Air in human lungs has a temperature of 37.0°C and a saturation vapor density of 44.00 g/m3.   (a)If 1.700 L of air is exhaled and very dry air inhaled, what is the maximum loss of water vapor in grams by the person?    ____________g   (b)Calculate the partial pressure of water vapor having this density, and compare it with the vapor pressure of 6.31 ✕ 103 N/m2.    _________________N/m2

The vapor pressure of water at 5°C is 0.8726 kPa. Calculate the vapor pressure in atm.Round answer to 4 significant digits.

Two containers of equal volume each hold samples of the same ideal gas. Container A has 2 times as many molecules as container B. If the gas pressure is the same in the two containers, find the ratio of the the absolute temperatures TA and TB ( i.e  TA / TB  ) . Calculate to 2 decimals.

The partial pressure of carbon dioxide in the lungs is about 470 Pa when the total pressure in the lungs is 1.0 atm. What percentage of the air molecules in the lungs is carbon dioxide? Compare your result to the percentage of carbondioxide in the atmosphere, about 0.033%.

H.W: A mass flow rate m(g/s) is measured as a function of temperature T(°C). T 10 20 40 80 m 14.76 20.14 27.73 38.47 There is reason to believe that m varies linearly with the square root of T: m = aT/2 + b Use a straight-line plot to verify this formula and determine a and b.

The gauge pressure of a  50 L volume of gas is 4 atm and its initial temperature is 37 degree Celisus. What is the final gauge pressure when the temperature is 77 degrees Celsius and the volume is 20 L? Final gauge pressure is [x] _________ atm

The gas law for an ideal gas at absolute temperature T (in kelvins), pressure P (in atmospheres), and volume V (in liters) is PV = nRT, where n is the number of moles of the gas and R = 0.0821 is the gas constant. Suppose that, at a certain instant, P = 9.0 atm and is increasing at a rate of 0.15 atm/min and V = 13 L and is decreasing at a rate of 0.17 L/min. Find the rate of change of T with respect to time at that instant if n = 10 mol. (Round your answer to four decimal places.) dT=0.512 dt X K/min

The gas law for an ideal gas at absolute temperature T (in kelvins), pressure P (in atmospheres), and volume V (in liters) is PV = nRT, where n is the number of moles of the gas and R = 0.0821 is the gas constant. Suppose that, at a certain instant, P = 9.0 atm and is increasing at a rate of 0.15 atm/min and V = 13 L and is decreasing at a rate of 0.17 L/min. Find the rate of change of T with respect to time at that instant if n = 10 mol. (Round your answer to four decimal places.) K/min dT_ dt

What is the molar mass of a gas if 1.30g of the gas has a volume of 255 mL at STP? ( THE ANSWER IS NOT 130g/mol)

answer part b and c