http://macmillanhighered.com/chemicalprinciples7e ning Given that the partial pr
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http://macmillanhighered.com/chemicalprinciples7e ning Given that the partial pressure of carbon dioxide in the tropo- blue sphere is 0.26 Torr and that the temperature is 25 °C, calculate neon the volume of air at 1.0 atm needed to produce 10.0 g of glucose. re of 3.4 Roommates fill ten balloons for a party, five with hydrogen and five with helium- After the party the hydrogen balloons have lost one-fifth of their hydrogen due to effusion through the walls of the balloons. What fraction of helium will the other balloons have lost at that same time? 3.5 Suppose that 200. mL of hydrogen chloride gas at 690. Torr and 20.C is dissolved in 100. mL of water. The solution is titrated to the stoichiometric point with 15.7 mL of a sodium hydroxide solution. What is the molar concentration of NaOH in the solu- ame ains on- r of ity ed; y? tion used for the titration? 3.6 When people dive into deep water, the pressure exerted by the water above can become great enough to collapse their lungs. Hence, scuba gear must sense the external pressure and increase the pres- sure of the breathing mixture provided to the diver until it equals the external pressure. A diver exploring a sunken ship uses an oxygen- enriched breathing mixture of 36% oxygen and 64% nitrogen by mass. At a depth of 33 ft, the pressure on the diver is 2.0 bar. What is al pressure of oxygen in the breathing mixture at that depth? 3.7 A flask of volume 5.00 L is evacuated and 43.78 g of solid dini- en tetroxide, N204, is introduced at-196 The sample is then e slowly ar warmed to 25 , during which time the N204 vaporizes and some ice of it dissociates to form brown NO, gas. The increases until it stabilizes at 2.96 atm. (a) Write a balanced equationExplanation / Answer
The basic concept which will help you to solve this problem in c) is,
N2O4 -----> 2NO2
mol of NO2 = 2 * mol of N2O4
in b) you should have calculated the pressure using the ideal gas law i.e) p = nRT/V
Note : You have remember that even after reaction the total pressure will remain the same
but the individual pressures vary with the progress in the reaction.
To calculate c) you should know that PN2O4 = XN2O4 * Ptotal ; PNO2 = XNO2*Ptotal
where PN2O4 and PNO2 are partial pressures of N2O4 and NO2 respectively.
While XN2O4 and XNO2 are partial pressures of N2O4 and NO2 .
Assume that total no of moles, nT = 1 and and Ptotal is the answer you got from b)
Since, PNO2 = nNO2 * Ptotal we can say that partial pressure of NO2 is directly
proportional to moles of NO2 , also you to remember that mol of NO2 = 2 * N2O4
So by clubbing these 2 highlighted statements you get the solution.
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