Interpretation:
The ratios of diffusion of
Concept introduction:
The mutual diffusion constant involves the three mean free paths, that is, between like gas particles and between the different gas particles. The mutual diffusion constant is given by,
Where,
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The mutual diffusion constant does not depend on the mole fractions of the involved gases.
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Chapter 19 Solutions
Physical Chemistry
- Exhaled air contains 74.5% N2, 15.7% O2, 3.6% CO2, and 6.2% H2O (mole percent). (a) Calculate the molar mass of exhaled air. (b) Calculate the density of exhaled air at 37C and 757 mm Hg and compare the value you obtained with that of ordinary air (MM=29.0g/mol) under the same conditions.arrow_forwardIn the discussion on the composition of air, mention is made of the fact that water vapor may have a concentration as high as 40,000 ppm. Calculate the partial pressure exerted by water vapor at this concentration. Assume that this represents a situation with 100% humidity. What temperature would be needed to achieve this value? (See Appendix G.)arrow_forwardAt the critical point for carbon dioxide, the substance is very far from being an ideal gas. Prove this statement by calculating the density of an ideal gas in g/cm3 at the conditions of the critical point and comparing it with the experimental value. Compute the experimental value from the fact that a mole of CO2 at its critical point occupies 94 cm3.arrow_forward
- A cylinder of compressed gas is labeled Composition (mole %): 4.5% H2S, 3.0% CO2, balance N2. The pressure gauge attached to the cylinder reads 46 atm. Calculate the partial pressure of each gas, in atmospheres, in the cylinder.arrow_forwardScottish physicist W. J. M. Rankine proposed an absolute temperature scale based on the Fahrenheit degree, now called degree Rankine abbreviated R and used by some engineering fields. If a degree Rankine is 5/9 of a degree Kelvin, what is the value of the ideal gas law constant in L. atm/mol. R?arrow_forwardBriefly define Amagat’s Law and Dalton’s law for mixtures. Explain which of these laws best approximates real gas behaviourarrow_forward
- A student performed the experiment described in this module, using 5.00 mL of a 3.2% H2O2 solution with a density of 1.52 g mL-1. The water temperature was 18 ° C, and the barometric pressure in the laboratory was 30.1 in. Hg. After the student immersed the yeast in the peroxide solution, she collected 85.3 mL of O2. (4) Calculate the water temperature, in Celsius, to kelvins.arrow_forwardNitrogen oxide is a pollutant commonly found in smokestack emissions. One way to remove it is to react it with ammonia. 4 NH3(g) + 6 NO(g) → 5 N2(g) + 6 H2O(l) How many liters of ammonia are required to react with 13.1 L NO? Assume standard temperature and pressure. I am not sure how to solve this problem. I am assuming i use pv=nrt?arrow_forwardThe mole fraction of He in a He/Ne mixture at 300 K is 0.40. If the total pressure is 1.2 atm, determine the value of ZNe-He. Use rHe = 0.13 nm, rNe = 0.14 nm, MHe = 4 amu, and MNe = 20.18 amu. Use units of the International System. Use up to a maximum of 3 significant figures in the answer, DO NOT include units. Use the following notation: 6.02e23 if your answer is 6.02 x 1023 or 6.63e-34 if your answer is 6.63 x 10−34. Note that there are NO spaces between any digits of the answer.arrow_forward
- In an experiment as described in the Principles section, 158 mL of O2 is collected over water. The mass of the O2 is measured to be 0.207 g, the temperature is 290 K and the barometric pressure that day is 754 mm Hg. Calculate the value of R in the units L, atm, K, mol, showing those units clearly with your calculated value. Remember the correct pressure of O2 for the vapor pressure of water.arrow_forwardAt 298 K, N2(g) + 3H2(g) ⇄ 2NH3(g) K = 5.8 x 105At 298 K, NH3(g) ⇄ 1/2N2(g) + 3/2H2(g) K = 1.3 x 10⁻3 Is NH3 favorably formed at 298 K? Explain your answer.arrow_forward
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