The average person takes 500mL of air into the lungs with each normal inhalation, which corresponds to aproximately 1x10^22 molecules of air. Calculate the number of molecules of air inhaled by a person with a respiratoy problem who takes in only 350mL of air with each breath. Assume constant pressure and temperature.
The average person takes 500mL of air into the lungs with each normal inhalation, which corresponds...
How many moles of air are in the lungs of a average person with a total lung capacity of 3.8 L? Assume that the person is at 1.0 atm pressure and has a normal body temperature of 37 C
1))))A person’s lungs might hold 6.0 x 10-3 m3 of air at body temperature (37 0C) and atmospheric pressure (101 kPa). Given that air is 21% oxygen (O2), find the number of O2 molecules in the lungs ans: 2.97 x 1022 2)) If the person takes a particularly deep breath, so that the lungs hold a total of 1.5 x 1023 molecules, what is the new volume of the lungs? [Answer: 6.35 x 10-3 m3 ]
A normal breath takes in about 1.0 L of air. Assuming that air has an average molar mass of 28.8 g, and that its density is 0.97 g/L. how many molecules of air do you take in with each breath? 2.0 times 10^22 2.2 x 10^22 5.8 times 10^23 1.7 times 10^25 1.8 times 10^25
A young male adult takes in about 5.80 x 10-4 m3 of fresh air during a normal breath. Fresh air contains approximately 21% oxygen. Assuming that the pressure in the lungs is 1.03 x 105 Pa and air is an ideal gas at a temperature of 310 K, find the number of oxygen molecules in a normal breath.
2. The air we breathe contains approximately 21.0 mol% oxygen. The average person breathes 0.50 L of air per breath a. If the atmospheric pressure is 745 mmHg, what is the partial pressure of oxygen in atmospheres? b. On a warm April day in Indiana, the air is 26.85 °C, how many moles of oxygen are inhaled in one breath? c. On top of Pikes Peak in Colorado, the temperature is -6.74 °C and the pressure is 442 mmHg. How...
answer asap please
A sealed balloon is filled with air at atmospheric pressure (P = 1.01 X 105 Pa) at 30°C (typical conditions for the surface of the Earth in St. Thomas). You take the (sealed) balloon with you on top of Mountain Top, which has an elevation of about 450m, where the average air pressure is 9.6 x 109 Pa. The temperature at the top is 26°C, a bit cooler. 2.5 pts. - a) How big is the balloon...
If you have ever hiked or climbed to high altitudes in the mountains, you surely have noticed how short of breath you get. This occurs because the air is thinner, so each breath contains fewer O2 molecules than at sea level. At the top o Mt. Everest, the pressure is only atm Air contains 21.0% O2 and 78.0% N2, and an average human breath is 0.450 L of air. For related problem-solving tips and strategies, you may want to view...
Please use simple equations from one of these concepts:
1.) combined gas law
2.)Boyle & Charles
3.) Ideal Gas Law
Please clearly display the equation used to find the answer.
Thank you.
QUESTION 9 Consider a gas with a volume of 15.0 mL at a temperature of 390 K. What is the temperature of the gas if the volume drops to 5.0 mL? QUESTION 10 Boyle's Law is helpful for understanding breathing, however it does not fully apply because as...
The next three questions all go together. 21. Expired air is saturated with water vapor and generally contains more of it than does inspired air. There is usually a net loss of water from the body due to breathing. Water vapor pressure in the at saturation in the lungs (at 37°C) is 47 mmHg, while in expired air at 33°C it is 37.7 mmHg. Consider the case of someone who is breathing dry air in and moist air out at...
9,10,11,12,13,14, and 15 please
a syringe is filled with 40. mL. of air at room temperature (22°C) in the lab and then this syringe is placed into a boiling water bath. After S minutes, the volume of gas in in the syringe (still at lab pressure) should be close to which volume? 9. Which of these is a true statement about a below a tube that is filled with a liquid such as mercury b. The weight of the liquid...