A study of climbers who reached the summit of Mount Everest without supplemental oxygen showed that the partial pressures of O 2 and CO 2 in their lungs were 35 mm Mg and 7.5 mm Hg, respectively. The barometric pressure at the summit was 253 mm Hg. Assume the lung gases are saturated with moisture at a body temperature of 37 °C [which means the partial pressure of water vapor in the lungs is P (H 2 O) = 47.1 mm Hg]. If you assume the lung gases consist of only O 2 , N 2 , CO 2 , and H 2 O, what is the partial pressure of N 2 ?
A study of climbers who reached the summit of Mount Everest without supplemental oxygen showed that the partial pressures of O 2 and CO 2 in their lungs were 35 mm Mg and 7.5 mm Hg, respectively. The barometric pressure at the summit was 253 mm Hg. Assume the lung gases are saturated with moisture at a body temperature of 37 °C [which means the partial pressure of water vapor in the lungs is P (H 2 O) = 47.1 mm Hg]. If you assume the lung gases consist of only O 2 , N 2 , CO 2 , and H 2 O, what is the partial pressure of N 2 ?
Solution Summary: The author explains how the ideal gas equation can be obtained by combining Boyle's, Charles’s Law and Avogadro.
A study of climbers who reached the summit of Mount Everest without supplemental oxygen showed that the partial pressures of O2 and CO2 in their lungs were 35 mm Mg and 7.5 mm Hg, respectively. The barometric pressure at the summit was 253 mm Hg. Assume the lung gases are saturated with moisture at a body temperature of 37 °C [which means the partial pressure of water vapor in the lungs is P(H2O) = 47.1 mm Hg]. If you assume the lung gases consist of only O2, N2, CO2, and H2O, what is the partial pressure of N2?
A person's daily caloric requirement could be obtained from about 675 g of glucose, C 6 H 12 O 6 What volume (L) of oxygen gas at STP must be breathed to react with this much glucose? The balanced equation is given below . C 6 H 12 O 6 (s)+6O 2 (g) -> 6CO 2 (g)+6H 2 O(l)
A 5.50-mole sample of NH3 gas is kept in a 1.85-L container at 309 K. If the van der Waals equation is assumed to give the correct answer for the pressure of the gas, calculate the percent error made in using the ideal-gas equation to calculate the pressure. (Use a = 4.17 atm·L2·mol−2 and b = 0.0371 L·mol−1 for the van der Waals equation.)
The temperature of your water was 22.4 degrees Celsius. The volume of hydrogen collected was 35.3 mL. The atmospheric pressure in the lab room was 29.60 inches Hg. The difference in the water level between the beaker and the burette is 20.0 cm. What was the mass of the magnesium ribbon used?
Hint: 2 HCl(aq) + Mg(aq) = H2(g) + MgCl2(aq)
General, Organic, and Biological Chemistry - 4th edition
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