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A 3.00 L flask containing 2.0 mol of O2 and 1.0 mol of N2 is in...

A 3.00 L flask containing 2.0 mol of O2 and 1.0 mol of N2 is in a room that is at 22.0˚C.

a. What is the total pressure in the flask?

b. What fraction of the total pressure in the flask is due to N2?

c. If the temperature of the flask is lowered, what happens to the pressure inside the flask?

d. On a molecular level, explain why the pressure changes as you predicted in part (c).

e. If 1.0 mol of H2 is added to the flask, what happens to the total pressure? What happens to the partial pressure of N2?

f. If 1.0 L is added to the original flask from part (a), how would you expect the pressure in the flask to change?

g. Which gas, N2 or O2, would you expect to have greater solubility in water? In terms of intermolecular forces, explain your answer.

Please be very specific with all the answers and explain the reasons thoroughly.

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Answer #1

No ofmoles O2 presentin gassample, no, -2.0 mol Volume of the flask,?-3.00 L Temperature, T = 22.0 C+273 Gas constant, R - 0.0821 L.atm.K mol According to i deal gas equati on, PV nRT Parti al pressure of 02, -295 K RT 2.0 mol ×0.0821 L. atm. K-mol-x295 K 3.00 L 16.1 atm So, partial pressure of the oxygen (O2) gas is 16.1 atm No of moles N2 presentingassample, n,-1.0mol According to i deal gas equati on, PV nRT Partial pressure of N2,R- nRT 1.0 mol ×0.0821 L. atm·K-mol-x295 K 3.00 L - 8.1 atnm So, partial pressure of the nitrogen (N2) gas is 8.1atm. Partal pressure of the oxygen gas, Pa 16.1 atm Partal pressure of the nitrogen gas,D-8.1 atm Total pressure, Botal ? According to Daltons law of parti al pressures Total pressur 8.1 atm +16.1 atm -24.2 atm Therefore, total pressure in the flask is 24.2 atm

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