0 g mol-1 .(a) Compute the density of dry air on a July day when the     temperature is 95.0°F and the pressure is 1.00 atm.(b) Compute the density of dry air on an October evening     when the temperature is 50.0°F and the pressure is     1.00 atm.(c) Suppose that the humidity on the July day is 100%;     thus, the air is saturated with water vapor. Is the density     of this hot, moist air less than, equal to, or greater than     the density of the hot, dry air computed in part (a)? In     other terms, does high humidity favor the home run?

The flame produced by the burner of a gas (propane) grill is a pale blue color when enough air mixes with the propane (C3H8) to burn it completely. For every gram of propane that flows through the burner, what volume of air is needed to burn it completely? Assume that the temperature of the burner is 200.0°C, the pressure is 1.20 atm, and the mole fraction of O2 in air is 0.210.

The flame produced by the burner of a gas (propane) grill is a pale blue color when enough air mixes with the propane (C3H8) to burn it completely. For every gram of propane that flows through the burner, what volume of air is needed to burn it completely? Assume that the temperature of the burner is 205.0°C, the pressure is 1.25 atm, and the mole fraction of O2 in air is 0.210.

A sample of 263.0 mL of wet nitrogen gas was collected over water at a total pressure of 756 torr and a temperature of 21.0 °C. (The vapor pressure of water at 21.0 °C is 18.7 torr.) The nitrogen was produced by the reaction of sulfamic acid, HNH,SO3, with 368.5 mL of a solution of sodium nitrite according to the following equation. NaNO2 + HNH2SO3- N2 + NaHSO4 + H2O Calculate what must have been the molar concentration of the sodium nitrite. M

The van der Waals constants a and b are 5.489 L2 atm mole-1 and 0.0638 L mole-1 for C2H6. (a) Calculate the pressure (atm) of a 10.0 mole sample of C2H6 in a 4.86 L flask at 300.0 K. (b) Compare this value if the pressure is calculated under ideal conditions. Does this show a positive or a negative deviation from ideal gas behavior?

(a) (c) A column of water in a buret is 336 mm Hg high. How high would that column be if it were mercury instead of water? (d) In order for the pressures to be equal, density and height of a column are inversely proportional, therefore the following relationship applies: (denHg)(hHg) = (denH20)(hH20) Note: the density of mercury is 13.6 g/mL and the density of water is 1.00 g/mL. An electrolysis experiment was run for 15 minutes and 45 seconds at an average current of 189 milliamps (mA). The mass lost by the copper anode was 0.0589 grams. (b) Calculate the number of coulombs transferred. (Remember: coulomb = amps x sec) Show full calculation of the height in mercury (remember to use proper significant figures.) Calculate the moles of copper lost from the anode. Based on the moles of copper lost determined in 1c, calculate the moles of electrons transferred. Remember, the reaction at the copper anode is: Cu(s)---> Cu¹² (aq) + 2 e

A mixture of gaseous disulfur difluoride, dinitrogen tetra-fluoride, and sulfur tetrafluoride is placed in an effusion appara-tus. (a) Rank the gases in order of increasing effusion rate.(b) Find the ratio of effusion rates of disulfur difluoride and dini-trogen tetrafluoride. (c) If gas X is added, and it effuses at 0.935 times the rate of sulfur tetrafluoride, find the molar mass of X

(a) A piston at 5.7 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 1.54 L? atm(b) A piston at 63.0°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 4.1 L at constant pressure? °C(c) A piston at 7395 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 1.69 L? atm

What pressure permits 25.0 cm3 of neon at 735 mmHg to expand to a volume of 40.0 cm3?

An “empty" spray can contains residual propellant gas that has a pressure of 772 torr at 23°C. The can is then heated to 475 °C. (a) What is the gas pressure in the hot can if the volume remains constant? (b) What is the gas pressure in the hot can if the can slightly expands during heating and its volume increases by 6.50%?